The equilibrium constant (Kc) at 800 K is 4.86 × 10³
What is the equilibrium constant?The equilibrium constant expression for the given reaction is:
Kc = [SO3]^2 / ([SO2]^2 [O2])
where;
[SO3], [SO2], and [O2] represent the equilibrium concentrations of sulphur trioxide, sulphur dioxide, and oxygen, respectively.Substituting the given equilibrium concentrations in the expression, we get:
Kc = (5.0×10^-2)^2 / ((3.0×10^-3)^2 × 3.5×10^-3)
Kc = 4.86 × 10³ (rounded to 3 significant figures)
Therefore, the equilibrium constant (Kc) at 800 K is 4.86 × 10³
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[tex] \:\:\:\:\:\:\star[/tex]The equilibrium constant, Kc can be deduced for a reversible reaction by using the following expression:
[tex] \:\:\:\:\:\:\star\longrightarrow\sf \underline{Kc = \dfrac{\bigg[Products\bigg ]}{\bigg[Reactants \bigg]}}\\[/tex]
For a reaction [tex]\boxed{\sf xP+yQ=zPQ}[/tex] the equilibrium constant Kc is defined as [tex]\sf[PQ]^z/[P]^x[Q]^y[/tex].Where brackets denote reagent concentrations (in molarity) of each substance that must be given in order to compute the equilibrium constant Kc and each concentration term is raised to the power of its coefficient in the balanced chemical equation.Now for solving this problem we may write the equilibrium expression for the reaction system.
[tex] \:\star\:\sf2\:SO_2\:(g)\:+O_2\:(g)\:⇌2\:SO_3\:(g)\:\\[/tex]
The equilibrium constant expression for the given reaction is:
[tex] \:\:\:\:\:\:\star\longrightarrow \sf \underline{Kc = \dfrac{\bigg[SO_3\bigg]^2 }{ \bigg[SO_2\bigg]^2\:\bigg [O_2\bigg]}....Eq}\\[/tex]
As per question, following concentrations are present in the system is given -
[tex] \sf{[SO_3] = 5.0×10^{−2}\:M}[/tex][tex]\sf{ [O_2] =3.5×10^{−3 }\:M}[/tex][tex] \sf{[SO_2]=3.0×10^{−3}\: M}[/tex]Now that, we have all the required molar equilibrium concentrations, so we can substitute the molar equilibrium concentrations into the equation and calculate the value of Kc:-[tex] \:\:\:\:\:\:\star\longrightarrow \sf \underline{ Kc = \dfrac{\bigg[SO_3\bigg]^2 }{ \bigg[SO_2\bigg]^2\:\bigg [O_2\bigg]}}\\[/tex]
[tex] \:\:\:\:\:\:\longrightarrow \sf Kc = \dfrac{\bigg[5\times 10^{-2}\bigg]^2 }{ \bigg[3\times10^{-3}\bigg]^2\:\bigg [3\times10^{-3}\bigg]}\\[/tex]
[tex] \:\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf Kc = \dfrac{25\times 10^{-4}}{9\times 10^{-6}\times3.5\times 10^{-3}}\\[/tex]
[tex] \:\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf Kc=\dfrac{25}{9\times3.5}\times 10^{-4}\times10^{3}\times10^{6}\\[/tex]
[tex] \:\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf Kc=\dfrac{25}{31.5}\times 10^{-4+3+6}\\[/tex]
[tex] \:\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf Kc=\cancel{\dfrac{25}{31.5}}\times 10^{5}\\[/tex]
[tex] \:\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf Kc= 0.793650......\times 10^{5}\\[/tex]
[tex] \:\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf \underline{Kc= 7.9365\times 10^{4}}\\[/tex]
Therefore,the equilibrium constant (Kc) at 800 K is [tex]\bf\underline{ 7.9365\times 10^{4}.}\\[/tex]
What is the pressure exerted by a .50 mol sample of N₂ gas in a 10.0L container
at 298K?
The pressure exerted by the nitrogen gas in the container of volume 10.0L at a temperature of 298K is 12.14 atm.
What is pressure in chemistry?Pressure in chemistry is defined as the force per unit area exerted by a gas on the walls of its container. It is the result of the constant, random motion of gas molecules colliding with the walls of the container.
To find the pressure exerted by the N₂ gas, we can use the ideal gas law:
PV = n*R*T
R is the universal gas constant, whose value is constant and is given by 0.0821 L·atm/mol·K
To solve for P:
P = n*R*T/V
Substituting the given values, we get:
P = (0.50 mol) * (298 K) / (10.0 L)* (0.0821 L·atm/mol·K)
P = 12.14 atm
Therefore, the pressure exerted by the N₂ gas in the 10.0L container at 298K is 12.14 atm.
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What does volume measure?
A. The space a substance takes up
B. The amount of energy in a substance
C. The phase of matter of a substance
D. The amount of matter (particles) in a substance
Volume is the measure of the space a substance takes up, hence the correct option is A.
Various types of measurementsNominal, ordinal, interval, and ratio measurements are the four main types of measurement.
An object or event's attributes are quantified through measurement so that they can be compared to those of other things or events. In other words, measurement is the process of comparing a physical quantity to a fundamental reference quantity of the same kind to determine how big or small it is.
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Use equivalent weights to calculate 81.00 mg/L calcium carbonate (CaCO3) in terms of mg/L as dihydrogen phosphate (H2PO4-)
According to the question Therefore, 81.00 mg/L CaCO3 is equivalent to 162.00 mg/L H2PO4-.
What is CaCO3 ?Calcium Carbonate, also known as CaCO3, is a naturally occurring mineral which is found in rocks, shells, and pearls. It is composed of the elements calcium, carbon, and oxygen, and is a major component of sedimentary rocks. Calcium Carbonate is an important building material, and is used in a range of industries, from paper and plastic to pharmaceuticals and cement. It is also used as an additive in many food products, such as baking powder and cheese.
To calculate this, we must first convert 81.00 mg/L CaCO3 to moles.
81.00 mg/L CaCO3 = 0.00045 moles CaCO3
Next, we need to convert from moles of CaCO3 to moles of H2PO4-. The molar ratio between CaCO3 and H2PO4- is 1:2, so for every mole of CaCO3, there are two moles of H2PO4-.
Therefore, 0.00045 moles CaCO3 = 0.00090 moles H2PO4-
Finally, we must convert the moles of H2PO4- back to mg/L:
0.00090 moles H2PO4- = 162.00 mg/L H2PO4-
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Why is capturing quality data and the use of analytics critical for the fire and emergency services?
Capturing quality data and using analytics are critical for the fire and emergency services to improve situational awareness, enhance resource management, improve incident management, and develop better planning and prevention strategies.
What is fire?
Fire is a chemical reaction that occurs when a fuel (such as wood, paper, or gasoline) combines with oxygen in the air, producing heat and light. The reaction is exothermic, meaning it releases energy in the form of heat and light. Fire requires three elements to exist: fuel, oxygen, and heat. These elements are often referred to as the "fire triangle."
Capturing quality data and using analytics are critical for the fire and emergency services for several reasons:
Improved situational awareness: Fire and emergency services need accurate, up-to-date information to make informed decisions and respond effectively to emergencies.
Enhanced resource management: Fire and emergency services often operate under tight budget constraints and need to make the most of their resources.
Improved incident management: The ability to capture and analyze data in real-time can help fire and emergency services manage incidents more effectively.
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Predicting the units of the solution to a basic quantitative... A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. (0.22L)×(1 mL/10‐³ L)×(1.57g/mL)/(61.04 g/mol) = ?
Answer:
(0.22 L) × (1 mL/10^-3 L) × (1.57 g/mL) / (61.04 g/mol) = ?
First, let's simplify the units:
(0.22 L) × (1000 mL/1 L) × (1.57 g/mL) / (61.04 g/mol) = ?
(0.22 L) × (1570 g/mol) / (61.04 g/mol) = ?
Now we can cancel out the units of g/mol:
(0.22 L) × (1570/61.04) = ?
(0.22 L) × 25.73 = ?
5.66 L·g
Therefore, the units of the student's answer are L·g.
Compared with the rate of water loss before soaking, what difference, if any, would you expect in the rate of water loss after soaking the hand in alcohol? (Clue: Fats are soluble in alcohol.)
Lipids dissolve in alcohol, a solvent. It removes the skin's lipids, particularly from the stratum corneum.
Because the lipids that normally prevent water loss are removed during alcohol soaking, the rate of water loss increases.
Why does alcohol evaporate water?Therefore, water may evaporate more slowly than other liquids despite having a lower molecular weight. The molecules of ethyl (rubbing) alcohol, which are more loosely bound than those of water, evaporate almost five times faster than water. Lower-energy, lower-temperature molecules are left behind when energetic molecules leave a liquid.
Question incomplete:The rate of water loss from the skin of a hand was measured. Following the measurement, the hand was soaked in alcohol for 15 minutes. After all the alcohol had been removed from the hand, the rate of water loss was again measured. Compared with the rate of water loss before soaking, what difference, if any, would you expect in the rate of water loss after soaking the hand in alcohol?
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If I leave 800 mL of 0.70 M sodium chloride solution uncovered on a windowsill and 300 mL of the solvent evaporates, what will the new concentration of the sodium chloride solution be?
Answer:
the new concentration of the sodium chloride solution after 300 mL of solvent evaporates is 1.12 M.
Explanation:
To calculate the new concentration of the sodium chloride solution after 300 mL of solvent evaporates, we need to first determine how many moles of solute are present in the original solution:
moles of solute = concentration x volume
moles of solute = 0.70 M x 0.800 L
moles of solute = 0.56 moles
Next, we can calculate the new volume of the solution after 300 mL evaporates:
new volume = original volume - amount evaporated
new volume = 0.800 L - 0.300 L
new volume = 0.500 L
Finally, we can calculate the new concentration of the solution using the moles of solute and the new volume:
new concentration = moles of solute / new volume
new concentration = 0.56 moles / 0.500 L
new concentration = 1.12 M
Therefore, the new concentration of the sodium chloride solution after 300 mL of solvent evaporates is 1.12 M.
8. What's the volume of 108g of a material if the material has a density of 0.90 g/mL?
A. 108.9 mL
B. 97.2 mL
C. 120 mL
D. 107.1 mL
Answer:
density = mass/volume
Rearranging, we get:
volume = mass/density
Substituting the given values, we get:
volume = 108g / 0.90 g/mL
volume = 120 mL
Therefore, the volume of the material is 120 mL. Answer: C
The density of a substance is its mass by volume. Then, the volume of the 108 g of material with a density of 0.90 g/ml is 120 mL.
What is density ?Density is a physical property of matter that describes the amount of mass in a given volume of a substance. It is defined as the ratio of an object's mass to its volume.
Mathematically, density is expressed as:
Density = Mass / Volume
The unit of density depends on the units of mass and volume used. For example, in the SI system, the unit of mass is kilograms (kg) and the unit of volume is cubic meters (m³), so the unit of density is kg/m³.
Given that, density = 0.90 g/ml
mass = 108 g
then volume = mass/densiy
v = 108 g/0.900 g/ml = 120 mL.
Therefore, density of the material is 120 mL.
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How many moles of S2 are needed to produce
.750 moles of SO2 gas?
Number of moles of S2 needed to produce 750 moles of SO2 is 375.
Mole calculationS2 + 202 ---> 2SO2 750 moles of SO2 = 375 moles of S2750 Mole Units750 ÷ 2 =375Balance the equation in step one. Chemical equations never have their individual components lost or destroyed; the yield of a reaction must precisely match the original reagents.Step 2: Converting the Units of a Substance Provided to Mole Conversion factors are applied during the conversion of supplied units into moles. Below, you'll find the most crucial conversion factors for converting between moles and grams, moles and gas volumes, moles and molecules, and moles and solutions. Similar to the ones outlined in the preceding section, these conversion factors also work Moreover, keep in mind that while these conversion factors are geared toward converting from one unit to another to determine moles, they can also be used to determine another unit to determine moles.For more information on moles kindly visit to
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What are the examples of tests performed on aspirin
Most frequently, a salicylates component is used to: Aid in the diagnosis of sudden or progressive aspirin toxicity. When you take a lot of aspirin at once, you might get acutely poisoned.
Can aspirin be detected in blood tests?Blood test results are frequently impacted by prescription medicines, non-prescription pharmaceuticals (such as aspirin, cold medicine, and vitamins), and alcohol consumption. In order to properly interpret the findings of your blood tests, your doctor needs a thorough and candid picture of your medication use.
What laboratory results does aspirin impact?Aspirin Reaction Units are used to report test findings (ARU). 350-549 ARU is the therapeutic range for people on an antiplatelet regimen to effectively suppress platelets. Those who are not taking aspirin or whose treatment is ineffectively suppressing platelet function have values of 550–700 ARU.
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if 100.0 ml ethyl alcohol weighs 78.5g ;determine the volume in litres occupied by 1,59 kg of ethyl alcohol
Answer: 2.025
Explanation: Set up the ratio 100ml/78.5g = xml/1.59kg
Once you have your units in order, solve for x and then convert to liters and there you have your answer!
you design an experiment to test the effect of adding different amounts of ice (grams) to a given volume of water.
For each trial you record the initial temperature of the water and then the final temperature after the ice was added.
In this experiment, the amount of ice is the
variable, and the temperature change is the
variable.
Answer:
In this experiment, the amount of ice is the independent variable, and the temperature change is the dependent variable.
The vapor pressure of mercury at 25 degrees Celsius is 1.85 mmHg . Calculate the vapor pressure in atm and torr . Round each of your answers to 3 significant digits.
The vapor pressure of mercury at 25°C is 1.85 torr. To convert the vapor pressure of mercury from mmHg to atm, we can use the conversion factor 1 atm = 760 mmHg:
Why does vapour pressure exist?A liquid's molecules enter the gaseous phase when heated because they have enough kinetic energy to overcome the forces holding them in the liquid. By doing this, they produce a population of molecules in the vapour phase above the liquid, which leads to the creation of a pressure—the liquid's vapour pressure.
1.85 mmHg x (1 atm / 760 mmHg) = 0.00243 atm (rounded to 3 significant digits)
Therefore, the vapor pressure of mercury at 25°C is 0.00243 atm.
To convert the vapor pressure of mercury from mmHg to torr, we can simply use the definition that 1 torr = 1 mmHg:
1.85 mmHg = 1.85 torr (rounded to 3 significant digits)
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write down the formulas and predict the products. Name and balance the equation iron(ii) bromide + Barium Chloride
The formula for iron(II) bromide is FeBr2, while the formula for barium chloride is BaCl2. The products of the reaction are barium bromide (BaBr2) and iron(II) chloride (FeCl2).
What is Balanced Equation ?
A balanced chemical equation is a symbolic representation of a chemical reaction that shows the relative numbers of reactant and product molecules or ions involved. In a balanced equation, the number of atoms of each element must be the same on both the reactant and product sides, in order to obey the law of conservation of mass.
The balanced chemical equation for the reaction between iron(II) bromide and barium chloride is:
FeBr2 + BaCl2 → BaBr2 + FeCl2
In this reaction, the iron(II) ion (Fe2+) in iron(II) bromide (FeBr2) is replaced by the barium ion (Ba2+) from barium chloride (BaCl2), forming barium bromide (BaBr2) and iron(II) chloride (FeCl2). The balanced equation shows that two bromide ions (Br-) and two chloride ions (Cl-) are involved in the reaction, which ensures that the equation is balanced in terms of both mass and charge.
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and H
An organic liquid having carbon, hydrogen and oxygen was
found to contain C = 37.5%
37.5% and H= 12.5% and the rest
oxygen. The molecular mass of this compound is 32. The
molecular formula for this compound is C2H5OH. True or false
The statement is false that the chemical compound ethanol, with a molecular mass of 46.07 g/mol, has the same molecular formula as Ethanol. The organic liquid, on the other hand, has molecules that weigh 32 g/mol.
Which of the following compounds has a carbon content by mass of 38.7%?Ethylene glycol is a substance that is frequently used as antifreeze. 38.7% of it is carbon, 9.75% hydrogen, and the remainder is oxygen. Ethylene glycol has a molecular weight of 62.07 g.
What is the name for organic substances with a carbon, hydrogen, and oxygen content of 121?In the molecules of carbohydrates, the proportion of carbon to hydrogen to oxygen is 1:2:1. This class of organic compounds gets its name from the parts water (water, -hydrate) and carbon (carbon, carbo-).
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Start with a 1.0 L solution with a 0.40 M concentration of sulfuric acid. The above solution is divided into two equal parts of the same volume. To the first part, 0.50 L of water is added. To the second part 1.5 L of water are added. After the previous procedure, the two parts are mixed and 2.0 L of 0.1 M sulfuric acid are added to this new solution. Determine the final molar concentration.
It’s urgent, please!
Answer:
Explanation:Before dividing the initial solution:
Initial volume = 1.0 L
Initial concentration = 0.40 M
After dividing into two equal parts:
Each part has a volume of 0.5 L
The first part has a concentration of 0.40 M
The second part has a concentration of 0.20 M (diluted by 50% with 1.5 L of water)
When the two parts are mixed:
Total volume = 1.0 L + 0.5 L + 0.5 L + 1.5 L = 3.5 L
Total moles of sulfuric acid = (1.0 L x 0.40 M / 1000) + (0.5 L x 0.40 M / 1000) + (0.5 L x 0.20 M / 1000) + (1.5 L x 0 / 1000) = 0.5 mol
Final concentration before adding more sulfuric acid = 0.5 mol / 3.5 L = 0.14 M
When 2.0 L of 0.1 M sulfuric acid are added:
Total volume = 3.5 L + 2.0 L = 5.5 L
Total moles of sulfuric acid = 0.5 mol + (2.0 L x 0.1 M / 1000) = 0.7 mol
Final concentration = 0.7 mol / 5.5 L = 0.13 M
Therefore, the final molar concentration of the solution is 0.13 M.
Cl2 + 2NaBr → 2NaCl + Br2
How many moles of bromine gas, are produced by the reaction of chlorine gas and of 5.2 moles of sodium bromide, NaBr?
Answer:
1 mole of Cl2 reacts with 2 moles of NaBr to produce 1 mole of Br2.
So, to calculate the number of moles of Br2 produced, we first need to find the number of moles of Cl2 required to react with 5.2 moles of NaBr. Since the stoichiometric ratio of Cl2 to NaBr is 1:2, we need half as many moles of Cl2 as moles of NaBr:
Number of moles of Cl2 = 5.2 moles NaBr / 2 = 2.6 moles Cl2
Now we can use the stoichiometric ratio between Cl2 and Br2 to calculate the number of moles of Br2 produced:
1 mole Cl2 produces 1 mole Br2
Therefore, 2.6 moles Cl2 will produce 2.6 moles Br2.
Explanation:
what is the product of the reaction of 2,2-dichloro-3-methylbutane with water. how does this product react with OH-
The reaction of 2,2-dichloro-3-methylbutane with water results in the formation of 3-methyl-2-butanol, which can react with OH- in a nucleophilic substitution reaction to form 3-methyl-2-butyl alcohol and water.
The reaction can be represented by the following equation:
2,2-dichloro-3-methylbutane + H2O → 3-methyl-2-butanol + H+ + Cl-
The reaction of 2,2-dichloro-3-methylbutane with water can result in the formation of an alcohol and a hydrogen ion. The product of this reaction is 3-methyl-2-butanol.
The reaction can be represented by the following equation:
2,2-dichloro-3-methylbutane + H2O → 3-methyl-2-butanol + H+ + Cl-
In this reaction, one of the chlorine atoms from 2,2-dichloro-3-methylbutane is replaced by a hydroxyl group (-OH) from water, resulting in the formation of an alcohol group (-OH) in the product, 3-methyl-2-butanol. The other chlorine atom remains as an ion, Cl-.
The product, 3-methyl-2-butanol, can react with OH- in a nucleophilic substitution reaction. In this reaction, the hydroxide ion (OH-) acts as a nucleophile and attacks the carbon atom that is attached to the leaving group (the -OH group) in the 3-methyl-2-butanol molecule. The leaving group then departs with its pair of electrons, forming a new bond with the nucleophile (OH-). The result is the formation of a new alcohol molecule.
The reaction can be represented by the following equation:
3-methyl-2-butanol + OH- → 3-methyl-2-butyl alcohol + H2O
In this reaction, the -OH group of 3-methyl-2-butanol is replaced by the hydroxide ion (OH-) to form 3-methyl-2-butyl alcohol, and a water molecule is formed as a byproduct.
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Which of the following is NOT a synthetic material?
Multiple choice question.
cross out
A)
polyester
cross out
B)
bone china
cross out
C)
wood
cross out
D)
concrete
Answer: C) wood cross out
Consider a solution that is 1.4×10−2 M in Ba2+ and 1.9×10−2 M in Ca2+. What minimum concentration of Na2SO4 is required to cause the precipitation of the cation that precipitates first? Express your answer using two significant figures.
Tο determine which catiοn will precipitate first, we need tο cοmpare the sοlubility prοducts (Ksp) οf their respective sulfates. The catiοn with the smaller Ksp value will precipitate first. The Ksp values fοr BaSO₄ and CaSO₄ are:
Ksp(BaSO₄) = 1.1 × 10⁻¹⁰
Ksp(CaSO₄) = 2.4 × 10⁻⁵
What is a catiοn?A catiοn is an iοn with a pοsitive charge that is fοrmed by the lοss οf οne οr mοre electrοns frοm a neutral atοm. Catiοns are fοrmed when atοms lοse electrοns tο achieve a mοre stable electrοn cοnfiguratiοn, typically by becοming isοelectrοnic with a nearby nοble gas.
Since the Ksp value fοr BaSO4 is smaller, it will precipitate first. Tο calculate the minimum cοncentratiοn οf Na₂SO₄ required tο precipitate all οf the Ba2+ iοns, we need tο use the sοlubility prοduct expressiοn fοr BaSO₄:
BaSO₄(s) ⇌ Ba2+(aq) + SO₄₂-(aq)
Ksp = [Ba2+][SO₄₂-]
Since all οf the Ba2+ iοns will be precipitated, the cοncentratiοn οf Ba2+ will be zerο οnce precipitatiοn is cοmplete. Thus, the Ksp expressiοn simplifies tο:
Ksp = [SO₄₂-]²
Sοlving fοr [SO₄₂-], we get:
[SO₄₂-] = sqrt(Ksp) = sqrt(1.1 × 10⁻¹⁰) = 1.05 × 10⁻⁵ M
This means that the cοncentratiοn οf Na₂SO₄ needs tο be at least 1.05 × 10⁻⁵M tο prοvide enοugh SO₄₂- iοns tο precipitate all οf the Ba₂+ iοns. We rοund this tο twο significant figures, giving a final answer οf 1.1 × 10⁻⁵ M Na₂SO₄.
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A 15.0 g sample of potassium chlorate is decomposed, according to the following balanced equation:
2 KClO3(s) ----> 2 KCl(s) + 3 O2(g)
Part A) Assuming complete decomposition, calculate the volume of O2 (in L) collected at 27°C and 756 torr pressure.
Part B) If the oxygen gas in the reaction above is collected over water, it will be saturated with water vapor. Will you need to adjust the pressure of 756 torr?
We can use the ideal gas law to solve for the volume of oxygen gas produced:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.08206 L atm/mol K), and T is the temperature in Kelvin.
First, we need to calculate the number of moles of oxygen gas produced from the given mass of potassium chlorate. We can use the molar mass of KClO3 (122.55 g/mol) and the stoichiometry of the balanced equation:
15.0 g KClO3 x (1 mol KClO3/122.55 g KClO3) x (3 mol O2/2 mol KClO3) = 0.184 mol O2
Now we can solve for the volume of oxygen gas at 756 torr (convert to atm) and 27°C (convert to Kelvin):
P = 756 torr = 0.996 atm
T = 27°C + 273.15 = 300.15 K
n = 0.184 mol
R = 0.08206 L atm/mol K
V = nRT/P = (0.184 mol)(0.08206 L atm/mol K)(300.15 K)/(0.996 atm) = 4.76 L
Therefore, the volume of O2 collected at 27°C and 756 torr pressure is 4.76 L.
Part B:
If the oxygen gas is collected over water, it will be saturated with water vapor. This means that the total pressure in the container will be the sum of the pressure of the oxygen gas and the pressure of the water vapor. The pressure of the water vapor can be calculated using the vapor pressure of water at the given temperature.
At 27°C, the vapor pressure of water is 26.7 torr. Therefore, the total pressure in the container will be:
P total = P oxygen gas + P water vapor = 756 torr + 26.7 torr = 782.7 torr
Since the problem provided the pressure in torr, we need to convert to atm before using the ideal gas law. Therefore, we need to adjust the pressure to:
P = 782.7 torr x (1 atm/760 torr) = 1.03 atm
We can then use the same equation as in part A to calculate the volume of oxygen gas:
V = nRT/P = (0.184 mol)(0.08206 L atm/mol K)(300.15 K)/(1.03 atm) = 4.32 L
Therefore, if the oxygen gas is collected over water, the volume of oxygen gas produced would be 4.32 L instead of 4.76 L (as in part A).
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Chemistry Help!
1. Imagine that you are dissolving a red Gatorade mix in water.
a. What is the solute?
b. What is the solvent?
c. What is the solution?
d. What could you do to increase the molarity of the Gatorade in the water?
Answer:
a. The solute is the substance that is being dissolved, in this case, the red Gatorade mix.
b. The solvent is the substance in which the solute is being dissolved, in this case, water.
c. The solution is the resulting homogeneous mixture of the solute (red Gatorade mix) and the solvent (water).
d. To increase the molarity of the Gatorade in the water, you could add more Gatorade mix to the water while keeping the volume of the solution constant. Alternatively, you could decrease the volume of water while keeping the amount of Gatorade mix constant, which would increase the concentration of Gatorade in the solution.
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Given the following balanced equation, determine the mass of H2 if you start with 4.55x1025 molecules of C5H12.
C5H12-->C5H8+2H2
If you start with 4.55 x 10²⁵ molecules of C₅H₁₂, you would produce 1.82 x 10²⁶ g of H₂.
What is the mass of H₂ ?The balanced equation shows that for every one molecule of C₅H₁₂ that reacts, 2 molecules of H₂ are produced.
C₅H₁₂ --> C₅H₈ + 2H₂
To determine the mass of H₂ produced, we need to convert the number of molecules of C₅H₁₂ to molecules of H₂ using the stoichiometry of the balanced equation:
1 molecule of C₅H₁₂ produces 2 molecules of H₂
4.55 x 10²⁵ molecules of C₅H₁₂ x (2 molecules of H₂ / 1 molecule of C₅H₁₂) = 9.10 x 10²⁵ molecules of H₂
Now, to find the mass of H₂ produced, we need to use the molar mass of H₂, which is approximately 2 g/mol:
9.10 x 10²⁵ molecules of H₂ x (2 g/mol) = 1.82 x 10²⁶ g of H₂
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Answer:
9.10 x 10²⁵ molecules of H₂ x (2 g/mol) = 1.82 x 10²⁶ g of H₂
Explanation:
In a perfect world, your calorimeter will not exchange any heat with its contents. In this perfect world, if hot water loses 75 calories when cool metal pieces are poured in, how many calories do the metal pieces gain?
Answer:
In a perfect world, where the calorimeter does not exchange any heat with its contents, the amount of heat lost by the hot water will be equal to the amount of heat gained by the cool metal pieces. This is due to the principle of conservation of energy, which states that energy cannot be created or destroyed, only transferred from one form to another. Therefore, the number of calories gained by the metal pieces will be equal to the number of calories lost by the hot water, which is 75 calories.
Explanation:
In summary, according to the principle of conservation of energy, in a perfect world where a calorimeter does not exchange any heat with its contents, the number of calories gained by the cool metal pieces will be equal to the number of calories lost by the hot water, which is 75 calories.
C₂H5OH + 302 → 2CO₂ + 3H₂O AH-1367kJ/mol
How many grams of carbon dioxide are produced when 370. kJ of energy are used in the following reaction?
We can start by using the given enthalpy change and the balanced equation to calculate the amount of moles of carbon dioxide produced:
1 mol of C2H5OH produces 2 mol of CO2
-1367 kJ/mol is released when 1 mol of C2H5OH is combusted
370 kJ of energy are used in the reaction
Now we can use a proportion to find the number of moles of C2H5OH that produce 370 kJ of energy:
-1367 kJ/mol / 1 mol of C2H5OH = -x kJ / (2 mol of CO2)
Solving for x gives:
x = (370 kJ) (1 mol of C2H5OH) / (-1367 kJ/mol) (2 mol of CO2)
x = 0.1355 mol of CO2
Finally, we can use the molar mass of CO2 (44.01 g/mol) to find the mass of CO2 produced:
mass of CO2 = number of moles of CO2 * molar mass of CO2
mass of CO2 = 0.1355 mol * 44.01 g/mol = 5.96 g of CO2
Therefore, when 370 kJ of energy are used in the reaction, 5.96 g of carbon dioxide are produced.
the density of a fluid is given by the empirical equation p=70.5exp
the density fluid is given by the empirical equation p=70.5exp (82700000p) where rho is density (lbm/ft3)and p is the pressure (lbf/in2) a, what are the unit of 70.5 and 82700000
Answer:
The density equation is given by:
p = 70.5 * exp(82700000 * p)
where p is the pressure in pounds per square inch (lbf/in²) and ρ is the density in pounds per cubic foot (lbm/ft³).
To determine the units of the constants 70.5 and 82700000 in short, we can use dimensional analysis.
The unit of the exponential term is dimensionless, so we only need to consider the units of the constant term.
The unit of the density (ρ) is lbm/ft³, and the unit of the pressure (p) is lbf/in².
So, we can write the equation as:
ρ = (70.5 lbm/ft³) * exp(82700000 * p)
To get the units of the constant 70.5, we can divide both sides by the exponential term and simplify:
ρ / exp(82700000 * p) = 70.5 lbm/ft³
Therefore, the units of 70.5 are lbm/ft³.
To get the units of the constant 82700000, we can rearrange the equation and take the natural logarithm of both sides:
ln(ρ/70.5 lbm/ft³) = 82700000 * p
The units of the left-hand side are dimensionless, and the units of the right-hand side are 1/in². So, the units of the constant 82700000 are 1/in².
(i) Calculate the mass of CO2(g) in gram produced by the reaction between 3 mol of CH4(g) and 2 mol of
O2(g) according to the equation : CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
Answer: 0.1334983576 g
Explanation:
The mass must be conserved on both sides of the equation. Mass put in must must = mass put out. So we must start by finding the mass of the reactants and then the mass of 2H2O. Then we must subtractio the mass of the reactants from the mass of 2H2O which will gives us the mass of CO2.
Mass of CH4:
(12.0107)+ 4(1.00794) = 16.48246 g/mol
we are given three mols of CH4 so divide 3 mol by 16.48246 g/mol
3 mol/ 16.48246 g/mol = 0.1820116657 g CH4
Mass of 2O2:
2(15.99994) = 31.99988 g/mol
we are given 2 moles of 2O2 so divide 2 mol by 31.99988 g/mol
2 mol/ 31.99988 g/mol = 0.0625002344 g 2O2
Mass of 2H2O:
2(1.00794)+(15.99994) = 18.01582 g/mol
we are given 2 moles of 2H2O so divide 2 mol by 18.01582 g/mol
2 mol/ 18.01582 g/mol = 0.1110135425 g 2H20
Now we add up the grams on the reactatnt side and subtract that number from the mass of 2H2O:
0.1820116657 g CH4 + 0.0625002344 g 2O2 = 0.2445119001 g (total of g of reactants)
0.2445119001 g - 0.1110135425 g = 0.1334983576 g CO2
check bracket.The temperature of an/
(dt h)²-(q nn)²( ja ki)⁴ /oven being heated using a pulsed resistance heater varies as T = 120 + 5cos(25t+30°) where t is the time in seconds. The temperature of the oven is being measured with a ther mo couple having a time constant of 5 s. ( a ) What are the maximum and minimum temperatures indicated by the thermocouple? ( What is the maximum difference between the actual temperature and the indicated temperature? ( c ) What is the time lag between the actual temperature and the indicated temperature?
a. The maximum and minimum temperature of a thermocouple is [tex]-200^{o} C to 350^{o} C[/tex].
Therefore the difference between the actual and indicated temperature is indicated as [tex](125*5 = 625^{o} C/s)[/tex]
c.The time lag between the actual temperature and the indicate temperature is equal to the time constant of the thermocouple.
What do you mean thermocouple ?A sensor that detects temperature is a thermocouple. It is made up of two distinct metals that are attached at one end. A voltage is produced that is linked to temperature when the junction of the two metals is heated or cooled.
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Which set of reactants will be the most efficient (LEAST wasteful of materials) for the reaction?
We need to calculate the stoichiometric ratios of the reactants and choose the set that provides the required ratios with the least amount of excess or unused reactants.
How to determine most efficient chemicals?To determine the most efficient set of reactants for a reaction, we should consider the stoichiometry of the reaction, which tells us the ratios of the reactants and products that are involved in the reaction. The most efficient set of reactants will be the one that produces the desired product with the least amount of excess or unused reactants, and hence the least amount of waste.
What is the example for that?2A + 3B → 4C If we have 4 moles of A and 6 moles of B, we have the exact stoichiometric amounts required for the reaction to proceed, and all the reactants will be consumed completely to form 8 moles of product C. In this case, there will be no waste of materials, and the reaction will be the most efficient. On the other hand, if we have an excess of one of the reactants, for example, if we have 6 moles of A and 6 moles of B, then only 4 moles of A can react with 6 moles of B to produce 8 moles of C, and the remaining 2 moles of A will be unused and wasted. In this case, the reaction will be less efficient.
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A sample of the compound weighs 80 grams. How many grams of cobalt are in the sample?
The mass of the unknown element cobalt is obtained as 40 g. This can be seen from the calculation that we have in the solution.
How can you use the molar mass of the compound to find the relative atomic mass of the unknown element?If you have a compound that contains an unknown element, you can use the molar mass of the compound to find the relative atomic mass of the unknown element
We can see that the question has already given us the mass of the sample as we have and the percentage of the cobalt that we have in the sample.
50 = x/80 × 100
x = 50/100 × 80
= 40 g
Thus we would have a total of about 40 g of cobalt in the sample.
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Missing parts;
A sample of the compound weighs 80 grams. If the mass percent of cobalt is 50%, How many grams of cobalt are in the sample?