Answer:
Concentrations of HAc and NaAc you need are 0.122M
Explanation:
pKa of acetic acid is 4.75, that means when amount of sodium acetate and acetic acid is the same, pH will be 4.75
Thus, you know [NaAc]i = [HAc]i
Now, using H-H equation, when pH = 3.75:
3.75 = 4.75 + log [NaAc] / [HAc]
0.1 = [NaAc] / [HAc]
10 [NaAc] = [HAc]
Thus, after the reaction [HAc] must be ten times, [NaAc].
Based in the reaction of NaAc with HCl
NaAc + HCl → HAc + NaCl
Moles of HCl added are:
1mL = 0.001L * (10mol /L) = 0.01 moles HCl.
That means moles of both compounds after the reaction are:
[NaAc] = [NaAc]i - 0.01 mol
[HAc] = [HAc]i + 0.01
Replacing these equations with the information you know:
[NaAc] = [NaAc]i - 0.01 mol
10[NaAc] = [NaAc]i + 0.01
Subtracting both equations:
9[NaAc] = 0.02mol
[NaAc] = 0.0022 moles.
Replacing in [NaAc] = [NaAc]i - 0.01 mol
0.0022mol = [NaAc]i - 0.01 mol
0.0122mol = [NaAc]i = [HAc]i
These moles in 100.00mL = 0.1000L:
[NaAc]i = [HAc]i = 0.0122mol / 0.100L =
0.122M
Thus, concentrations of HAc and NaAc you need are 0.122M
To create this buffer, you need to pipette 12.2mL of both 1.0M NaAc and 1.0M HAc and dilute this mixture to 100.0mL
Based on the Henderson-Hasselbach equation, the concentrations of HAc and NaAc required is 0.122M
In order to prepare this buffer, pipette 12.2 mL each of the stock 1.0M NaAc solution and 1.0M HAc solution, and dilute this mixture to 100.0mL.
What is a buffer solution?A buffer solution is a solution which resists changes to its pH when a small volume of acid or base is added to it.
A buffer solution is usually prepared from a weak acid and its conjugate base or a weak base and its conjugate acid.
From the data provided:
pKa of acetic acid is 4.75
Thus, at pH 4.75, the initial concentrations of NaAc and HAc are equal.
[NaAc]i = [HAc]iFrom the Henderson-Hasselbach equation, when pH = 3.75
3.75 = 4.75 + log [NaAc]/[HAc]
0.1 = [NaAc] / [HAc]
10[NaAc] = [HAc]
Therefore, after the reaction, [HAc] will be ten times [NaAc].
HCl is added to the buffer to bring the pH to 3.75
Equation of the reaction of NaAc with HCl is given as:
NaAc + HCl → HAc + NaClMoles of HCl added = molarity × volume in Lmoles of HCl added = 0.001L * (10mol /L) = 0.01 moles HCl.
Thus, after the addition of HCl, concentration of NaAc and HAc will be:
[NaAc] = [NaAc]i - 0.01 mol
[HAc] = [HAc]i + 0.01
Recall; 10[NaAc] = [HAc]
Substituting [HAc] = 10[NaAc
[NaAc] = [NaAc]i - 0.01 mol ----(1)
10[NaAc] = [NaAc]i + 0.01 -----(2)
Subtracting (1) from (2) equations:
9[NaAc] = 0.02mol
[NaAc] = 0.0022 moles.
Substituting in [NaAc] = [NaAc]i - 0.01 mol
0.0022mol = [NaAc]i - 0.01 mol
[NaAc]i = 0.0122mol
Also, [HAc]i = 0.0122mol
What is the Molarity of the required solutions?The molarity is determined using the formula below:
Molarity of the solution = moles/volumevolumeof buffer = 100 mL = 0.100 L
[NaAc]i = [HAc]i = 0.0122mol / 0.100L
[NaAc]i = [HAc]i = 0.122M
Therefore, concentrations of HAc and NaAc required is 0.122M
In order to prepare this buffer, pipette 12.2 mL each of the stock 1.0M NaAc solution and 1.0M HAc solution, and dilute this mixture to 100.0mL.
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An unknown monoprotic acid HA with a concentration of 0.050 M has a pH of 2.3. Which of the following can we conclude?
A) It must be a strong acid.
B) It must be a weak acid.
C) A salt of its conjugate base would have no pH effect in solution.
D) Both A and C
E) None of the above
Answer:
B) It must be a weak acid.
Explanation:
If HA is a strong acid
[tex]HA\rightleftharpoons H^++A^-[/tex]
Now the pH value can be written as follows
[tex]pH=-log[H^+]\\pH=-log(5\times 10^{-2})\\pH=2\times log5\\pH=1.4[/tex]
But given that acid HA has 2.3 pH value.
Therefore we can say that HA is weak acid.
Thus the answer will be option (B).
B) It must be a weak acid.
If 500 mL of 2.0 M HCl is diluted with water to a volume of 1 liter, what is the molarity of the new solution?
Answer: 1 mole per L
Explanation:
(2M)(500mL)=(M)(1000mL)
1000=(M)(1000mL)
M=1
Taking into account the definition of dilution, if 500 mL of 2.0 M HCl is diluted with water to a volume of 1 liter, the molarity of the new solution is 1 M.
DilutionWhen it is desired to prepare a less concentrated solution from a more concentrated one, it is called dilution.
Dilution is the process of reducing the concentration of solute in solution, which is accomplished by simply adding more solvent to the solution at the same amount of solute.
In a dilution the amount of solute does not change, but as more solvent is added, the concentration of the solute decreases, as the volume (and weight) of the solution increases.
A dilution is mathematically expressed as:
Ci×Vi = Cf×Vfwhere
Ci: initial concentrationVi: initial volumeCf: final concentrationVf: final volumeFinal molarityIn this case, you know:
Ci= 2.0 MVi= 500 mLCf= ?Vf= 1 L= 1000 mLReplacing in the definition of dilution:
2.0 M× 500 mL= Cf× 1000 mL
Solving:
(2.0 M× 500 mL)÷ 1000 mL= Cf
1 M= Cf
In summary, if 500 mL of 2.0 M HCl is diluted with water to a volume of 1 liter, the molarity of the new solution is 1 M.
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If an electromagnetic wave has a frequency of 4.5 x 10^18 Hz, what is its wavelength? The speed of light is 3 x 108 m/s.
Answer:
Wavelength, λ = 6.7 x 10^-11 m
Explanation:
Frequency and wavelength are inversely proportional to each other.
In this problem;
f = 4.5 x 10^18 Hz
wavelength, λ = ?
Speed of light, c = 3 x 108 m/s.
These variables are related by the following equation;
c = λ * f
Making λ subject of focus, we have;
λ = c / f
λ = 3 x 10^8 / 4.5 x 10^18
λ = 0.67 x 10^-10
λ = 6.7 x 10^-11 m
How many ng(nanogram) are in 3.3 mg(milligram)
Answer:
There are [tex]3.3(10^6)[/tex] nanograms in 3.3 milligrams
Explanation:
The conversion is 1 milligram is equal to [tex]1(10^6)[/tex] nanograms. Use the base 10 decimal system to help you.
Answer:
3 300 000 000 000 ng * nanogram
Explanation:
If the same amount of heat is added to 25.0 g of each of the metals, which are all at the same initial temperature, which metal will have the highest final temperature
Answer:
The metal with the lowest specific heat capacity
Explanation:
Hello, this question can be solved when we compare their specific heat capacities.
Specific heat capacity of a metal /substance is the heat required to raise it's temperature by one degree Celsius.
Mathematically,
Q = mc∇θ
Q = heat energy applied
M = mass of the metal
C = specific heat capacity of the metal
∇θ = (θ₂ - θ₁) which corresponds to the change in temperature of the metal.
In a given experiment of different metals with different specific heat capacities, assuming they're of equal mass and same amount of energy is applied with the same amount of initial temperature, the metal with the lowest specific heat capacity would have the highest final temperature likewise the metal with the highest specific heat capacity would have the lowest final temperature.
The is due to the energy required to raise the temperature of the metal by 1°C
What is the molarity of a solution that is 7.00% by mass magnesium sulfate and has a density of 1.071 g/mL?
Answer:
0.623 M
Explanation:
Step 1: Given data
Percent by mass (%m/m): 7.00 %Density of the solution (ρ): 1.071 g/mLMolar mass of magnesium sulfate: 120.37 g/molStep 2: Calculate the percent by volume (%m/v)
We will use the following expression.
[tex]\%m/v = \%m/m \times \rho = 7.00\% \times 1.071g/mL = 7.50g\%mL[/tex]
Step 3: Calculate the molarity
7.50 g of magnesium sulfate are dissolved in 100 mL of the solution. The molarity is:
[tex]M = \frac{7.50g}{120.37g/mol \times 0.100L } = 0.623 M[/tex]
As , P , S , Na which of these atomes has the highest ionization energy ?
Answer:
it is Na
Explanation:
because u need to pay attention i school and u wouldnt need to know these answer
At a temperature of 393 K, the pressure of a sample of nitrogen is 1.07 atm. What will the pressure be at a temperature of 478 K? (Assume constant volume)
Answer:
1.30atm
Explanation:
P1/T1 = P2/T2
1.07/393 = P2/478
Answer: the first one is correct
Explanation:
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A sample of hydrogen gas exerts a pressure of 466 torr in a container. What is this pressure in atmospheres? (1 atmosphere = 1.01325 x 10^5 Pa=760 torr
Answer:
pressure = 0.61512atm
Explanation:
1 torr = 0.00132 atm
466 torr = unknown atm
unknown = 0.61512 atm
pressure = 0.61512atm
The complex [Ni(CN)4]2- is diamagnetic and the complex [NiCl4]2- is paramagnetic. What can you conclude about their molecular geometries
Answer:
[Ni(CN)4]2- square planar
[NiCl4]2- tetrahedral
Explanation:
For a four coordinate complex such as [Ni(CN)4]2- and [NiCl4]2-, we can decide its geometry by closely considering its magnetic properties. Both of the complexes are d8 complexes which could be found either in the tetrahedral or square planar crystal field depending on the nature of the ligand.
CN^- being a strong field ligand leads to the formation of a square planar diamagnetic d8 complex of Ni^2+. Similarly, Cl^- being a weak field ligand leads to the formation a a tetrahedral paramagnetic d8 complex of Ni^+ hence the answer given above.
A compound consisting of atoms of small atomic mass is more likely to require what
Answer:
a lower temperature to liquefy
Explanation:
7.2 litters of an ideal gas are contained at 4.0 atm and 27•C. Using the ideal gas law, calculate how many moles of this gas are present.
Answer:
The correct answer is 1.17 moles
Explanation:
The ideal gas equation combines the pressure (P), volume (V), temperature (T) and number of moles of a gas (n):
PV= nRT
R is the gas constant (0.082 L.atm/K.mol)
In this case, we have:
V= 7.2 L
P= 4.0 atm
T= 27ºC + 273 = 300 K
We calculate the number of moles (n) of gas as follows:
n= (PV)/(RT)= (4.0 atm x 7.2 L)/(0.082 L.atm/K.mol x 300 K) = 1.17 mol
What would the cathode be in a nickel and copper electrolytic cell
Answer:
d
Explanation:
The following ions contain the same number of electrons. Rank them in order of decreasing ionic radii. Rank from largest to smallest radius. To rank items as equivalent, overlap them.K^+,Sc^3+,Cl^-,S^2-,P^3-
Answer:
P^3- > S^2- > Cl^- > K^+ > Sc^3+
Explanation:
Ionic radii is an example of physical properties of Periodicity.
The size of an atom's ion is difficult to estimate because of the electronic distribution and arrangement. This is due to the fact that the atom' ion have no definite outer boundary. In order to circumvent this problem, the atom's ion is estimated in a crystal lattice in terms of its ionic radii.
Ionic radii is taken as half the distance between atomic ions in a crystal lattice. Across a period in the periodic table , ionic radii decreases progressively from left to right.
Down the group, the ionic radius increases from top to bottom.
So the arrangement of the given elements from largest to smallest radius in the decreasing order of ionic radius will be:
P^3- > S^2- > Cl^- > K^+ > Sc^3+
The ranging from largest to smallest should be P^3- > S^2- > Cl^- > K^+ > Sc^3+.
What are ionic radii?It represents an example of the physical properties of Periodicity. It is considered to be half of the distance that lies between the atomic ions in a crystal lattice. It should be decreased progressively from left to right.
The ionic radius rises from top to bottom. It contains similar no of electrons, there should be the size difference because of the strength of the nuclear attraction.
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What energy transfer happens when wood is burning?
Answer:
Mechanical to Heat
explanation:
The wood itself can make mechanical energy but when it's on fire it makes heat energy
Answer: Chemical to heat and light
Explanation: The energy transforms from chemical energy to heat and light energy. Because when the candle burns a chemical reaction occurs and produces heat and light.
Think about it: Gold is one of the densest substances known, with a density of 19.3 g/cm3. If the gold in the crown was mixed with a less-valuable metal like bronze or copper, how would that affect its density?
Answer:
If gold has a rare, high density then it would sink quickly. If mixed substances that are less-valued, are added to the gold crown (remember that gold is rare and very dense which makes it special) then we can assume the cheap substances are less dense, thus making the crown FLOAT more rather than sink (I say more, because unless the crown was extremely mixed with cheap material then it could possibly float but it depends on how much is in the crown). Summary: The crown would either be lighter and float, or barely be sunken due to the less-dense substance.
*Hint to think about: People consider cheaper things lighter such as plastic ring/less dense for example, compared to a silver ring which is heavier/more dense (btw heavy does not always mean high density, it depends on the liquid density )
Hope this actually helps!
Explanation:
High-Desnity=Sink
Low Density=Float
As lead chemist for a pharmaceutical manufacturing company, you need to inform the purchasing office of a supply order for the next batch of cisplatin, PtCl2(NH3)2. If you intend to make a 500kg batch, how many kg chlorine gas do you need to order?
Answer:
mass of chlorine gas required is 118 kg.
Explanation:
Total mass of the drug (Cisplatin) required = 500 kg
For the drug PtCl2(NH3)2, we first find the molar mass of the compound.
The molar mass of the drug is the total of all the molar mass of the elements in the drug
molar mass of Pt (platinum) in the drug = 195.078 g/mol
molar mass of chlorine (Cl) in the drug = 2 x (35.453 g/mol) = 70.908 g/mol
molar mass of ammonia (NH3) in the drug = 2 x (17.031 g/mol) = 34.062 g/mol
Total molar mass of the drug = 195.078 g/mol + 70.908 g/mol + 34.062 g/mol = 300.048 g/mol
fractional composition of chlorine in the drug = 70.908/300.048 = 0.236
mass of chlorine required for 500 kg of the drug = 0.236 x 500 = 118 kg
How many water molecules are in a block of ice containing 1.25 mol of water (H2O)
Answer:
Molecules = 7.5 × 10²³ molecules
Explanation:
Given:
Moles = 1.25 mol
Avogadro's No. = [tex]N_{A}[/tex] = 6.022 * 10²³
Required:
Molecules = ?
Formula:
Molecules = Moles × [tex]N_{A}[/tex]
Solution:
Molecules = 1.25 × 6.022 × 10²³
Molecules = 7.5 × 10²³ molecules
Look up and record the boiling point of acetic acid, and explain why only some of it evaporates from the reaction mixture.
Answer:
Heating the mixture to a temperature above the boiling point of acetic acid, but below 100°C (the boiling point of water). The vapours from the acetic acid rise, and go into a tube. They are then condensed within the tube, and run off into a separate storage area. Because water can exist as a gas at pretty much any temperature above 0°C, it will result in an impure mixture, but repeatedly doing this will get the acetic acid to the desired purity.
The mathematics of combining quantum theory with wave motion of atomic particles is known as _____.
Combining quantum theory with wave motion of atomic particles is: Wave Mechanics
Morphine, C 17H 19NO 3, is often used to control severe post-operative pain. What is the pH of the solution made by dissolving 25.0 mg of morphine in 100. mL of water? (For morphine, K b = 1.62 × 10 –6.)
Answer:
pH = 9.58
Explanation:
First of all, we need to determine the molarity of the solution.
We determine the molar mass of morphine:
12g/m . 17 + 1 g/m . 19 + 14 g/m + 16 g/m . 3 = 285.34 g/m
molar mass g/m, is the same as mg/mm
25 mg . 1 mmol / 285.34 mg = 0.0876 mmoles / 100 mL = 8.76×10⁻⁴ M
In diltuted solution, we must consider water.
Mass balance for morphine = [Morphine] + [Protonated Morphine]
8.76×10⁻⁴ M = [Morphine] + [Protonated Morphine]
As Kb is too small, I can skipped, the [Protonated Morphine]
8.76×10⁻⁴ M = [Morphine]
In the charge balance I will have:
[OH⁻] = [H⁺ morphine] + [H⁺]
Let's go to the Kb expression
Morphine + H₂O ⇄ MorphineH⁺ + OH⁻ Kb
Kb = [MorphineH⁺] [OH⁻] / [Morphine]
Kb = [MorphineH⁺] [OH⁻] / 8.76×10⁻⁴ M
So now, we need to clear [MorphineH⁺] to replace it in the charge balance
Kb . 8.76×10⁻⁴ M / [OH⁻] = [MorphineH⁺]
Now, the only unknown value is the [OH⁻]
[OH⁻] = Kb . 8.76×10⁻⁴ M / [OH⁻] + Kw/[OH⁻]
Remember that Kw = [H⁺] . [OH⁻]
[H⁺] = Kw/[OH⁻]
[OH⁻]² = 1.62×10⁻⁶ . 8.76×10⁻⁴ + 1×10⁻¹⁴
[OH⁻] = √(1.62×10⁻⁶ . 8.76×10⁻⁴ + 1×10⁻¹⁴)
[OH⁻] = 3.76×10⁻⁵ → - log [OH⁻] = pOH = 4.42
pH = 14 - pOH → 14 - 4.42 = 9.58
What is the product(s) of the reaction below?
2Al(s) + Fe2O3(s) Al2O3(s) + 2Fe(s)
A. Solid aluminum oxide and solid iron
B. Solid aluminum
C. Saturated aluminum oxide and saturated iron
D. Iron(III) oxide and aluminum oxide
Answer:
I would put A
Explanation:
A new substance is produced as a result of a chemical reaction in which bonds between the molecules of the reactant and product are broken and new bonds are formed. Here the products are Al₂O₃ and Fe. The correct option is A.
Chemical reactions are interactions between two or more molecules that result in the production of new products. Products, as opposed to reactants, are compounds that result from an interaction between two other substances.
The reactants are on the left, while the products that are created are on the right. A one-headed or two-headed arrow connects the reactants and products.
Thus the correct option is A.
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the iupac name this compound
Answer:
It's HYDROXIDE
Explanation:
You do not call it as hydroxide ion because ion always have + or -
I hope this helps
HAVE A GOOD DAY!
Answer:
Tetranol
Explanation:
Since it consist of 4 carbons So the prefix is "Tetra"
=> It has an "OH" group attached to it so the functional group is "ALCOHOL".
For alcohols, the suffix is "-ol" so the name becomes
=> Tetranol
A 8.06 g piece of solid CO 2 is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 300.0 K. What is the pressure of the gas?
Answer:
The pressure of the gas is 4.428 atm.
Explanation:
Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.
Considering a certain amount of ideal gas confined in a container where the pressure, volume and temperature can vary, but keeping the mass constant, that is, without altering the number of moles, the pressure, P, the temperature can be related, T and the volume, V, of an ideal gas using the ideal gas law:
P*V = n*R*T
where R is the ideal gas constant, and n is the number of moles of the gas.
In this case, to know n you must know the molar mass of the CO₂ compound. Being:
C: 12 g/moleO: 16 g/molethen, the molar mass of CO₂ is: 12 g/mole + 2*16 g/mole= 44 g/mole
Then you apply a rule of three: if 44 grams of CO₂ are present in 1 mole, 8.06 grams in how many moles are they?
[tex]moles of CO_{2} =\frac{8.06 grams*1 mole}{44 grams}[/tex]
moles of CO₂= 0.18 moles
Then, you know:
P: ?V: 1 Ln: 0.18 molesR= 0.082[tex]\frac{atm*L}{mol*K}[/tex]T= 300 KReplacing in the equation of the ideal gas law:
P* 1 L= 0.18 moles* 0.082[tex]\frac{atm*L}{mol*K}[/tex] * 300 K
Solving:
[tex]P=\frac{0.18 moles* 0.082 \frac{atm*L}{mol*K} *300 K}{1 L}[/tex]
P= 4.428 atm
The pressure of the gas is 4.428 atm.
Resources Use the exothermic and endothermic interactive to classify the solution process for each solute. Exothermic solution process Endothermic solution process
KOH CaCl, NaCT NaOH NaNO, NH NO,
Answer:
Exothermic interractive are the following: NaOH, KOH, CaCl₂
Endothermic interactive are the following: NaCl, NH₄NO₃, NaNO₃
Explanation:
NaOH, KOH, and CaCl2 are exothermic reactants. NaCl, NH4NO3, and NaNO3 are endothermic interacting substances.
Endothermic reactions: what are they?Chemical processes that can release or absorb energy are referred to as endothermic. In endothermic reactions, more energy is used when bonds in the reactants are broken than is released when new bonds are formed in the products.
How do endothermic processes take place?When the temperature of the an isolated system drops while the surroundings of the a non-isolated system warm up, this is known as an endothermic response. The heat of reaction is generally positive in endothermic processes (qrxn>0).
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The basic function of a carburetor of an automobile is to atomize the gasoline and mix it with air to promote rapid combustion. As an example, assume that 30 cm3 of gasoline is atomized into N spherical droplets, each with a radius of 2.0 × 10−5 m. What is the total surface area of these N spherical droplets? Answer: [A] m2.
Answer:
The total surface area of these N spherical droplets is 4.4929 m²
Explanation:
From the information given :
assuming that :
30 cm³ of gasoline is atomized into N spherical droplets &
each with a radius of 2.0 × 10−5 m
We are tasked to determine the total surface area of these N spherical droplets
We all known that:
[tex]1 \ cm^3 = 10 ^{-6} m^3[/tex]
Therefore
[tex]30 \ cm^3 = 30 * 10 ^{-6} m^3 = 3 *1 0^{-5} \ m^3[/tex]
For each droplet; there is a required volume which is = [tex]\dfrac{4}{3} \pi r ^3[/tex] since it assumes a sphere shape .
Thus;
replacing radius(r) with 2.0 × 10−5 m; we have:
[tex]= \dfrac{4}{3} \pi * (2.0 *10^{-5} m) ^3[/tex]
= [tex]3.35 * 10^{-14} \ m^3[/tex]
However; there are [tex]3*10^{-5} \ m^3[/tex] gasoline atomized into N spherical droplets with each with radius 2.0 × 10−5 m
For N ; we have ;
[tex]=\dfrac{3*10^{-5} \ m^3}{3.35 * 10^{-14} \ m^3/ droplet}[/tex]
= [tex]8.95*10^8 \ droplet s[/tex]
So; each droplet have a surface area = [tex]4 \pi r^2[/tex]
= [tex]4 \pi (2.0*10^{-5}m) ^2[/tex]
= [tex]5.02*10^{-9} \ m^2/droplets[/tex]
The surface area per droplet is equivalent to [tex]5.02*10^{-9} \ m^2/droplets[/tex]
Thus;
The total surface area of these N spherical droplets will be :
= [tex]8.95*10^8 \ droplet s * 5.02*10^{-9} \ m^2/ droplets[/tex]
= 4.4929 m²
The total surface area of these N spherical droplets is 4.4929 m²
If 175mL of oxygen is produced at STP, how many grams of hydrogen peroxide, H2O2
were decomposed? At STP, 1 mole of gas occupies 22.4L. Be sure to balance first.
2 H202 > H202 + O2
what's the
Mass of H2O2
Answer:
0.53g
Explanation:
We'll begin by converting 175mL to L. This is illustrated below:
1000mL = 1L
Therefore 175mL = 175/1000 = 0.175L
Next, we shall calculate the number of mole of O2 that occupy 0.175L. This is illustrated below:
1 mole of O2 occupy 22.4L at stp.
Therefore, Xmol of O2 will occupy 0.175L i.e
Xmol of O2 = 0.175/22.4
Xmol of O2 = 7.81×10¯³ mole
Therefore, 7.81×10¯³ mole of O2 occupy 175mL.
Next, we shall determine the number of mole of H2O2 that decomposed to produce 7.81×10¯³ mole of O2. This is illustrated below:
2H2O2 —> 2H2O + O2
From the balanced equation above,
2 moles of H2O2 decomposed to produce 1 mole of O2.
Therefore, Xmol of H2O2 will decompose to produce 7.81×10¯³ mole of O2 i.e
Xmol of H2O2 = 2 x 7.81×10¯³
Xmol of H2O2 = 1.562×10¯² mole
Therefore, 1.562×10¯² mole of H2O2 decomposed in the reaction.
Finally, we shall convert 1.562×10¯² mole of H2O2 to grams. This is illustrated below:
Molar mass of H2O2 = (2x1) + (16x2) = 34g/mol
Mole of H2O2 = 1.562×10¯² mole
Mass of H2O2 =..?
Mole = mass /Molar mass
1.562×10¯² = mass /34
Cross multiply
Mass of H2O2 = 1.562×10¯² x 34
Mass of H2O2 = 0.53g
Therefore, 0.53g of Hydrogen peroxide, H2O2 were decomposition in the reaction.
Select the chemical equation that represents an acid base reaction??? Please help
Answer:
HCl + AgNO3 ------ AgCl + HNO3
Explanation:
HCl is an acid called hydrochloric acid, while AgNO3 is a base called Silver Nitrate.
Hope it helps.
A gas contained in a steel tank has a volume of 1.5 L at a temperature of 390 K. What will be the volume when the temperature changes to 1470C? Group of answer choices
Answer:
1.5 L
Explanation:
If the gas is contained in a steel tank, the volume will remain constant when the temperature changes.
The volume will be 1.5 L.
1) Aluminum sulphate can be made by the following reaction: 2AlCl3(aq) + 3H2SO4(aq) Al2(SO4)3(aq) + 6 HCl(aq) It is quite soluble in water, so to isolate it the solution has to be evpourated to dryness. This drives off the volatile HCl, but the residual solid has to be heated to a little over 200 oC to drive off all of the water. In one experiment, 25.0 g of 2AlCl3 was mixed with 30.0 g of H2SO4. Eventually, 28.46 g of pure Al2(SO4)3 was isolated. Calculate the percentage yield
Answer:
88.9%
Explanation:
Step 1:
The balanced equation for the reaction. This is given below:
2AlCl3(aq) + 3H2SO4(aq) —> Al2(SO4)3(aq) + 6HCl(aq)
Step 2:
Determination of the masses of AlCl3 and H2SO4 that reacted and the mass of Al2(SO4)3 produced from the balanced equation.
Molar mass of AlCl3 = 27 + (35.5x3) = 133.5g/mol
Mass of AlCl3 from the balanced equation = 2 x 133.5 = 267g
Molar mass of H2SO4 = (2x1) + 32 + (16x4) = 98g/mol
Mass of H2SO4 from the balanced equation = 3 x 98 = 294g
Molar mass of Al2(SO4)3 = (27x2) + 3[32 + (16x4)]
= 54 + 3[32 + 64]
= 54 + 3[96] = 342g/mol
Mass of Al2(SO4)3 from the balanced equation = 1 x 342 = 342g
Summary:
From the balanced equation above,
267g of AlCl3 reacted with 294g of H2SO4 to produce 342g of Al2(SO4)3.
Step 3:
Determination of the limiting reactant. This is illustrated below:
From the balanced equation above,
267g of AlCl3 reacted with 294g of H2SO4.
Therefore, 25g of AlCl3 will react with = (25 x 294)/267 = 27.53g of H2SO4.
From the calculations made above, we see that only 27.53g out 30g of H2SO4 given were needed to react completely with 25g of AlCl3.
Therefore, AlCl3 is the limiting reactant and H2SO4 is the excess.
Step 4:
Determination of the theoretical yield of Al2(SO4)3.
In this case we shall be using the limiting reactant because it will produce the maximum yield of Al2(SO4)3 since all of it is used up in the reaction.
The limiting reactant is AlCl3 and the theoretical yield of Al2(SO4)3 can be obtained as follow:
From the balanced equation above,
267g of AlCl3 reacted to produce 342g of Al2(SO4)3.
Therefore, 25g of AlCl3 will react to produce = (25 x 342) /267 = 32.02g of Al2(SO4)3.
Therefore, the theoretical yield of Al2(SO4)3 is 32.02g
Step 5:
Determination of the percentage yield of Al2(SO4)3.
This can be obtained as follow:
Actual yield of Al2(SO4)3 = 28.46g
Theoretical yield of Al2(SO4)3 = 32.02g
Percentage yield of Al2(SO4)3 =..?
Percentage yield = Actual yield /Theoretical yield x 100
Percentage yield = 28.46/32.02 x 100
Percentage yield = 88.9%
Therefore, the percentage yield of Al2(SO4)3 is 88.9%