Answer:
jdksyeuueueuueueuueueudyydheyehhdhdhdhdhhdhdhdhjjdj
what is the maximum number of electrons in p&q shell
Answer:
6 electrons
Explanation:
:)
hope this helps :))))))))
Answer:
each p shell can hold max. 6 electorns
i dont know what a q shell is
Write the chemical reaction for hydrogen thiocyanate in water, whose equilibrium constant is Ka. Include the physical states for each species
Write the chemical reaction for thiocyanate ion in water, whose equilibrium constant is Kb. Include the physical states for each species
Answer:
HSCN (aq) + H₂O(l) ⇄ SCN⁻(aq) + H₃O⁺(aq) Ka
SCN⁻ (aq) + H₂O(l) ⇄ HSCN (aq) + OH⁻(aq) Kb
Explanation:
We identify the formula:
HSCN → hydrogen thiocyanate which is also known as Thiocyanic acid
HSCN (aq) + H₂O(l) ⇄ SCN⁻(aq) + H₃O⁺(aq) Ka
As an acid, it gives proton to the solution. It is a weak acid, because the Ka
Ka = [SCN⁻] . [H₃O⁺] / [HSCN]
As a weak acid, the thiocyanate ion, will be the conjugate strong base. In water It can make hydrolisis:
SCN⁻ (aq) + H₂O(l) ⇄ HSCN (aq) + OH⁻(aq) Kb
As a base, it takes a proton from water.
Kb = [HSCN] . [OH⁻] / [SCN⁻]
H-S-C-N is the structure of hydro-thi-ocyanate.
H-S-C-N structure:1. combines with water, it produces the ion thiocyanate and the ion hydronium.
2. When thiocyanate combines with water, it produces the ion hydrogen thiocyanate and the ion hydroxy.
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Questlon 25 of 25
2 Points
Substitute 4 for xand evaluate the expression below.
3x+9x
Answer:
48
Explanation:
hi hope this helps
3*4+9*4
12+36
48
Lead forms two compounds with oxygen. One contains 2.98g of lead and 0.461g of oxygen. The other contains 9.89g of lead and 0.763g of oxygen. For a given mass of oxygen, what is the lowest whole-number mass ratio of lead in the two compounds
The given question is incomplete, the complete question is:
Lead forms two compounds with oxygen. One contains 2.98g of lead and 0.461g of oxygen. The other contains 9.89g of lead and 0.763g of oxygen. For a given mass of oxygen, what is the lowest whole-number mass ratio of lead in the two compounds that combines with a given mass of oxygen?
Answer:
The lowest whole-number mass ratio in the two compounds is 1:2.
Explanation:
There is a need to find the mole ratio between lead and oxygen atoms in order to find the whole-number mass ratio of lead in the two compounds. In the first compound, the given mass of lead is 2.98 grams, the molar mass of lead is 207.2 gram per mole.
The no. of moles can be determined by using the formula,
moles = mass/molecular mass
moles = 2.98 g/207.2 g/mol
= 0.0144 moles
The mass of oxygen in the compound I is 0.461 grams, the molecular mass of oxygen is 16 gram per mol.
moles = 0.461 g /16 g/mol
= 0.0288 moles
The ratio between the lead and oxygen in the compound I is 0.0144/0.0288 = 1:2
On the other hand, in the compound II, the mass of lead given is 9.89 grams, therefore, the moles of lead in compound II is,
moles = 9.89 g / 207.2 g/mol
= 0.0477 moles
The mass of oxygen given in compound II is 0.763 grams, the moles of oxygen present in the compound II is,
moles = 0.763 g / 16 g
= 0.0477 moles
The ratio between the lead and oxygen in the compound II is, 0.0477 moles lead /0.0477 moles oxygen = 1:1
Hence, of the two compounds, the lowest ratio is found in the compound I, that is, 1:2.
The temperature of 2.97 mol of a monatomic ideal gas is 511 K. The internal energy of this gas is doubled by the addition of heat. How much heat is needed when it is added at (a) constant volume and (b) constant pressure
Answer:
The heat needed when volume is constant is 18926.9 J
The heat needed when pressure is constant is 31544.8 J
Explanation:
Step 1: Data given
Number of moles of a monoatomic gas = 2.97 mol
Temperature of the gas = 511 K
The internal energy of this gas is doubled by the addition of heat.
Step 2:
At a constant volume workdone is 0.
Q = ΔU + W
Q = 3/2 n*R*T
⇒n = the number of moles = 2.97 moles
⇒R = the gas constant = 8.314 J/mol*K
⇒with T = the temperature = 511 K
Q = 3/2 *2.97 * 8.314 * 511
Q = 18926.9 J
Step 3: At a constant pressure workdone is:
W = p*V
W = n*R*T
⇒ Q = ΔU + W
Q = 3/2 *nRT + nRT
Q = 18926.9 + 2.97 * 8.314 * 511
Q = 31544.8 J
The heat needed when volume is constant is 18926.9 J
The heat needed when pressure is constant is 31544.8 J
What is the temperature, in degrees Celsius, of a substance with a temperature of 49K? –322°C –224°C 224°C 322°C
Answer:
-224ºC
Explanation:
Answer:
-224c
Explanation:
A volume of 105 mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water. If the final temperature of the system is 21.50 ∘C , what is the mass of the steel bar? Use the following values: specific heat of water = 4.18 J/(g⋅∘C) specific heat of steel = 0.452 J/(g⋅∘C) Express your answer to three significant figures and include the appropriate units.
Answer:
25.0 grams is the mass of the steel bar.Explanation:
Heat gained by steel bar will be equal to heat lost by the water
[tex]Q_1=-Q_2[/tex]
Mass of steel= [tex]m_1[/tex]
Specific heat capacity of steel = [tex]c_1=0.452 J/g^oC[/tex]
Initial temperature of the steel = [tex]T_1=2.00^oC[/tex]
Final temperature of the steel = [tex]T_2=T=21.50^oC[/tex]
[tex]Q_1=m_1c_1\times (T-T_1)[/tex]
Mass of water= [tex]m_2= 105 g[/tex]
Specific heat capacity of water=[tex]c_2=4.18 J/g^oC[/tex]
Initial temperature of the water = [tex]T_3=22.00^oC[/tex]
Final temperature of water = [tex]T_2=T=21.50^oC[/tex]
[tex]Q_2=m_2c_2\times (T-T_3)-Q_1=Q_2(m_1c_1\times (T-T_1))=-(m_2c_2\times (T-T_3))[/tex]
On substituting all values:
[tex](m_1\times 0.452 J/g^oC\times (21.50^o-2.00^oC))=-(105 g\times 4.18 J/g^oC\times (21.50^o-22.00^o))\\\\m_1*8.7914=241.395\\\\m_1=\frac{219.45}{8.7914} \\\\m_1=24.9\\\\ \approx25 \texttt {grams}[/tex]
25.0 grams is the mass of the steel bar.Answer:
[tex]m_{steel}=24.9g[/tex]
Explanation:
Hello,
In this case, since the water is initially hot, the released heat by it is gained by the steel rod since it is initially cold which in energetic terms is illustrated by:
[tex]\Delta H_{water}=-\Delta H_{steel}[/tex]
That in terms of mass, specific heat and temperature change is:
[tex]m_{water}Cp_{water}(T_f-T_{water})=-m_{steel}Cp_{steel}(T_f-T_{steel})[/tex]
Thus, we simply solve for the mass of the steel rod:
[tex]m_{steel}=\frac{m_{water}Cp_{water}(T_f-T_{water})}{-Cp_{steel}(T_f-T_{steel})} \\\\m_{steel}=\frac{105mL*\frac{1g}{1mL}*4.18\frac{J}{g\°C}*(21.50-22.00)\°C}{-0.452\frac{J}{g\°C}*(21.50-2.00)\°C} \\\\m_{steel}=24.9g[/tex]
Best regards.
For the reaction A+B↽−−⇀C+D, assume that the standard change in free energy has a positive value. Changing the conditions of the reaction can alter the value of the change in free energy (ΔG). Classify the conditions as to whether each would decrease the value of ΔG, increase the value of ΔG, or not change the value of ΔG for the reaction. For each change, assume that the other variables are kept constant.
A. Adding a catalystb.
B. Increasing [C] and [D]
C. Coupling with ATP hydrolysis
D. Increasing [A] and [B]
Explanation:
a. Adding a catalyst
no effect .( Catalyst can only change the activation energy but not the free energy).
b. increasing [C] and [D]
Increase the free energy .
c. Coupling with ATP hydrolysis
decrease the free energy value .
d.Increasing [A] and [B]
decrease the free energy.
A volume of 38.7 mL of H2O is initially at 28.0 oC. A chilled glass marble weighing 4.00 g with a heat capacity of 3.52 J/oC is placed in the water. If the final temperature of the system is 26.1 oC , what was the initial temperature of the marble? Water has a density of 1.00 g/mL and a specific heat of 4.18 J/goC. Enter your answer numerically, to three significant figures and in terms of oC.
Answer:
- 61.2°C = Initial T°
Explanation:
This is a calorimetry problem, where the heat from the water was gained by the marble.
Q = m . C . ΔT
where ΔT is final T° - initial T°, C is the specific heat and m, mass.
By the volume of water, we realize the mass (we apply density):
1 g/mL = mass / 38.7 mL
38.7 g = mass of water
Now, we need to find out the specific heat for the marble and we have Heat Capacity data
Heat Capacity = C . m
3.52 J/°C / 4 g = C → specific heat → 0.88 J/g °C
We make the equations for both heats:
m . C . ΔT from water = m . C . ΔT from the marble
38.7 g . 4.18 J/g°C ( 26.1°C - 28°C) = 4 g . 0.88 J/g °C . (26.1°C - Initial T°)
307.35 J = 4 g . 0.88 J/g °C . (26.1°C - Initial T°)
- 307.35 is a negative value, because the was has decreased the temperature, is a loss of heat, but we have to work with the positive number.
307.35 J / (4 . 0.88 °C/J) = 26.1°C - Initial T°
87.32°C = 26.1°C - Initial T°
- 61.2°C = Initial T°
A 3.3 g sample of sodium hydrogen carbonate is added to a solution of acetic acid weighing 10.3 g. The two substances react, releasing carbon dioxide gas to the atmosphere. After the reaction, the contents of the reaction vessel weigh 12.1 g. What is the mass of carbon dioxide released during the reaction
Answer:
1.73g of CO2.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is given below:
NaHCO3 + CH3COOH → CH3COONa + H2O + CO2
Next we shall determine the masses of NaHCO3 and CH3COOH that reacted and the mass of CO2 produced from the balanced equation. This is illustrated below:
Molar mass of NaHCO3 = 23 + 1 + 12 + (16x3) = 84g/mol
Mass of NaHCO3 from the balanced equation = 1 x 84 = 84g
Molar mass of CH3COOH = 12 + (3x1) + 12 + 16 + 16 + 1 = 60g/mol
Mass of CH3COOH from the balanced equation = 1 x 60 = 60g
Molar mass of CO3 = 12 + (2x16) = 44g/mol
Mass of CO2 from the balanced equation = 1 x 44 = 44g
From the balanced equation above,
84g of NaHCO3 reacted with 60g of CH3COOH to produce 44g of CO2.
Next, we shall determine the limiting reactant of the reaction. This is illustrated below:
From the balanced equation above,
84g of NaHCO3 reacted with 60g of CH3COOH.
Therefore, 3.3g of NaHCO3 will react with = (3.3 x 60)/84 = 2.36g of CH3COOH.
From the above illustration, we can see that only 2.36g of CH3COOH out of 10.3g given reacted completely with 3.3g of NaHCO3. Therefore, NaHCO3 is the limiting reactant while CH3COOH is the excess reactant.
Finally, can determine the mass of CO2 produced during the reaction.
In this case the limiting reactant will be used because it will produce the mass yield of CO2 as all of it were used up in the reaction. The limiting reactant is NaHCO3 and the mass of CO2 produced is obtained as shown below:
From the balanced equation above,
84g of NaHCO3 reacted to produce 44g of CO2.
Therefore, 3.3g of NaHCO3 will react to produce = (3.3 x 44)/84 = 1.73g of CO2.
Therefore, 1.73g of CO2 is released during the reaction.
The difference in the water levels of a beaker holding an upside-down buret containing a pocket of hydrogen gas is 23 cm H2O. What is the difference in pressure (pressure correction factor) between the atmospheric pressure and the pressure inside the buret? Express this in torr.
Answer:
Pressure difference = 16.9 torr
Explanation:
The formula to be used since their is a difference in water level in the beaker and burette is;
Atmospheric pressure = pressure of gas in burette + pressure of water
Atmospheric pressure - gas pressure = pressure of water
Therefore, the difference between atmospheric pressure and gas pressure can be seen to be the pressure of the water
The pressure of water in mmHg = 23 cm H20 = 230 mmH2O
To convert to mmHg, we have to divide by 13.6 since mercury is 13.6 times heavier than water.
Pressure of water = 230 mmH2O * (1 mmHg/13.6 mmH20) = 16.9 mmHg
Since I mmHg = 1 torr, therefore,
Pressure difference = 16.9 torr
The partial pressure of CO2 gas above the liquid in a carbonated drink is 0.45 atm. Assuming that the Henry's law constant for CO2 in the drink is that same as that in water, 3.7 x 10-2 mol/L atm, calculate the solubility of carbon dioxide in this drink.
Answer:
[tex]M_{CO_2}=0.01665M[/tex]
Explanation:
Hello,
In this case, the Henry's law allows us to relate the molar concentration and partial pressure of a solute (carbon dioxide) in a solution (solvent is water) by:
[tex]M_{CO_2}=H_{CO_2}p_{CO_2}[/tex]
Whereas we introduce the Henry constant, therefore, we can easily compute the molar solubility by:
[tex]M_{CO_2}=p_{CO_2}*H_{CO_2} =0.45atm*3.7x10^{-2}\frac{M}{atm}\\\\M_{CO_2}=0.01665M[/tex]
Regards.
Amino acids are the building blocks of proteins. The simplest amino acid is glycine . Draw a Lewis structure for glycine. (Hint: The central atoms in the skeletal structure are nitrogen bonded to carbon which is bonded to another carbon. The two oxygen atoms are bonded directly to the right-most carbon atom.
Answer:
Sorry for the lack of precision, if you have any questions you can consult me again.
Explanation:
Glycine is an amino acid, forms proteins and is also called in its molecular chemical formula as C2H5NO2
From the given electron configurations, predict which one is for a representative element?
A) 1s22s22p63s23p64s2
B) 1s22s22p63s23p63d74s2
C) 1s22s22p63s23p63d64s2
D) 1s22s22p63s23d5
From the given electron configurations, predict which one is for a representative element is 1s₂, 2s₂, 2p₆,3s₂, 3p₆, 3d₆, 4s₂.
What is element ?A chemical element is a species of atoms, including the pure material made entirely of that species, that have a specific number of protons in their nuclei. Chemical elements, unlike chemical compounds, cannot be reduced by any chemical process into simpler molecules.
The most basic form of a material is an element. In general, it cannot be streamlined or divided into smaller parts. A component of an element is an atom. A certain element only has one kind of atom per atom. Protons, neutrons, and electrons, which are subatomic particles, make up atoms.
We begin by applying the aufbau principle to the prediction of the electron configuration of an atom. It instructs us to fill the lowest energy accessible orbital, one electron at a time. It operates through element 18 (argon) in a filling pattern that is simple to predict: 1s, 2s, 2p, 3s, then 3p.
Thus, option C is correct.
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Which of the following is a buffer system? Which of the following is a buffer system? H2CO3(aq) and KHCO3(aq) NaCl(aq) and NaOH(aq) H2O(l) and HCl(aq) HCl(aq) and NaOH(aq) NaCl(aq) and NaNO3(aq)
Answer:
Explanation:
A buffer is defined as an aqueous mixture of a weak acid and its conjugate base or vice versa.
In the systems:
H₂CO₃(aq) and KHCO₃(aq): Carbonic acid, H₂CO₃, is a weak acid that, in solution with its conjugate pair, HCO₃⁻ make a buffer system.
NaCl(aq) and NaOH(aq): NaCl is a salt and NaOH is a strong base. Thus, this system is not a buffer system.
H₂O(l) and HCl(aq): Water is a solvent and HCl a strong acid. This is not a buffer system.
HCl(aq) and NaOH(aq): HCl is a strong acid and NaOH a strong base. This is not a buffer system.
NaCl(aq) and NaNO₃(aq): Both NaCl and NaNO₃ are salts and this system is not a buffer system.
Among the available buffer systems are [tex]\rm H_2CO_3[/tex](aq) and [tex]\rm KHCO_3[/tex](aq) solution. Therefore, the correct option is option A.
In an aqueous solution, a buffer system consists of a weak acid and its conjugate base (or a weak base and its conjugate acid). [tex]\rm H_2CO_3[/tex] (carbonic acid) is a weak acid in this example, and [tex]\rm KHCO_3[/tex] (potassium bicarbonate) is its conjugate base. When mixed in solution, they can resist pH changes by receiving or donating protons, thereby helping to keep the solution's acidity or alkalinity within a specific range.
NaCl(aq) and NaOH(aq): This is a salt and a strong base together. It is not a buffer system because it lacks a weak acid and its conjugate base.[tex]\rm H_2O[/tex](l) and HCl(aq): A mixture of water and a strong acid. It is not a buffer system because it lacks a weak acid and its conjugate base.A strong acid and a strong base are combined in HCl(aq) and NaOH(aq). It is not a buffer system because it lacks a weak acid and its conjugate base.This is a mixture of two salts, NaCl(aq) and [tex]\rm NaNO_3[/tex](aq). It does not include a weak acid and its conjugate base, hence it is not a weak acid.Therefore, the correct option is option A.
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In one experiment, magnesium metal melts. In a second experiment, magnesium metal ignites as it combines with oxygen. Classify the change in each experiment as chemical or physical. Explain your reasoning.
Answer:
magnesium metal melts = physical change
magnesium metal ignites = chemical change
Explanation:
Physical changes are those in which the identity of the subtance remains unaltered. No new compounds are formed. They involve generally changes in agreggation states of matter: solid, liquid or gas. The first experiment, in which magnesium metal melts is a physical change because it only changes the state of matter, from solid to liquid, but it is still magnesium metal.
Conversely, chemical changes involve atoms combinations to form new compounds. The second experiment, in which magnesium metal ignites, is a chemical change. After the change, magnesium metal is no longer the metal but a metal oxide.
Which image best represents the particles in liquids
Answer:
The 2nd Picture represents the particles in liquids.
Explanation:
For some hypothetical metal, the equilibrium number of vacancies at 600°C is 1 × 1025 m-3. If the density and atomic weight of this metal are 7.40 g/cm3 and 85.5 g/mol, respectively, calculate the fraction of vacancies for this metal at 600°C. Enter your answer using scientific notation.
Answer:
fraction of vacancies for this metal FV = 1.918*10⁻⁴
Explanation:
Given:
The number of vacancies per unit volume => ( Nv = 1*10²⁵ m⁻³ )
But we know that Avogrado's constant NA = 6.022*10²³ atoms/mol
Density of the material is given in g/cm3 we need to convert it to g/m³
Density of material ( p ) in g/m³ :
To convert we know that
1 g/cm³ = 1000000 g/m³ then
7.40 * ( 1000000 ) = 7.40*10⁶ g/m³
So, Density of material ( p ) in g/m³ = 7.40*10⁶ g/m³
Given Atomic mass = 85.5 g/mol
To Calculate the number of atomic sites per unit volume , we will use the below formula by substituting those values above
N = NA * p / A
N = ( 6.022*10²³ ) * ( 7.40*10⁶ ) / 85.5
N = 4.45*10³⁰ / 85.5
N = 5.212*10²⁸ atoms/m³
We can now Calculate the fraction of vacancies using the formula below;
Fv = Nv / N
Fv = 1*10²⁵ / 5.212*10²⁸
fraction of vacancies for this metal at 600c.= 1.918*10⁻⁴
Compounds A and B (both C10H14) show prominent peaks in their mass spectrum at m/z 134 and 119. Compound B also shows a less prominent peak at m/z 91. On vigorous oxidation with chromic acid, compound A is nonreactive while compound B yielded terephthalic acid.
From this information, deduce the structures of both compounds, and then draw the structure of B.
You do not have to consider stereochemistry
You do not have to explicitly draw H atoms
Answer:
1-methyl-4-propylbenzene
Explanation:
In this case, we have several clues that can help.
1) We have the production of terephthalic acid for compound B
2) The mass spectrometry info.
With the first clue, we can deduce that the initial molecule has a benzene ring and that in this ring we have alky groups bonded in para position. Additionally, we have to add 4 more carbons if we want to obtain the mass of the compound (134).
So, the question is ¿How we have to add these carbons? To answer this we have to check the mass spectrometry info. In this case, we have a mass in 119, therefore we have a loss of 15 m/z, this indicates that we have a methyl group. Also, we have a mass on 91, this can be explain as a loss of a propyl group. If we take into account that we have to have these groups on para position (due to the first clue) we will have a 1-methyl-4-propylbenzene. (See figure 1)
For molecule A we only know that we dont have any benzene ring because it doesn't react with the chromic acid. So, probably we will have a linear structure on which we have several double or triples bonds. Or we can have several rings that fit with the molecular mass. We will need more information for structure A.
I hope it helps!
gas syringe
bung
chips
25 cm of dilute
hydrochloric acid
Which channes slow down the rate of reaction?
Decrease the size of pieces of marble chips
Decrease surface area of marble chips
Inercase concentration of acid
Increase temperature of acid
Answer:
Decrease surface area of marble chips.
Explanation:
Because the reaction goes on the surface of marble chips, decreasing surface area of marble chips will decrease(slow down) the rate of the reaction.
The volume of an ideal gas is held constant. Determine the ratio P2/P1 of the final pressure to the initial pressure when the temperature of the gas rises (a) from 48 to 96 K and (b) from 26.0 to 68.7 oC.
Answer:
A. 2
B. 1.14
Explanation:
A. Data obtained from the question include:
Initial temperature (T1) = 48K
Final temperature (T2) = 96K
Final pressure (P2)/initial pressure (P1) =?
Since the volume is constant, we shall determine the ratio of final pressure to initial pressure (P2/P1) by applying the following equation:
P1/T1 = P2/T2
P1/48 = P2 /96
Cross multiply
48 x P2 = P1 x 96
Divide both side by 48
P2 = P1 x 96/48
Divide both side P1
P2/P1 = 96/48
P2/P1 = 2
Therefore, the ratio of final pressure to the initial pressure is 2
B. Data obtained from the question include:
Initial temperature (T1) = 26°C = 26°C + 273 = 299K
Final temperature (T2) = 68.7°C = 68.7°C + 273 = 341.7K
Final pressure (P2)/initial pressure (P1) =?
Since the volume is constant, we shall determine the ratio of final pressure to initial pressure (P2/P1) by applying the following equation:
P1/T1 = P2/T2
P1/299 = P2 /341.7
Cross multiply
299 x P2 = P1 x 341.7
Divide both side by 299
P2 = P1 x 341.7/299
Divide both side P1
P2/P1 = 341.7/299
P2/P1 = 1.14
Therefore, the ratio of final pressure to the initial pressure is 1.14
Question
2 Points
An object in a fluid will sink if:
A. the buoyant force is larger than the weight of the object.
B. the buoyant force is larger than the mass of the object.
C. the buoyant force is smaller than the weight of the object.
D. the buoyant force is smaller than the mass of the object.
SUBM
Answer:
c
Explanation:
when the weight of the object is greater than the buoyant force sinking is occurred.
Determine the hydroxide ion concentration in a solution that is: 1 × 10-4 M HCl. (kw = 1.0 X10-14)
Answer: The hydroxide ion concentration in a solution is [tex]1\times 10^{10}M[/tex]
Explanation:
pH or pOH is the measure of acidity or alkalinity of a solution.
pH is calculated by taking negative logarithm of hydrogen ion concentration.
[tex]pH=-\log [H^+][/tex]
[tex]HCl\rightarrow H^++Cl^{-}[/tex]
According to stoichiometry,
1 mole of [tex]HCl[/tex] gives = 1 mole of [tex]H^+[/tex]
Thus [tex]1\times 10^{-4}[/tex] moles of [tex]HCl[/tex] gives =[tex]\frac{1}{1}\times 1\times 10^{-4}=1\times 10^{-4}[/tex] moles of [tex]H^+[/tex]
[tex]K_w=[H^+][OH^-][/tex]
[tex]10^{-14}=[1\times 10^{-4}][OH^-][/tex]
[tex][OH^-]=1\times 10^{10}M[/tex]
Thus the hydroxide ion concentration in a solution is [tex]1\times 10^{10}M[/tex]
A solution has a hydrogen ion (or hydronium ion) concentration of 1.00×10−9 M.
What is the pH of the solution?
7.5
8.0
8.5
9.0
Why are covalent substances gases and liquid rather than solids?
Covalent compounds are held together with an intra molecular attraction which is weaker than metallic bond
hence covalent compounds exist as liquids, gases and soft solids
A 4.215 g sample of a compound containing only carbon, hydrogen, and oxygen is burned in an excess of oxygen gas, producing 9.582 g CO2 and 3.922 g H2O. What percent by mass of oxygen is contained in the original sample?
Answer:
[tex]\% O=27.6\%[/tex]
Explanation:
Hello,
In this case, for the sample of the given compound, we can compute the moles of each atom (carbon, hydrogen and oxygen) that is present in the sample as shown below:
- Moles of carbon are contained in the 9.582 grams of carbon dioxide:
[tex]n_C=9.582gCO_2*\frac{1molCO_2}{44gCO_2}*\frac{1molC}{1molCO_2} =0.218molC[/tex]
- Moles of hydrogen are contained in the 3.922 grams of water:
[tex]n_H=3.922gH_2O*\frac{1molH_2O}{18gH_2O} *\frac{2molH}{1molH_2O} =0.436molH[/tex]
- Mass of oxygen is computed by subtracting both the mass of carbon and hydrogen in carbon dioxide and water respectively from the initial sample:
[tex]m_O=4.215g-0.218molC*\frac{12gC}{1molC} -0.436molH*\frac{1gH}{1molH} =1.163gO[/tex]
Finally, we compute the percent by mass of oxygen:
[tex]\% O=\frac{1.163g}{4.215g}*100\% \\\\\% O=27.6\%[/tex]
Regards.
A buffered solution has a pH of 7.5. What would happen to the pH if a small
amount of acid were added?
Answer:
Dear user,
Answer to your query is provided below
When small amount of acid was added to buffered solution, pH will change very less.
Explanation:
Buffer solution resists change in ph on adding small amount of acid or base but when we calculate the value of buffer capacity we take the change in ph when we add acid or base to 1 lit solution of buffer.This contradicts the definition of buffer solution.
What are three things that
living things need to live?
Answer:
Water, air, and food.
Explanation:
All living things need air water and food to live.
Answer:
the first the Question is what do you need to live then that your answer
food,water,air ;]
What is the density (in g/L) of a gas with
a molar mass of 32.49 g/mol at
2.569 atm and 458 K?
Answer:
2.22 g/L
Explanation:
There's a relationship using the ideal gas law between molar mass and density: [tex]MM=\frac{dRT}{P}[/tex], where MM is the molar mass, d is the density, R is the gas constant, T is the temperature, and P is the pressure.
We know from the problem that MM = 32.49 g/mol, T = 458 Kelvin, and P = 2.569 atm. The gas constant, R, in terms of the units atm and Kelvin is 0.08206. Let's substitute these values into the formula:
[tex]MM=\frac{dRT}{P}[/tex]
[tex]32.49g/mol=\frac{d*0.08206*458K}{2.569atm}[/tex]
Solve for d:
d * 0.08206 * 458 K = 32.49 * 2.569
d = (32.49 * 2.569) / (0.08206 * 458 K) ≈ 2.22 g/L
The answer is thus 2.22 g/L.
~ an aesthetics lover
Answer:
2.22 g/L
Explanation:
1- Alum used in cooking is potassium aluminum sulfate hydrate, KAl(SO4)2. XH2O. To find the value of X, you can heat the sample of compound. Assume you heat 4.74 g of the hydrated compound and that sample loses 2.16 g of water. What is the value of X
Answer:
THE VALUE OF X IS 7 AND THE FORMULA OF THE HYDRATED SALT IS KAl(SO4)2.7H20
Explanation:
1. write out the varibales given in thequestion:
Mass of the hydrated salt = 4.74 g
Mass of water lost = 2.16 g
Formula of the hydrated salt = KAl(SO4)2. XH20
2. calculate the molar mass of the salt and that of water of crystallization:
Molar mass of anhydrous salt = ( K = 39, Al = 27, S = 32, 0=16)
= ( 39 + 27 + 32*2 + 16 * 8
= (39 + 27 + 64 + 128)
= 258 g/mol
Molar mass of water = 18 g/mol
3. Use this expression to calculate X:
The expression,
XH20 / molar mass of anhydrous salt = Mass of water lost / Mass of hydrated salt.
X = molar mass of anhydrous salt * mass of water lost / mass of anhydrous salt * H20
where XH20 is the molar mass of water of crystallization, is used to calculate the value of X.
4. Solve for X:
So therefore:
X = 258 * 2.16 / 4.74 * 18
X = 557.28/ 85.32
X = 6.53
X is approximately 7.
The value of X is 7 and the formula pf the hydrated salt is KAl(SO4)2.7H20
The value of X in the potassium aluminum sulfate hydrate, KAl(SO₄)₂.XH₂O is 12
From the question given above, the following data were obtained:
Mass of KAl(SO₄)₂.XH₂O = 4.74 g
Mass of water = 2.16 g
Value of X =?Next, we shall determine the mass of KAl(SO₄)₂.Mass of KAl(SO₄)₂.XH₂O = 4.74 g
Mass of H₂O = 2.16 g
Mass of KAl(SO₄)₂ = 4.74 – 2.16
Mass of KAl(SO₄)₂ = 2.58 gFinally, we shall determine the formula of the compound in order to obtain the value of X. This is illustrated below:Molar mass of KAl(SO₄)₂ = 39 + 27 + 2[32 + (4×26)] = 258 g/mol
Molar mass of H₂O = (2×1) + 16 = 18 g/mol
Mass of KAl(SO₄)₂ = 2.58 g
Mass of H₂O = 2.16 g
Divide by their molar mass
KAl(SO₄)₂ = 2.58 / 258 = 0.01
H₂O = 2.16 / 18 = 0.12
Divide by the smallest
KAl(SO₄)₂ = 0.01 / 0.01 = 1
H₂O = 0.12 / 0.01 = 12
Thus, the formula of the compound is KAl(SO₄)₂.12H₂O
Comparing KAl(SO₄)₂.12H₂O with KAl(SO₄)₂.XH₂O, the value of X is 12
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