Question 1

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, NO = 0.526 atm,   = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g)  + Br2(g)    2NOBr(g)  A)  7.45 × 10-3 B)  0.109 C)  9.18 D)  91.8 E)  134" class="answers-bank-image d-inline" rel="preload" > = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g)  + Br2(g)  NO = 0.526 atm,   = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g)  + Br2(g)    2NOBr(g)  A)  7.45 × 10-3 B)  0.109 C)  9.18 D)  91.8 E)  134" class="answers-bank-image d-inline" rel="preload" > 2NOBr(g)

Accepted Answer

A)   7.45 × 10-3
B)   0.109
C)   9.18
D)   91.8
E)   134F) A) and D)
G) A) and E)

Question 2

A good catalyst for a reaction will speed up the forward reaction and slow down the reverse reaction.

Accepted Answer

A) True 
 B)False

Question 3

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH 17H35COOH   (C17H35COOH) 2 H°rxn = -172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C. A)  4.7 × 105 B)  2.6 × 104 C)  1.9 × 103 D)  3.2 × 102 E)  18" class="answers-bank-image d-inline" rel="preload" > (C17H35COOH) 2 H°rxn = -172 kJ
The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

Accepted Answer

A)   4.7 × 105
B)   2.6 × 104
C)   1.9 × 103
D)   3.2 × 102
E)   18F) B) and E)
G) B) and D)

Question 4

At high temperatures, carbon reacts with O2 to produce CO as follows: C(s)  + O2(g)  2 to produce CO as follows: C(s)  + O2(g)      2CO(g) . When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction? A)  0.010 B)  0.072 C)  0.090 D)  0.17 E)  1.2" class="answers-bank-image d-inline" rel="preload" >  
2CO(g) .
When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?

Accepted Answer

A)   0.010
B)   0.072
C)   0.090
D)   0.17
E)   1.2F) A) and B)
G) B) and C)

Question 5

In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant Kc will also increase.

Accepted Answer

A) True 
 B)False

Question 6

Write the mass-action expression, Qc , for the following chemical reaction. Zn(s)  + 2Ag+(aq)  c , for the following chemical reaction. Zn(s)  + 2Ag+(aq)    Zn2+(aq)  + 2Ag(s)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > Zn2+(aq)  + 2Ag(s)

Accepted Answer

A)   c , for the following chemical reaction. Zn(s)  + 2Ag+(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   c , for the following chemical reaction. Zn(s)  + 2Ag+(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   c , for the following chemical reaction. Zn(s)  + 2Ag+(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   c , for the following chemical reaction. Zn(s)  + 2Ag+(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   c , for the following chemical reaction. Zn(s)  + 2Ag+(aq)    Zn2+(aq)  + 2Ag(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) B) and D)
G) C) and D)

Question 7

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3) 3COH(g)  3) 3COH(g)    (CH3) 2CCH2(g)  + H2O(g)  A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature? A)  The forward reaction will proceed to reestablish equilibrium. B)  The reverse reaction will proceed to reestablish equilibrium. C)  No change occurs. D)  The equilibrium constant will increase. E)  The equilibrium constant will decrease." class="answers-bank-image d-inline" rel="preload" > (CH3) 2CCH2(g)  + H2O(g) 
A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Accepted Answer

A)   The forward reaction will proceed to reestablish equilibrium.
B)   The reverse reaction will proceed to reestablish equilibrium.
C)   No change occurs.
D)   The equilibrium constant will increase.
E)   The equilibrium constant will decrease.F) B) and C)
G) C) and D)

Question 8

Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2)  CO(g)  + Cl2(g)  2)  CO(g)  + Cl2(g)      COCl2(g)  If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown. [CO] = [Cl2] = 0.010 M; [COCl2] = 0.070 M A)  The reaction will proceed to the right. B)  The reaction will proceed to the left. C)  The reaction is at equilibrium, and no change in concentrations will occur. D)  The container volume needs to be specified before a prediction can be made. E)  The temperature needs to be specified before a prediction can be made." class="answers-bank-image d-inline" rel="preload" >  
COCl2(g) 
If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.010 M; [COCl2] = 0.070 M

Accepted Answer

A)   The reaction will proceed to the right.
B)   The reaction will proceed to the left.
C)   The reaction is at equilibrium, and no change in concentrations will occur.
D)   The container volume needs to be specified before a prediction can be made.
E)   The temperature needs to be specified before a prediction can be made.F) A) and D)
G) A) and C)

Question 9

If Q > K, more products need to be formed as the reaction proceeds to equilibrium.

Accepted Answer

A) True 
 B)False

Question 10

SO2 reacts with O2 to produce SO3. If 86.0 g of SO2 is placed in a reaction vessel along with excess oxygen gas, how many moles of SO2 remain when 50.0 g of SO3 have been formed?

Accepted Answer

A)   0.56 mol
B)   0.62 mol
C)   0.72 mol
D)   0.78 mol
E)   1.34 molF) C) and D)
G) All of the above

Question 11

Sodium hydrogen carbonate decomposes above 110°C to form sodium carbonate, water, and carbon dioxide. 2NaHCO3(s)  3(s)    Na2CO3(s)  + H2O(g)  + CO2(g)  One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added? A)  The partial pressure of carbon dioxide will increase. B)  The partial pressure of carbon dioxide will decrease. C)  The partial pressure of carbon dioxide will be unchanged. D)  The amounts of all products will be greater when equilibrium is reestablished. E)  None of the above conclusions is justified without knowing the equilibrium constant." class="answers-bank-image d-inline" rel="preload" > Na2CO3(s)  + H2O(g)  + CO2(g) 
One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added?

Accepted Answer

A)   The partial pressure of carbon dioxide will increase.
B)   The partial pressure of carbon dioxide will decrease.
C)   The partial pressure of carbon dioxide will be unchanged.
D)   The amounts of all products will be greater when equilibrium is reestablished.
E)   None of the above conclusions is justified without knowing the equilibrium constant.F) B) and C)
G) B) and E)

Question 12

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s)  + CO2(g)  2(g)    NaHCO3(s)  H°rxn 2 gas present at equilibrium? A)  adding N2 gas to double the pressure B)  adding more solid NaOH C)  increasing the volume of the container D)  lowering the temperature E)  none of the above" class="answers-bank-image d-inline" rel="preload" > NaHCO3(s)  H°rxn 2 gas present at equilibrium?

Accepted Answer

A)   adding N2 gas to double the pressure
B)   adding more solid NaOH
C)   increasing the volume of the container
D)   lowering the temperature
E)   none of the aboveF) None of the above
G) B) and C)

Question 13

The following reaction, in CCl4 solvent, has been studied at 25°C. 2BrCl 4 solvent, has been studied at 25°C. 2BrCl   Br2  + Cl2 The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine? A)  1.35 × 10-3 M B)  2.70 × 10-3 M C)  8.82 × 10-3 M D)  9.70 × 10-2 M E)  none of the above" class="answers-bank-image d-inline" rel="preload" > Br2  + Cl2
The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?

Accepted Answer

A)   1.35 × 10-3 M
B)   2.70 × 10-3 M
C)   8.82 × 10-3 M
D)   9.70 × 10-2 M
E)   none of the aboveF) B) and D)
G) A) and D)

Question 14

Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?

Accepted Answer

A)   10.0 g hydrogen remains
B)   10.9 g hydrogen remains
C)   15.0 g hydrogen remains
D)   19.9 g hydrogen remains
E)   Need to know the equilibrium constant in order to calculate the answer.F) D) and E)
G) A) and B)

Question 15

The equilibrium constant Kc for the reaction PCl3(g)  + Cl2(g)  c for the reaction PCl3(g)  + Cl2(g)    PCl5(g)  Is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established? A)  0.049 M B)  0.11 M C)  0.30 M D)  0.59 M E)  0.83 M" class="answers-bank-image d-inline" rel="preload" > PCl5(g) 
Is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?

Accepted Answer

A)   0.049 M
B)   0.11 M
C)   0.30 M
D)   0.59 M
E)   0.83 MF) A) and B)
G) C) and E)

Question 16

Write the mass-action expression, Qc, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)  c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 12CO2(g)  + 6H2O(g)

Accepted Answer

A)   c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   c, for the following chemical reaction equation. 2C6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and B)
G) All of the above

Question 17

Ammonia is synthesized in the Haber process:
N2(g) + 3H2(g)  2NH3(g)
Kp for this reaction is 1.49 × 10-5 at 500.°C. Calculate Kc at this temperature.

Accepted Answer

Question 18

The equilibrium constant for reaction (1)  below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1)  2(g)  +   Y2(g)    XY(g)  (2)  2XY(g)    X2(g)  + Y2(g)  A)  6.02 × 10-2 B)  7.25 × 10-3 C)  3.62 × 10-3 D)  1.31 × 10-5 E)  none of the above" class="answers-bank-image d-inline" rel="preload" > X2(g)  + 2(g)  +   Y2(g)    XY(g)  (2)  2XY(g)    X2(g)  + Y2(g)  A)  6.02 × 10-2 B)  7.25 × 10-3 C)  3.62 × 10-3 D)  1.31 × 10-5 E)  none of the above" class="answers-bank-image d-inline" rel="preload" > Y2(g)  2(g)  +   Y2(g)    XY(g)  (2)  2XY(g)    X2(g)  + Y2(g)  A)  6.02 × 10-2 B)  7.25 × 10-3 C)  3.62 × 10-3 D)  1.31 × 10-5 E)  none of the above" class="answers-bank-image d-inline" rel="preload" > XY(g) 
(2)  2XY(g)  2(g)  +   Y2(g)    XY(g)  (2)  2XY(g)    X2(g)  + Y2(g)  A)  6.02 × 10-2 B)  7.25 × 10-3 C)  3.62 × 10-3 D)  1.31 × 10-5 E)  none of the above" class="answers-bank-image d-inline" rel="preload" > X2(g)  + Y2(g)

Accepted Answer

A)   6.02 × 10-2
B)   7.25 × 10-3
C)   3.62 × 10-3
D)   1.31 × 10-5
E)   none of the aboveF) B) and C)
G) A) and D)

Question 19

What is the mass-action expression, Qp, for the following reaction? SbF5(g)  + 4Cl2(g)  p, for the following reaction? SbF5(g)  + 4Cl2(g)    SbCl3(g)  + 5ClF(g)  A)    B)    C)    D)    E)  None of the above is the correct mass-action expression." class="answers-bank-image d-inline" rel="preload" > SbCl3(g)  + 5ClF(g)

Accepted Answer

A)   p, for the following reaction? SbF5(g)  + 4Cl2(g)    SbCl3(g)  + 5ClF(g)  
A)     
B)     
C)     
D)     
E)   None of the above is the correct mass-action expression." class="answers-bank-image d-inline" rel="preload" >
B)   p, for the following reaction? SbF5(g)  + 4Cl2(g)    SbCl3(g)  + 5ClF(g)  
A)     
B)     
C)     
D)     
E)   None of the above is the correct mass-action expression." class="answers-bank-image d-inline" rel="preload" >
C)   p, for the following reaction? SbF5(g)  + 4Cl2(g)    SbCl3(g)  + 5ClF(g)  
A)     
B)     
C)     
D)     
E)   None of the above is the correct mass-action expression." class="answers-bank-image d-inline" rel="preload" >
D)   p, for the following reaction? SbF5(g)  + 4Cl2(g)    SbCl3(g)  + 5ClF(g)  
A)     
B)     
C)     
D)     
E)   None of the above is the correct mass-action expression." class="answers-bank-image d-inline" rel="preload" >
E)   None of the above is the correct mass-action expression.F) C) and E)
G) B) and E)

Question 20

The reaction system CS2(g)  + 4H2(g)  2(g)  + 4H2(g)    CH4(g)  + 2H2S(g)  Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled? A)  As equilibrium is reestablished, the partial pressure of carbon disulfide increases. B)  As equilibrium is reestablished, the partial pressure of methane, CH4, decreases. C)  As equilibrium is reestablished, the partial pressure of hydrogen decreases. D)  As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases. E)  As equilibrium is reestablished, all the partial pressures will decrease." class="answers-bank-image d-inline" rel="preload" > CH4(g)  + 2H2S(g) 
Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

Accepted Answer

A)   As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B)   As equilibrium is reestablished, the partial pressure of methane, CH4, decreases.
C)   As equilibrium is reestablished, the partial pressure of hydrogen decreases.
D)   As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.
E)   As equilibrium is reestablished, all the partial pressures will decrease.F) A) and B)
G) B) and D)

Exam 17: Equilibrium: the Extent of Chemical Reactions

Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?

Correct Answer
verified

Ammonia is synthesized in the Haber process: N₂(g) + 3H₂(g) 2NH₃(g) K_p for this reaction is 1.49 × 10^-5at 500.°C. Calculate K_c at this temperature.

Correct Answer
verified

The equilibrium constant K_c for the reaction PCl₃(g) + Cl₂(g) PCl₅(g) Is 49 at 230°C. If 0.70 mol of PCl₃is added to 0.70 mol of Cl₂in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl₃when equilibrium has been established?

Correct Answer
verified

If Q > K, more products need to be formed as the reaction proceeds to equilibrium.

Correct Answer
verified

Write the mass-action expression, Q_c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) Zn²⁺(aq) + 2Ag(s)

Correct Answer
verified

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) H°_rxn < 0 Which, if any, of the following actions will decrease the concentration of CO₂ gas present at equilibrium?

Correct Answer
verified

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH₃) ₃COH(g) (CH₃) ₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Correct Answer
verified

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

Correct Answer
verified

Write the mass-action expression, Q_c, for the following chemical reaction equation. 2C₆H₆(g) + 15O₂(g) 12CO₂(g) + 6H₂O(g)

Correct Answer
verified

A good catalyst for a reaction will speed up the forward reaction and slow down the reverse reaction.

Correct Answer
verified

The reaction system CS₂(g) + 4H₂(g) CH₄(g) + 2H₂S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the mass-action expression, Q_p, for the following reaction? SbF₅(g) + 4Cl₂(g) SbCl₃(g) + 5ClF(g)

Correct Answer
verified

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C₁₇H₃₅COOH (C₁₇H₃₅COOH) ₂H°_rxn = -172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

Correct Answer
verified

Correct Answer
verified

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) X₂(g) + Y₂(g) XY(g) (2) 2XY(g) X₂(g) + Y₂(g)

Correct Answer
verified

The following reaction, in CCl₄ solvent, has been studied at 25°C. 2BrCl Br₂ + Cl₂ The equilibrium constant K_c is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?

Correct Answer
verified

SO₂ reacts with O₂ to produce SO₃. If 86.0 g of SO₂ is placed in a reaction vessel along with excess oxygen gas, how many moles of SO₂ remain when 50.0 g of SO₃ have been formed?

Correct Answer
verified

In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant K_c will also increase.

Correct Answer
verified

Exam 17: Equilibrium: the Extent of Chemical Reactions

Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?

Correct AnswerverifiedShow Answer

Ammonia is synthesized in the Haber process: N2(g) + 3H2(g) 2NH3(g) Kp for this reaction is 1.49 × 10-5 at 500.°C. Calculate Kc at this temperature.

Correct AnswerverifiedShow Answer

The equilibrium constant Kc for the reaction PCl3(g) + Cl2(g) PCl5(g) Is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?

Correct AnswerverifiedShow Answer

If Q > K, more products need to be formed as the reaction proceeds to equilibrium.

Correct AnswerverifiedShow Answer

Write the mass-action expression, Qc , for the following chemical reaction. Zn(s) + 2Ag+(aq) Zn2+(aq) + 2Ag(s)

Correct AnswerverifiedShow Answer

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO2(g) NaHCO3(s) H°rxn < 0 Which, if any, of the following actions will decrease the concentration of CO2 gas present at equilibrium?

Correct AnswerverifiedShow Answer

At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3) 3COH(g) (CH3) 2CCH2(g) + H2O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

Correct AnswerverifiedShow Answer

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g) + Br2(g) 2NOBr(g)

Correct AnswerverifiedShow Answer

Write the mass-action expression, Qc, for the following chemical reaction equation. 2C6H6(g) + 15O2(g) 12CO2(g) + 6H2O(g)

Correct AnswerverifiedShow Answer

A good catalyst for a reaction will speed up the forward reaction and slow down the reverse reaction.

Correct AnswerverifiedShow Answer

The reaction system CS2(g) + 4H2(g) CH4(g) + 2H2S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the mass-action expression, Qp, for the following reaction? SbF5(g) + 4Cl2(g) SbCl3(g) + 5ClF(g)

Correct AnswerverifiedShow Answer

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH (C17H35COOH) 2 H°rxn = -172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

Correct AnswerverifiedShow Answer

At high temperatures, carbon reacts with O2 to produce CO as follows: C(s) + O2(g) 2CO(g) . When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?

Correct AnswerverifiedShow Answer

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) X2(g) + Y2(g) XY(g) (2) 2XY(g) X2(g) + Y2(g)

Correct AnswerverifiedShow Answer

The following reaction, in CCl4 solvent, has been studied at 25°C. 2BrCl Br2 + Cl2 The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?

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SO2 reacts with O2 to produce SO3. If 86.0 g of SO2 is placed in a reaction vessel along with excess oxygen gas, how many moles of SO2 remain when 50.0 g of SO3 have been formed?

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In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant Kc will also increase.

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Ammonia is synthesized in the Haber process: N₂(g) + 3H₂(g) 2NH₃(g) K_p for this reaction is 1.49 × 10^-5at 500.°C. Calculate K_c at this temperature.

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The equilibrium constant K_c for the reaction PCl₃(g) + Cl₂(g) PCl₅(g) Is 49 at 230°C. If 0.70 mol of PCl₃is added to 0.70 mol of Cl₂in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl₃when equilibrium has been established?

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Write the mass-action expression, Q_c, for the following chemical reaction. Zn(s) + 2Ag⁺(aq) Zn²⁺(aq) + 2Ag(s)

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The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) H°_rxn < 0 Which, if any, of the following actions will decrease the concentration of CO₂ gas present at equilibrium?

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At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH₃) ₃COH(g) (CH₃) ₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

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Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

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Write the mass-action expression, Q_c, for the following chemical reaction equation. 2C₆H₆(g) + 15O₂(g) 12CO₂(g) + 6H₂O(g)

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The reaction system CS₂(g) + 4H₂(g) CH₄(g) + 2H₂S(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

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What is the mass-action expression, Q_p, for the following reaction? SbF₅(g) + 4Cl₂(g) SbCl₃(g) + 5ClF(g)

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Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C₁₇H₃₅COOH (C₁₇H₃₅COOH) ₂H°_rxn = -172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

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The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) X₂(g) + Y₂(g) XY(g) (2) 2XY(g) X₂(g) + Y₂(g)

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The following reaction, in CCl₄ solvent, has been studied at 25°C. 2BrCl Br₂ + Cl₂ The equilibrium constant K_c is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?

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SO₂ reacts with O₂ to produce SO₃. If 86.0 g of SO₂ is placed in a reaction vessel along with excess oxygen gas, how many moles of SO₂ remain when 50.0 g of SO₃ have been formed?

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In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant K_c will also increase.

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