Question 1 K 1 K 2 {( K 2 )/( K 1 )} {( K 1 )/( K 2 )} ( K 2 ) /( K 1 ) ( K 1 )(

Question

Question 1

K1 K2

{(K2)/(K1)}

{(K1)/(K2)}

(K2)/(K1)

(K1)(K2)

5 points   

Question 2

adding some S2Cl2 to the system.

adding some Cl2 to the system.

increasing the size of the reaction vessel.

decreasing the temperature of the reaction system.

adding some CCl4 to the system.

5 points   

Question 3

In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products?

5 points   

Question 4

Increase the volume of the reaction vessel.

Remove some NO.

Add some NOBr.

Remove some Br2.

Decrease the temperature.

5 points   

Question 5

1 only

2 only

3 only

1 and 2 only

1, 2, and 3

5 points   

Question 6

The rate law for a reaction is found to be Rate = k[A]2[B]. Which of the following mechanisms gives this rate law?

I only

II only

III only

two of these

none of these

5 points   

Question 7

step 1.

step 2.

step 3.

2 times step 2.

step 1 + step 2 + step 3.

5 points   

Question 8

For the reaction A + B + C ? products, the following initial-rate data were obtained.

[A]0 (mol/L)

[B]0 (mol/L)

[C]0 (mol/L)

Initial Rate (mol/(L s))

0.40

0.40

0.20

0.0160

0.20

0.40

0.40

0.0080

0.60

0.10

0.20

0.0015

0.20

0.10

0.20

0.0005

0.20

0.20

0.40

0.0020

What are the reaction orders with respect to A, B, and C, respectively?

1, 2, 0

0, 2, 1

0, 1, 1

1, 2, 1

1, 1, 1

5 points   

Question 9

The reaction A ? products is first-order in A. If the concentration of A is cut in half, the half-life of the reaction will

double.

decrease by a factor of 1/2.

decrease by a factor of 1/4.

remain constant.

quadruple.

5 points   

Question 10

The rate law for the reaction between chlorine and nitric oxide,2NO(g) + Cl2(g) ? 2NOCl(g)is Rate = k[NO]2[Cl2]. Which of the following changes will not alter the initial rate of the reaction?

decreasing the volume of the reaction system

running the reaction in a solvent rather than in the gas phase

increasing the volume of the reaction system

increasing the concentration of chlorine gas

increasing the concentration of NOCl

5 points   

Question 11

The rate law for the chemical reaction5Br(aq) + BrO3(aq) + 6H+(aq) ? 3Br2(aq) + 3H2O(l)has been determined experimentally to be Rate = k[Br][BrO3][H+]2. What is the overall order of the reaction?

1

2

3

4

5

5 points   

Question 12

Which of the following can we predict from an equilibrium constant for a reaction?1. The extent of a reaction2. Whether the reaction is fast or slow3. Whether the reaction is exothermic or endothermic

1 only

2 only

3 only

1 and 2 only

1 and 3 only

5 points   

Question 13

5 points   

Question 14

For the hypothetical first-order reaction A ? products, k = 0.0472 s-1. If the initial concentration of A is 0.671 M, how long would it take for A to be 81.8% consumed?

36.1 s

21.2 s

14.7 s

4.26 s

31.6 s

5 points   

Question 15

At a given temperature, a first-order reaction has a rate constant of 1.8 10-3 s-1. How long will it take for the reaction to be 64% complete?

250 s

250 s

2000 s

570 s

2300 s

5 points   

Question 16

3.50 102

3.01 105

3.32 104

1.20 104

2.86 101

5 points   

Question 17

For the reactionIO3(aq) + 5I(aq) + 6H+(aq) ? 3I2(aq) + 3H2O(l)the rate of disappearance of IO3(aq) at a particular time and concentration is 2.4 10-3 mol/(L s). What is the rate of appearance of I2(aq)?

7.2 10-3 mol/(L s)

2.4 10-3 mol/(L s)

7.2 10-3 mol/(L s)

8.0 10-3 mol/(L s)

1.3 10-3 mol/(L s)

5 points   

Question 18

1 only

2 only

1 and 2 only

2 and 3 only

1, 2, and 3

5 points   

Question 19

For the reaction:

A(g) + B(g) ? C(g)  ,    Kc =8.80x10-5

If the initial concentrion of A is 0.10 M and the initial concentration of B is 0.10 M,   what is the equilibrium concentration of C?

2.3 x10-8 M

8.8 x10-8 M

1.7 x10-7 M

8.8 x10-7 M

5 points   

Question 20

For the formation of 1 mol of nitrosyl chloride at a given temperature, ?H = 40 kJ.NO(g) + Cl2(g) ? NOCl(g)The activation energy for this reaction is 84 kJ/mol. What is the activation energy for the reverse reaction?

40 kJ/mol

44 kJ/mol

84 kJ/mol

124 kJ/mol

124 kJ/mol

5 points   

Question 21

The rate constants for the first-order decomposition of a compound are 5.48 104 s-1 at 41C and 3.13 103 s-1 at 62C. What is the value of the activation energy for this reaction? (R = 8.31 J/(mol K))

0.690 kJ/mol

72.5 kJ/mol

1.75 kJ/mol

0.761 kJ/mol

31.5 kJ/mol

K1 K2

{(K2)/(K1)}

{(K1)/(K2)}

(K2)/(K1)

(K1)(K2)

Question 1 Given the equilibrium constants for the following reactions: 4Cu(s) + O2(g) 2C2O(s); K1 4CuO(s) 2Cu2O(s) + O2(g); K2What is K for the system 2Cu(s) + O2(g) 2CuO(s)equivalent to? Question 2 Consider the reactionS2Cl2(l) + CCl4(l) CS2(g) + 3Cl2(g); ?H = 84.3 kJIf the above reactants and products are contained in a closed vessel and the reaction system is at equilibrium, the number of moles of CS2 can be increased by adding some S2Cl2 to the system. adding some Cl2 to the system. increasing the size of the reaction vessel. decreasing the temperature of the reaction system. adding some CCl4 to the system. Question 3 In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products? Question 4 For the following reaction system at equilibrium, which one of the changes below would cause the equilibrium to shift to the right?Br2(g) + 2NO(g) Question 5 Which of the following equilibria would be affected by volume changes at constant temperature?1. 2NO(g) + 3F2(g) 2F3NO(g)2. PCl3(g) + Cl2(g) PCl5(g)3. O3(g) + NO(g) NO2(g) + O2(g) 1 only 2 only 3 only 1 and 2 only 1, 2, and 3 Question 6 The rate law for a reaction is found to be Rate = k[A]^2[B]. Which of the following mechanisms gives this rate law?

Explanation / Answer

1){(K1)/(K2)}

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