Question 1

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 mol L-1.What is the rate constant for this reaction?

Accepted Answer

A) 1.0 × 10-2 L mol-1 s-1 
B) 4.5 × 10-2 L mol-1 s-1 
C) 9.7 × 10-2 L mol-1 s-1 
D) 2.2 × 10-2 L mol-1 s-1 
E) 3.8 × 10-2 L mol-1 s-1 
A) 1.0 × 10-2 L mol-1 s-1 
B) 4.5 × 10-2 L mol-1 s-1 
C) 9.7 × 10-2 L mol-1 s-1 
D) 2.2 × 10-2 L mol-1 s-1 
E) 3.8 × 10-2 L mol-1 s-1

Question 2

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 L mol-1 s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 mol L-1?

Accepted Answer

A) 4.55 mol L-1 
B) 0.258 mol L-1 
C) 3.87 mol L-1 
D) 2.20 mol L-1 
E) 2.39 mol L-1 
A) 4.55 mol L-1 
B) 0.258 mol L-1 
C) 3.87 mol L-1 
D) 2.20 mol L-1 
E) 2.39 mol L-1

Question 3

Given the following balanced equation,determine the rate of reaction with respect to [O2].If the rate of formation of O2 is 6.94 × 10-1 mol L-1 s-1,what is the rate of the loss of O3? 
2O3(g)→ 3O2(g)

Accepted Answer

A) 0.463 mol L-1 s-1 
B) 1.04 mol L-1 s-1 
C) 2.08 mol L-1 s-1 
D) 0.231 mol L-1 s-1 
E) 4.16 mol L-1 s-1 
A) 0.463 mol L-1 s-1 
B) 1.04 mol L-1 s-1 
C) 2.08 mol L-1 s-1 
D) 0.231 mol L-1 s-1 
E) 4.16 mol L-1 s-1

Question 4

Given the following balanced equation,determine the rate of reaction with respect to [SO3]. 
2SO2(g)+ O2(g)? 2SO3(g)

Accepted Answer

A) Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \mathrm { D } t }$ 
B) Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \Delta t }$ 
C) Rate = - $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \mathrm { D } t }$ 
D) Rate = + $\frac { 2 \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \Delta t }$ 
E) It is not possible to determine the answer without more information. 
A) Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \mathrm { D } t }$ 
B) Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \Delta t }$ 
C) Rate = - $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \mathrm { D } t }$ 
D) Rate = + $\frac { 2 \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \Delta t }$ 
E) It is not possible to determine the answer without more information.

Question 5

If a reaction carried out at 61 °C has an activation energy,Ea, of 67.3 kJ mol-1,a rate constant of 791 s-1,and a frequency factor,A,of 2.65 × 1013,what is the value of R? 
$k = A e ^ { \frac { - E _ { a } } { R T } }$

Accepted Answer

A) 0.08314 J mol-1 K-1 
B) 2.62 J mol-1 K-1 
C) 0.08206 J mol-1 K-1 
D) 9.51 J mol-1 K-1 
E) 8.314 J mol-1 K-1 
A) 0.08314 J mol-1 K-1 
B) 2.62 J mol-1 K-1 
C) 0.08206 J mol-1 K-1 
D) 9.51 J mol-1 K-1 
E) 8.314 J mol-1 K-1

Question 6

What data should be plotted to show that experimental concentration data fit a zeroth-order reaction?

Accepted Answer

A) ln[reactant] vs.time 
B)  $\frac { 1 } { [ \text { reactant] } }$ vs.time 
C) ln(k)vs. $\frac { 1 } { T }$ 
D) ln(k)vs.Ea 
E) [reactant] vs.time 
A) ln[reactant] vs.time 
B)  $\frac { 1 } { [ \text { reactant] } }$ vs.time 
C) ln(k)vs. $\frac { 1 } { T }$ 
D) ln(k)vs.Ea 
E) [reactant] vs.time

Question 7

Define activation energy.

Accepted Answer

The activation energ

Question 8

Identify a heterogeneous catalyst.

Accepted Answer

A) CFCs with ozone 
B) Pd in H2 gas 
C) KI dissolved in H2O2 
D) H2SO4 with concentrated HCl 
E) H3PO4 with an alcohol 
A) CFCs with ozone 
B) Pd in H2 gas 
C) KI dissolved in H2O2 
D) H2SO4 with concentrated HCl 
E) H3PO4 with an alcohol

Question 9

Given the following balanced equation,determine the rate of reaction with respect to [SO3].If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1,what is the rate of formation of SO3? 
2SO2(g)+ O2(g)→ 2SO3(g)

Accepted Answer

A) 3.56 × 10-3 mol L-1 s-1 
B) 1.19 × 10-3 mol L-1 s-1 
C) 1.78 × 10-3 mol L-1 s-1 
D) 1.42 × 10-2 mol L-1 s-1 
E) 7.12 × 10-3 mol L-1 s-1 
A) 3.56 × 10-3 mol L-1 s-1 
B) 1.19 × 10-3 mol L-1 s-1 
C) 1.78 × 10-3 mol L-1 s-1 
D) 1.42 × 10-2 mol L-1 s-1 
E) 7.12 × 10-3 mol L-1 s-1

Question 10

Given the following balanced equation,determine the rate of reaction with respect to [H2]. 
N2(g)+ 3H2(g)? 2NH3(g)

Accepted Answer

A) Rate = +$\frac { 3 \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
B) Rate = - $\frac { 2 } { 3 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
C) Rate = + $\frac { 3 } { 2 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
D) Rate = - $\frac { 1 } { 3 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
E) It is not possible to determine the answer without more information. 
A) Rate = +$\frac { 3 \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
B) Rate = - $\frac { 2 } { 3 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
C) Rate = + $\frac { 3 } { 2 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
D) Rate = - $\frac { 1 } { 3 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$ 
E) It is not possible to determine the answer without more information.

Question 11

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation: 
2HI(g)→ H2(g)+ I2(g)
At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 mol L-1 to 3.50 × 10-2 mol L-1.What is the rate constant for the reaction at this temperature?

Accepted Answer

A) 5.12 × 10-4 L mol-1 s-1 
B) 9.69 × 10-2 L mol-1 s-1 
C) 10.3 L mol-1 s-1 
D) 1.95 × 103 L mol-1 s-1 
A) 5.12 × 10-4 L mol-1 s-1 
B) 9.69 × 10-2 L mol-1 s-1 
C) 10.3 L mol-1 s-1 
D) 1.95 × 103 L mol-1 s-1

Question 12

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? 
Rate = k [X][Y]2

Accepted Answer

A) The rate of reaction will increase by a factor of 2. 
B) The rate of reaction will increase by a factor of 4. 
C) The rate of reaction will increase by a factor of 5. 
D) The rate of reaction will decrease by a factor of 2. 
E) The rate of reaction will remain unchanged. 
A) The rate of reaction will increase by a factor of 2. 
B) The rate of reaction will increase by a factor of 4. 
C) The rate of reaction will increase by a factor of 5. 
D) The rate of reaction will decrease by a factor of 2. 
E) The rate of reaction will remain unchanged.

Question 13

What is the activation energy for a reaction that has a rate constant of 5.68 × 10-8 s-1 at 298 K and 1.73 × 10-5 s-1 at 348 K?

Accepted Answer

A) 66.2 kJ mol-1 
B) 98.6 kJ mol-1 
C) 19.4 kJ mol-1 
D) 41.4 kJ mol-1 
E) 70.0 kJ mol-1 
A) 66.2 kJ mol-1 
B) 98.6 kJ mol-1 
C) 19.4 kJ mol-1 
D) 41.4 kJ mol-1 
E) 70.0 kJ mol-1

Question 14

Explain what the exponential factor in the Arrhenius equation represents.

Accepted Answer

The exponential factor depends on both t

Question 15

What is the unit of k in the following rate law? 
Rate = k[X][Y]1/2

Accepted Answer

A) mol L-1 s-1 
B) L mol-1 s-1 
C) L mol-1/2 s-1 
D) L1/2 mol-1/2 s-1 
E) L mol-1 s-1/2 
A) mol L-1 s-1 
B) L mol-1 s-1 
C) L mol-1/2 s-1 
D) L1/2 mol-1/2 s-1 
E) L mol-1 s-1/2

Question 16

Define the frequency factor.

Accepted Answer

The frequency factor

Question 17

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } 
{ [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \
\hline 0.10 & 0.020 \
0.20 & 0.080 \
0.30 & 0.180
\end{array}$$

Accepted Answer

A) zero order 
B) first order 
C) second order 
D) third order 
E) impossible to determine 
A) zero order 
B) first order 
C) second order 
D) third order 
E) impossible to determine

Question 18

What data should be plotted to show that experimental concentration data fit a second-order reaction?

Accepted Answer

A) ln[reactant] vs.time 
B) [reactant] vs.time 
C) ln(k)vs. $\frac { 1 } { T }$ 
D)  $\frac { 1 } { [ \text { reactant] } }$ vs.time 
E) ln(k)vs.Ea 
A) ln[reactant] vs.time 
B) [reactant] vs.time 
C) ln(k)vs. $\frac { 1 } { T }$ 
D)  $\frac { 1 } { [ \text { reactant] } }$ vs.time 
E) ln(k)vs.Ea

Question 19

The following reaction is first order,C2H6 → 2CH3.If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K,how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?

Accepted Answer

A) 4.5 min 
B) 17 min 
C) 53 min 
D) 65 min 
A) 4.5 min 
B) 17 min 
C) 53 min 
D) 65 min

Question 20

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1.If the initial concentration of cyclopropane is 1.33 mol L-1,what is the concentration of cyclopropane after 644 s?

Accepted Answer

A) 0.43 mol L-1 
B) 0.15 mol L-1 
C) 0.94 mol L-1 
D) 0.86 mol L-1 
E) 0.67 mol L-1 
A) 0.43 mol L-1 
B) 0.15 mol L-1 
C) 0.94 mol L-1 
D) 0.86 mol L-1 
E) 0.67 mol L-1

Exam 13: Chemical Kinetics

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 mol L-1.What is the rate constant for this reaction?

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 L mol-1 s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 mol L-1?

Given the following balanced equation,determine the rate of reaction with respect to [O2].If the rate of formation of O2 is 6.94 × 10-1 mol L-1 s-1,what is the rate of the loss of O3? 2O3(g)→ 3O2(g)

Given the following balanced equation,determine the rate of reaction with respect to [SO3]. 2SO2(g)+ O2(g)? 2SO3(g)

If a reaction carried out at 61 °C has an activation energy,Ea, of 67.3 kJ mol-1,a rate constant of 791 s-1,and a frequency factor,A,of 2.65 × 1013,what is the value of R? k=Ae−EaRTk = A e ^ { \frac { - E _ { a } } { R T } }k=AeRT−Ea​​

What data should be plotted to show that experimental concentration data fit a zeroth-order reaction?

Define activation energy.

Identify a heterogeneous catalyst.

Given the following balanced equation,determine the rate of reaction with respect to [SO3].If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1,what is the rate of formation of SO3? 2SO2(g)+ O2(g)→ 2SO3(g)

Given the following balanced equation,determine the rate of reaction with respect to [H2]. N2(g)+ 3H2(g)? 2NH3(g)

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]2

What is the activation energy for a reaction that has a rate constant of 5.68 × 10-8 s-1 at 298 K and 1.73 × 10-5 s-1 at 348 K?

Explain what the exponential factor in the Arrhenius equation represents.

What is the unit of k in the following rate law? Rate = k[X][Y]1/2

Define the frequency factor.

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: [] Initial Rate 0.10 0.020 0.20 0.080 0.30 0.180

What data should be plotted to show that experimental concentration data fit a second-order reaction?

The following reaction is first order,C2H6 → 2CH3.If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K,how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1.If the initial concentration of cyclopropane is 1.33 mol L-1,what is the concentration of cyclopropane after 644 s?

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The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 mol L^-1.What is the rate constant for this reaction?

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 L mol^-1s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 mol L^-1?

Given the following balanced equation,determine the rate of reaction with respect to [O₂].If the rate of formation of O₂ is 6.94 × 10^-1 mol L^-1 s^-1,what is the rate of the loss of O₃? 2O₃(g)→ 3O₂(g)

Given the following balanced equation,determine the rate of reaction with respect to [SO₃]. 2SO₂(g)+ O₂(g)? 2SO₃(g)

If a reaction carried out at 61 °C has an activation energy,E_a, of 67.3 kJ mol^-1,a rate constant of 791 s^-1,and a frequency factor,A,of 2.65 × 10¹³,what is the value of R? $k = A e ^ { \frac { - E _ { a } } { R T } }$

Given the following balanced equation,determine the rate of reaction with respect to [SO₃].If the rate of O₂ loss is 3.56 × 10^-3 mol L^-1 s^-1,what is the rate of formation of SO₃? 2SO₂(g)+ O₂(g)→ 2SO₃(g)

Given the following balanced equation,determine the rate of reaction with respect to [H₂]. N₂(g)+ 3H₂(g)? 2NH₃(g)

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]²

What is the activation energy for a reaction that has a rate constant of 5.68 × 10^-8 s^-1at 298 K and 1.73 × 10^-5 s^-1 at 348 K?

What is the unit of k in the following rate law? Rate = k[X][Y]^1/2

The following reaction is first order,C₂H₆ → 2CH₃.If the rate constant is equal to 5.5 × 10^-4 s^-1 at 1000 K,how long will it take for 0.35 mol of C₂H₆ in a 1.00 L container to decrease to 0.20 mol in the same container?

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10^-4 s^-1.If the initial concentration of cyclopropane is 1.33 mol L^-1,what is the concentration of cyclopropane after 644 s?