Question 1

The reaction A + 2B  →\rarr→  products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

Accepted Answer

A)  3
B)  6
C)  9
D)  27
E)  30 F) A) and C)
G) B) and C) C

Question 2

The isomerization of cyclopropane to form propene is a first-order reaction. -2 min-1 B) 1.04 * 10-2 min-1 C) 2.42 min-1 D) 2.06 * 10-3 min-1 E) 2.40 * 10-2 min-1" class="answers-bank-image d-inline" rel="preload" > At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

Accepted Answer

A)  3.66 * 10-2 min-1
B)  1.04 * 10-2 min-1
C)  2.42 min-1
D)  2.06 * 10-3 min-1
E)  2.40 * 10-2 min-1F) A) and B)
G) B) and E)

Question 3

A certain first-order reaction A  →\rarr→  B is 25% complete in 42 min at 25°C. What is the half-life of the reaction?

Accepted Answer

A)  21 min
B)  42 min
C)  84 min
D)  20 min
E)  101 min F) C) and D)
G) A) and C)

Question 4

Nitric oxide reacts with chlorine to form nitrosyl chloride, NOCl. Use the following data to determine the rate equation for the reaction. NO + 1/2Cl2  →\rarr→  NOCl 1/2Cl2  \rarr  NOCl   A) rate = k[NO] B) rate = k[NO][Cl2]1/2 C) rate = k[NO][Cl2] D) rate = k[NO]2[Cl2] E) rate = k[NO]2[Cl2]2 " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  rate = k[NO]
B)  rate = k[NO][Cl2]1/2
C)  rate = k[NO][Cl2]
D)  rate = k[NO]2[Cl2]
E)  rate = k[NO]2[Cl2]2 F) B) and D)
G) A) and C)

Question 5

The first-order reaction SO2Cl2  →\rarr→  SO2 + Cl2 is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

Accepted Answer

A)  1.8 min
B)  104 min
C)  530 min
D)  2300 min
E)  990 min F) A) and E)
G) All of the above D

Question 6

A reaction mechanism usually is

Accepted Answer

A)  the same as the balanced chemical equation.
B)  restricted to only one possible explanation.
C)  obvious if the reaction order is known.
D)  difficult, if not impossible, to prove.
E)  obvious if the activation energy is known.F) A) and C)
G) None of the above

Question 7

The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H3AsO4 + 3I - + 2 H3O + $\rarr$H3AsO3 + I3- + H2O. The experimental rate law for this reaction is
Rate = k [H3AsO4] [I-] [H3O+].
According to the rate law for the reaction, an increase in the concentration of hydronium ion has what effect on this reaction?

Accepted Answer

The rate of reaction...

Question 8

For the chemical reaction A  →\rarr→  B + C, a plot of [A]t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

Accepted Answer

A)  zeroth
B)  first
C)  second
D)  third
E)  Such a plot cannot reveal the order of the reaction. F) C) and E)
G) C) and D)

Question 9

The activation energy for the following first-order reaction is 102 kJ/mol. N2O5(g)  →\rarr→  2NO2(g) + 1/2O2(g) 
The value of the rate constant (k) is 1.35 * 10-4 s-1  at 35°C. What is the value of k at 0°C?

Accepted Answer

A)  8.2 * 10-7 s-1
B)  1.9 * 10-5 s-1
C)  4.2 * 10-5 s-1
D)  2.2 * 10-2 s-1
E)  none of these F) C) and E)
G) None of the above

Question 10

A first-order reaction has a rate constant of 3.00 * 10-3 s-1. The time required for the reaction to be 75.0% complete is

Accepted Answer

A)  95.8 s.
B)  462 s.
C)  231 s.
D)  201 s.
E)  41.7 s.F) None of the above
G) B) and C)

Question 11

With respect to the figure below, which choice correctly identifies all the numbered positions?

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) A) and B)
G) A) and C)

Question 12

The rate law predicted by the following two-step mechanism is rate = k[A][B].
A $\rarr$  C + B slow
A + B $\rarr$ C + E fast

Accepted Answer

A) True 
 B)False

Question 13

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO2, and zeroth-order with respect to CO below 25°C. NO2 + CO  →\rarr→  NO + CO2
 Which one of the following mechanisms is consistent with the observed reaction order?

Accepted Answer

A)  NO2 + 2CO  →\rarr→  N + 2CO2 fast N + NO2  →\rarr→  2NO slow
B)  NO2 + 2CO  →\rarr→  N + 2CO2 slow N + NO2  →\rarr→  2NO fast
C)  NO2 + NO2  →\rarr→  NO3 + NO fast NO3 + CO  →\rarr→  NO2 + CO2 slow
D)  NO2 + NO2  →\rarr→  NO3 + NO slow NO3 + CO  →\rarr→  NO2 + CO2 fast E) None of the above
F) A) and C)

Question 14

For the reaction C6H14(g)  →\rarr→  C6H6(g) + 4H2(g) ,  Δ\DeltaΔ P(H2) / Δ\DeltaΔ t was found to be 2.5 * 10-2 atm/s, where  Δ\DeltaΔ P(H2) is the change in pressure of hydrogen. Determine  Δ\DeltaΔ P(C6H14) / Δ\DeltaΔ t for this reaction at the same time.

Accepted Answer

A)  2.5 * 10-2 atm/s
B)  -6.2 * 10-3 atm/s
C)  -2.5 * 10-2 atm/s
D)  0.10 atm/s
E)  6.2 * 10-3 atm/s F) B) and E)
G) C) and E)

Question 15

At 25°C, the second-order reaction NOCl(g)  →\rarr→  NO(g) + 1/2Cl2(g)  is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

Accepted Answer

A)  8.22 hr
B)  11.6 hr
C)  15.5 hr
D)  17.5 hr
E)  23.0 hr F) B) and E)
G) B) and D)

Question 16

Ammonium ion (NH4+) reacts with nitrite ion (NO2-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. 4+) reacts with nitrite ion (NO2-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations.   Which of the following is the rate law (rate equation) for this reaction? A) rate = k [NH4+] [NO2-]4 B) rate = k [NH4+] [NO2-] C) rate = k [NH4+] [NO2-]2 D) rate = k [NH4+]2 [NO2-] E) rate = k [NH4+]1/2 [NO2-]1/4" class="answers-bank-image d-inline" rel="preload" > Which of the following is the rate law (rate equation) for this reaction?

Accepted Answer

A)  rate = k [NH4+] [NO2-]4
B)  rate = k [NH4+] [NO2-]
C)  rate = k [NH4+] [NO2-]2
D)  rate = k [NH4+]2 [NO2-]
E)  rate = k [NH4+]1/2 [NO2-]1/4F) B) and D)
G) B) and E)

Question 17

The following initial rate data apply to the reaction below. F2(g) + 2Cl2O(g)   →\rarr→  2FClO2(g) + Cl2(g)  2(g) + 2Cl2O(g)   \rarr  2FClO2(g) + Cl2(g)    Which of the following is the rate law (rate equation) for this reaction? A) rate = k[F2]2[Cl2O]4 B) rate = k[F2]2[Cl2O] C) rate = k[F2][Cl2O] D) rate = k[F2][Cl2O]2 E) rate = k[F2]2[Cl2O]2 " class="answers-bank-image d-inline" rel="preload" > Which of the following is the rate law (rate equation) for this reaction?

Accepted Answer

A)  rate = k[F2]2[Cl2O]4
B)  rate = k[F2]2[Cl2O]
C)  rate = k[F2][Cl2O]
D)  rate = k[F2][Cl2O]2
E)  rate = k[F2]2[Cl2O]2 F) A) and C)
G) A) and E) C

Question 18

The reaction A + 2B  →\rarr→  products was found to follow the rate law: rate = k[A]2[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

Accepted Answer

A)  5
B)  6
C)  12
D)  18
E)  None of these. F) C) and D)
G) B) and D)

Question 19

Which one of the following units would not be an acceptable way to express reaction rate?

Accepted Answer

A)  M/s
B)  M. min-1
C)  L .mol-1 . s-1
D)  mol. L-1 .s-1
E)  mmHg/minF) A) and B)
G) A) and E)

Question 20

For what order reaction does the half-life get longer as the initial concentration increases?

Accepted Answer

A)  zeroth order
B)  first order
C)  second order
D)  none of them because half-life is always independent of the initial concentrationE) None of the above
F) A) and B)

Exam 14: Chemical Kinetics

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]². While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

Correct Answer
verified
C

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

Correct Answer
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A certain first-order reaction A $\rarr$ B is 25% complete in 42 min at 25°C. What is the half-life of the reaction?

Correct Answer
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Correct Answer
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The first-order reaction SO₂Cl₂ $\rarr$ SO₂ + Cl₂ is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

Correct Answer
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D

A reaction mechanism usually is

Correct Answer
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Correct Answer
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The rate of reaction...
View Answer

For the chemical reaction A $\rarr$ B + C, a plot of [A]_t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

Correct Answer
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The activation energy for the following first-order reaction is 102 kJ/mol. N₂O₅(g) $\rarr$ 2NO₂(g) + ¹/₂O₂(g) The value of the rate constant (k) is 1.35 * 10^-4 s^-1 at 35°C. What is the value of k at 0°C?

Correct Answer
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A first-order reaction has a rate constant of 3.00 * 10^-3s^-1. The time required for the reaction to be 75.0% complete is

Correct Answer
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With respect to the figure below, which choice correctly identifies all the numbered positions?

Correct Answer
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The rate law predicted by the following two-step mechanism is rate = k[A][B]. A $\rarr$ C + B slow A + B $\rarr$ C + E fast

Correct Answer
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The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO₂, and zeroth-order with respect to CO below 25°C. NO₂ + CO $\rarr$ NO + CO₂ Which one of the following mechanisms is consistent with the observed reaction order?

Correct Answer
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For the reaction C₆H₁₄(g) $\rarr$ C₆H₆(g) + 4H₂(g) , $\Delta$ P(H₂) / $\Delta$ t was found to be 2.5 * 10^-2 atm/s, where $\Delta$ P(H₂) is the change in pressure of hydrogen. Determine $\Delta$ P(C₆H₁₄) / $\Delta$ t for this reaction at the same time.

Correct Answer
verified

At 25°C, the second-order reaction NOCl(g) $\rarr$ NO(g) + ¹/₂Cl₂(g) is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

Correct Answer
verified

Ammonium ion (NH₄⁺) reacts with nitrite ion (NO₂^-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Which of the following is the rate law (rate equation) for this reaction?

Correct Answer
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Correct Answer
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C

The reaction A + 2B $\rarr$ products was found to follow the rate law: rate = k[A]²[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

Correct Answer
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Which one of the following units would not be an acceptable way to express reaction rate?

Correct Answer
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For what order reaction does the half-life get longer as the initial concentration increases?

Correct Answer
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Exam 14: Chemical Kinetics

The reaction A + 2B →\rarr→ products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

Correct AnswerverifiedC

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

Correct AnswerverifiedShow Answer

A certain first-order reaction A →\rarr→ B is 25% complete in 42 min at 25°C. What is the half-life of the reaction?

Correct AnswerverifiedShow Answer

Nitric oxide reacts with chlorine to form nitrosyl chloride, NOCl. Use the following data to determine the rate equation for the reaction. NO + 1/2Cl2 →\rarr→ NOCl

Correct AnswerverifiedShow Answer

The first-order reaction SO2Cl2 →\rarr→ SO2 + Cl2 is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

Correct AnswerverifiedD

A reaction mechanism usually is

Correct AnswerverifiedShow Answer

Correct AnswerverifiedThe rate of reaction...View AnswerShow Answer

For the chemical reaction A →\rarr→ B + C, a plot of [A]t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

Correct AnswerverifiedShow Answer

The activation energy for the following first-order reaction is 102 kJ/mol. N2O5(g) →\rarr→ 2NO2(g) + 1/2O2(g) The value of the rate constant (k) is 1.35 * 10-4 s-1 at 35°C. What is the value of k at 0°C?

Correct AnswerverifiedShow Answer

A first-order reaction has a rate constant of 3.00 * 10-3 s-1. The time required for the reaction to be 75.0% complete is

Correct AnswerverifiedShow Answer

With respect to the figure below, which choice correctly identifies all the numbered positions?

Correct AnswerverifiedShow Answer

The rate law predicted by the following two-step mechanism is rate = k[A][B]. A →\rarr→ C + B slow A + B →\rarr→ C + E fast

Correct AnswerverifiedShow Answer

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO2, and zeroth-order with respect to CO below 25°C. NO2 + CO →\rarr→ NO + CO2 Which one of the following mechanisms is consistent with the observed reaction order?

Correct AnswerverifiedShow Answer

For the reaction C6H14(g) →\rarr→ C6H6(g) + 4H2(g) , Δ\DeltaΔ P(H2) / Δ\DeltaΔ t was found to be 2.5 * 10-2 atm/s, where Δ\DeltaΔ P(H2) is the change in pressure of hydrogen. Determine Δ\DeltaΔ P(C6H14) / Δ\DeltaΔ t for this reaction at the same time.

Correct AnswerverifiedShow Answer

At 25°C, the second-order reaction NOCl(g) →\rarr→ NO(g) + 1/2Cl2(g) is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

Correct AnswerverifiedShow Answer

Ammonium ion (NH4+) reacts with nitrite ion (NO2-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Which of the following is the rate law (rate equation) for this reaction?

Correct AnswerverifiedShow Answer

The following initial rate data apply to the reaction below. F2(g) + 2Cl2O(g) →\rarr→ 2FClO2(g) + Cl2(g) Which of the following is the rate law (rate equation) for this reaction?

Correct AnswerverifiedC

The reaction A + 2B →\rarr→ products was found to follow the rate law: rate = k[A]2[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

Correct AnswerverifiedShow Answer

Which one of the following units would not be an acceptable way to express reaction rate?

Correct AnswerverifiedShow Answer

For what order reaction does the half-life get longer as the initial concentration increases?

Correct AnswerverifiedShow Answer

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]². While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

Correct Answer
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C

Correct Answer
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A certain first-order reaction A $\rarr$ B is 25% complete in 42 min at 25°C. What is the half-life of the reaction?

Correct Answer
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Correct Answer
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The first-order reaction SO₂Cl₂ $\rarr$ SO₂ + Cl₂ is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

Correct Answer
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D

Correct Answer
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Correct Answer
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The rate of reaction...
View Answer

For the chemical reaction A $\rarr$ B + C, a plot of [A]_t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

Correct Answer
verified

The activation energy for the following first-order reaction is 102 kJ/mol. N₂O₅(g) $\rarr$ 2NO₂(g) + ¹/₂O₂(g) The value of the rate constant (k) is 1.35 * 10^-4 s^-1 at 35°C. What is the value of k at 0°C?

Correct Answer
verified

A first-order reaction has a rate constant of 3.00 * 10^-3s^-1. The time required for the reaction to be 75.0% complete is

Correct Answer
verified

Correct Answer
verified

The rate law predicted by the following two-step mechanism is rate = k[A][B]. A $\rarr$ C + B slow A + B $\rarr$ C + E fast

Correct Answer
verified

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO₂, and zeroth-order with respect to CO below 25°C. NO₂ + CO $\rarr$ NO + CO₂ Which one of the following mechanisms is consistent with the observed reaction order?

Correct Answer
verified

For the reaction C₆H₁₄(g) $\rarr$ C₆H₆(g) + 4H₂(g) , $\Delta$ P(H₂) / $\Delta$ t was found to be 2.5 * 10^-2 atm/s, where $\Delta$ P(H₂) is the change in pressure of hydrogen. Determine $\Delta$ P(C₆H₁₄) / $\Delta$ t for this reaction at the same time.

Correct Answer
verified

At 25°C, the second-order reaction NOCl(g) $\rarr$ NO(g) + ¹/₂Cl₂(g) is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

Correct Answer
verified

Ammonium ion (NH₄⁺) reacts with nitrite ion (NO₂^-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Which of the following is the rate law (rate equation) for this reaction?

Correct Answer
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Correct Answer
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C

The reaction A + 2B $\rarr$ products was found to follow the rate law: rate = k[A]²[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

Correct Answer
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Correct Answer
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Correct Answer
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