Question 1

The half life for a first order reaction is 45 min. What is the rate constant in units of s-1

Accepted Answer

A)   0.015 s-1
B)   65 s-1
C)   2.6 x 10-4 s-1
D)   3.9 x 103 s-1
E)   1.9 x 103 s-1F) A) and D)
G) A) and C)

Question 2

Given the rate law for a reaction, rate = k[A][B]2, where rate is measured in units of M s-1, what are the units for the rate constant k

Accepted Answer

A)   M-2s-2
B)   M-1s
C)   M-2s
D)   M2s
E)   None of the aboveF) C) and D)
G) B) and C)

Question 3

The Arrhenius equation is k = Ae-Ea/RT. The slope of a plot of ln k vs. 1/T is equal to

Accepted Answer

A)   -k
B)   k
C)   Ea
D)   -Ea /R
E)   AF) A) and C)
G) A) and B)

Question 4

The rate constant for the first-order decomposition of C4H8 at 500 ∘\circ∘ C is 9.2 * 10-3 s-1. How long will it take for 10.0% of a 0.100 M sample of C4H8 to decompose at 500 ∘\circ∘ C

Accepted Answer

A)   11 s
B)   14 s
C)   18 s
D)   22 s
E)   None of the above F) A) and B)
G) A) and E)

Question 5

The reaction A + 2B  →\rarr→  products has the rate law, rate = k[A][B]3. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

Accepted Answer

A)   2
B)   4
C)   6
D)   8
E)   9 F) A) and E)
G) A) and D)

Question 6

At a particular temperature the first-order gas-phase reaction 2N2O5  →\rarr→  2N2O4 + O2 has a half-life for the disappearance of dinitrogen pentoxide of 3240 s. If 1.00 atm of N2O5 is introduced into an evacuated 5.00 L flask, what will be the total pressure of the gases in the flask after 1.50 hours

Accepted Answer

A)   0.685 atm
B)   1.00 atm
C)   0.315 atm
D)   1.68 atm
E)   1.34 atm F) C) and D)
G) B) and D)

Question 7

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.   Expt. # [NH4+][NO2−]Initial rate (M/hr) 10.0100.0200.02020.0150.0200.03030.0300.0100.015\begin{array}{lccc}	ext { Expt. \# } & {\left[\mathrm{NH}_{4}{ }^{+}ight]} & {\left[\mathrm{NO}_{2}{ }^{-}ight]} & 	ext {Initial rate }(\mathrm{M} / \mathrm{hr})  \\hline 1 & 0.010 & 0.020 & 0.020 \2 & 0.015 & 0.020 & 0.030 \3 & 0.030 & 0.010 & 0.015\end{array} Expt. # 123​[NH4​+]0.0100.0150.030​[NO2​−]0.0200.0200.010​Initial rate (M/hr) 0.0200.0300.015​​  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-]1/4 F) B) and C)
G) B) and E)

Question 8

The activation energy for the following reaction is 60. kJ/mol.Sn2+ + 2Co3+  →\rarr→  Sn4+ + 2Co2+ By what factor (how many times)  will the rate constant increase when the temperature is raised from 10 ∘\circ∘ C to 28 ∘\circ∘ C

Accepted Answer

A)   1.002
B)   4.6
C)   5.6
D)   2.8
E)   696 F) C) and D)
G) None of the above

Question 9

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) D) and E)
G) A) and E)

Question 10

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

Accepted Answer

A)   2
B)   4
C)   6
D)   8
E)   9 F) A) and E)
G) A) and D)

Question 11

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 E)
G) D) and E)

Question 12

Calculate the activation energy, in kJ/mol, for the redox reaction Sn2+ + 2Co3+  →arr→  Sn4+ + 2Co2+.  Temp⁡(∘C) k(1/M⋅ s) 23.12×1032727.0×103\begin{array}{cc}\operatorname{Temp}\left({ }^{\circ} \mathrm{C}ight)  & \mathrm{k}(1 / \mathrm{M} \cdot \mathrm{~s}) \\hline2 & 3.12 	imes 10^{3} \27 & 27.0 	imes 10^{3}\end{array}Temp(∘C) 227​k(1/M⋅ s) 3.12×10327.0×103​​

Accepted Answer

A)   59.2
B)   0.477
C)   5.37
D)   163 kJ
E)   48.1 kJ F) A) and E)
G) C) and E)

Question 13

The activation energy for a certain reaction is 113 kJ/mol. By what factor (how many times)  will the rate constant increase when the temperature is raised from 310 K to 325 K

Accepted Answer

A)   36
B)   5.6
C)   7.6
D)   9.6
E)   None of the aboveF) All of the above
G) B) and E)

Question 14

Substitute natural gas can be synthesized by passing carbon monoxide and hydrogen over Ni or Co at 400$\circ$C.  This process is an example of homogeneous catalysis.

Accepted Answer

A) True 
 B)False

Question 15

Given the rate law for a reaction, rate = k[A]2, where rate is measured in units of M min-1, what are the units for the rate constant k

Accepted Answer

A)   M-2min-1
B)   M-1min-2
C)   M1min-1
D)   M-1min-1
E)   None of the aboveF) A) and B)
G) A) and C)

Question 16

According to the collision theory, all collisions do not lead to reaction. Which choice gives both reasons why not all collisions between reactant molecules lead to reaction
1. The total energy of two colliding molecules is less than some minimum amount of energy.
2. Molecules cannot react with each other unless a catalyst is present.
3. Molecules that are improperly oriented during collision will not react.
4. Solids cannot react with gases.

Accepted Answer

A)   1 and 2
B)   1 and 3
C)   1 and 4
D)   2 and 3
E)   3 and 4F) C) and D)
G) A) and D)

Question 17

Nitric acid is formed by the gas-phase hydrolysis of N2O5. For the reaction N2O5 + H2O  →\rarr→ 2HNO3, Ea(forward)  = 15 kJ/mol and Ea(reverse)  = 51 kJ/mol. Calculate  Δ\DeltaΔ Hrxn.

Accepted Answer

A)  -36 kJ/mol
B)  -56 kJ/mol
C)  -76 kJ/mol
D)  -96 kJ/mol
E)  None of the above F) A) and B)
G) C) and D)

Question 18

The peroxodisulfate ion can oxidize iodide ions to iodine according to the balanced equation S2O82- + 2I -  →\rarr→  2SO42- + I2.The reaction is catalyzed by certain chemical species. Identify the catalyst in the following mechanism:
Step 1: Fe3+ + 2I -  →\rarr→  Fe2+ + I2
Step 2: S2O82- + Fe2+  →\rarr→  2SO42- + Fe3+

Accepted Answer

A)   Fe3+
B)   I -
C)   S2O82-
D)   Fe2+
E)   SO42- F) D) and E)
G) B) and C)

Question 19

Which of the following elementary steps is bimolecular

Accepted Answer

A)  2A + B  →\rarr→  A2B
B)  3B  →\rarr→  B2 + B
C)  A + B + C  →\rarr→  AB + C
D)  A2  →\rarr→  2A
E)  2A  →\rarr→  A2 F) None of the above
G) B) and D)

Question 20

For the chemical reaction A  →\rarr→   C, a plot of 1/[A]t versus time was found to give a straight line with a positive slope. What is the order of reaction

Accepted Answer

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

Exam 13: Chemical Kinetics

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

Correct Answer
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The half life for a first order reaction is 45 min. What is the rate constant in units of s^-1

Correct Answer
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The rate constant for the first-order decomposition of C₄H₈ at 500^$\circ$C is 9.2 * 10^-3 s^-1. How long will it take for 10.0% of a 0.100 M sample of C₄H₈ to decompose at 500^$\circ$C

Correct Answer
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For the chemical reaction A $\rarr$ C, a plot of 1/[A]_t versus time was found to give a straight line with a positive slope. What is the order of reaction

Correct Answer
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Correct Answer
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Given the rate law for a reaction, rate = k[A][B]², where rate is measured in units of M s^-1, what are the units for the rate constant k

Correct Answer
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Given the rate law for a reaction, rate = k[A]², where rate is measured in units of M min^-1, what are the units for the rate constant k

Correct Answer
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The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

Correct Answer
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Correct Answer
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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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Correct Answer
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Correct Answer
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Correct Answer
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Nitric acid is formed by the gas-phase hydrolysis of N₂O₅. For the reaction N₂O₅ + H₂O $\rarr$ 2HNO₃, E_a(forward) = 15 kJ/mol and E_a(reverse) = 51 kJ/mol. Calculate $\Delta$ H_rxn.

Correct Answer
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The activation energy for the following reaction is 60. kJ/mol.Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺ By what factor (how many times) will the rate constant increase when the temperature is raised from 10^$\circ$C to 28^$\circ$C

Correct Answer
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Correct Answer
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The Arrhenius equation is k = Ae^-Ea/RT. The slope of a plot of ln k vs. 1/T is equal to

Correct Answer
verified

Which of the following elementary steps is bimolecular

Correct Answer
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The activation energy for a certain reaction is 113 kJ/mol. By what factor (how many times) will the rate constant increase when the temperature is raised from 310 K to 325 K

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
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Exam 13: Chemical Kinetics

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

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The half life for a first order reaction is 45 min. What is the rate constant in units of s-1

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The rate constant for the first-order decomposition of C4H8 at 500 ∘\circ∘ C is 9.2 * 10-3 s-1. How long will it take for 10.0% of a 0.100 M sample of C4H8 to decompose at 500 ∘\circ∘ C

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For the chemical reaction A →\rarr→ C, a plot of 1/[A]t versus time was found to give a straight line with a positive slope. What is the order of reaction

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Correct AnswerverifiedShow Answer

Given the rate law for a reaction, rate = k[A][B]2, where rate is measured in units of M s-1, what are the units for the rate constant k

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Given the rate law for a reaction, rate = k[A]2, where rate is measured in units of M min-1, what are the units for the rate constant k

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The reaction A + 2B →\rarr→ products has the rate law, rate = k[A][B]3. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

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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.

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Correct AnswerverifiedShow Answer

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Nitric acid is formed by the gas-phase hydrolysis of N2O5. For the reaction N2O5 + H2O →\rarr→ 2HNO3, Ea(forward) = 15 kJ/mol and Ea(reverse) = 51 kJ/mol. Calculate Δ\DeltaΔ Hrxn.

Correct AnswerverifiedShow Answer

The activation energy for the following reaction is 60. kJ/mol.Sn2+ + 2Co3+ →\rarr→ Sn4+ + 2Co2+ By what factor (how many times) will the rate constant increase when the temperature is raised from 10 ∘\circ∘ C to 28 ∘\circ∘ C

Correct AnswerverifiedShow Answer

Substitute natural gas can be synthesized by passing carbon monoxide and hydrogen over Ni or Co at 400 ∘\circ∘ C. This process is an example of homogeneous catalysis.

Correct AnswerverifiedShow Answer

The Arrhenius equation is k = Ae-Ea/RT. The slope of a plot of ln k vs. 1/T is equal to

Correct AnswerverifiedShow Answer

Which of the following elementary steps is bimolecular

Correct AnswerverifiedShow Answer

The activation energy for a certain reaction is 113 kJ/mol. By what factor (how many times) will the rate constant increase when the temperature is raised from 310 K to 325 K

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.

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

Correct Answer
verified

The half life for a first order reaction is 45 min. What is the rate constant in units of s^-1

Correct Answer
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The rate constant for the first-order decomposition of C₄H₈ at 500^$\circ$C is 9.2 * 10^-3 s^-1. How long will it take for 10.0% of a 0.100 M sample of C₄H₈ to decompose at 500^$\circ$C

Correct Answer
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For the chemical reaction A $\rarr$ C, a plot of 1/[A]_t versus time was found to give a straight line with a positive slope. What is the order of reaction

Correct Answer
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Correct Answer
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Given the rate law for a reaction, rate = k[A][B]², where rate is measured in units of M s^-1, what are the units for the rate constant k

Correct Answer
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Given the rate law for a reaction, rate = k[A]², where rate is measured in units of M min^-1, what are the units for the rate constant k

Correct Answer
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The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

Correct Answer
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Correct Answer
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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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Correct Answer
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Correct Answer
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Correct Answer
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Nitric acid is formed by the gas-phase hydrolysis of N₂O₅. For the reaction N₂O₅ + H₂O $\rarr$ 2HNO₃, E_a(forward) = 15 kJ/mol and E_a(reverse) = 51 kJ/mol. Calculate $\Delta$ H_rxn.

Correct Answer
verified

The activation energy for the following reaction is 60. kJ/mol.Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺ By what factor (how many times) will the rate constant increase when the temperature is raised from 10^$\circ$C to 28^$\circ$C

Correct Answer
verified

Correct Answer
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The Arrhenius equation is k = Ae^-Ea/RT. The slope of a plot of ln k vs. 1/T is equal to

Correct Answer
verified

Correct Answer
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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
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