The first-order decomposition of SO2Cl2 to sulfur dioxide gas and chlorine gas at 320$\circ$C has a half-life of 8.75 hr. If 600. mmHg of pure SO2Cl2 is placed in a 5.00-L flask at 320$\circ$C, how long does it take for the total pressure in the flask to rise to 1.000 atm

A) 6.45 hr B) 11.1 hr C) 3.91 hr D) 20.3 hr E) 6.91 hr A) 6.45 hr B) 11.1 hr C) 3.91 hr D) 20.3 hr E) 6.91 hr

The following initial rate data apply to the reaction below.F2(g) + 2Cl2O(g) $\rarr$2FClO2(g) + Cl2(g) $\begin{array}{lccc} \mathrm{Expt.\#} & \left[\mathrm{F}_{2}\right](\mathrm{M}) & \left[\mathrm{Cl}_{2} \mathrm{O}\right](\mathrm{M}) & \mathrm{Initial~ rate} (\mathrm{M} / \mathrm{s}) \\\hline 1 & 0.05 & 0.010 & 5.0 \times 10^{-4} \\ 2 & 0.05 & 0.040 & 2.0 \times 10^{-3} \\ 3 & 0.10 & 0.010 & 1.0 \times 10^{-3} \\ \end{array}$ 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 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

A reaction is experimentally found to follow the rate law, Rate = k[A]2 where k = 0.130 M-1min-1. Starting with [A]o = 2.50 M, how many seconds will it take for [A]t = 1.25 M

A) 3.08 s B) 185 s C) 5.33 s A) 3.08 s B) 185 s C) 5.33 s

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 $\begin{array}{llll} \text { Expt. \# } & [\mathrm{NO}] & {\left[\mathrm{Cl}_{2}\right]} & {\text { Initial Rate }} \\ \hline 1 & 0.22 & 0.065 & 0.96 \mathrm{M} / \mathrm{min} \\ 2 & 0.66 & 0.065 & 8.6 \mathrm{M} / \mathrm{min} \\ 3 & 0.44 & 0.032 & 1.9 \mathrm{M} / \mathrm{min} \end{array}$

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 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

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$\circ$C. What is the value of k at 0$\circ$C

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 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

Exam 13: Chemical Kinetics

The first-order decomposition of SO₂Cl₂ to sulfur dioxide gas and chlorine gas at 320^$\circ$C has a half-life of 8.75 hr. If 600. mmHg of pure SO₂Cl₂ is placed in a 5.00-L flask at 320^$\circ$C, how long does it take for the total pressure in the flask to rise to 1.000 atm

(Multiple Choice)

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Question 21

The following initial rate data apply to the reaction below.F₂(g) + 2Cl₂O(g) $\rarr$ 2FClO₂(g) + Cl₂(g) () () (/) 1 0.05 0.010 5.0\times1 2 0.05 0.040 2.0\times1 3 0.10 0.010 1.0\times1 Which of the following is the rate law (rate equation) for this reaction

(Multiple Choice)

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Question 22

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed 2H₂S(g) + O₂(g) $\rarr$ 2S(s) + 2H₂O(l)

(Multiple Choice)

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Question 23

A certain reaction A $\rarr$ products is second order with respect to A with a rate constant, k, 0.122 M^-1min^-1. Starting with [A]_o = 1.01M, how many seconds will it take for A to reach a concentration of 0.750M

(Multiple Choice)

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Question 24

The activation energy for the reaction CH₃CO $\rarr$ CH₃ + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170^$\circ$C than at 150^$\circ$C

(Multiple Choice)

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Question 25

Appropriate units for a first-order rate constant are

(Multiple Choice)

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Question 26

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

(Multiple Choice)

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Question 27

Nitrous oxide (N₂O) decomposes at 600^$\circ$C according to the balanced equation 2N₂O(g) $\rarr$ 2N₂(g) + O₂(g) A reaction mechanism involving three steps is shown below. Identify all of the catalysts in the following mechanism.Cl₂(g) $\rarr$ 2Cl(g) N₂O(g) + Cl(g) $\rarr$ N₂(g) + ClO(g) (occurs twice) ClO(g) + ClO(g) $\rarr$ Cl₂(g) + O₂(g)

(Multiple Choice)

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Question 28

In the reaction, 2N₂O $\rarr$ 2N₂ + O₂, oxygen and nitrogen gases are formed at the same rate (mol/L·s).

(True/False)

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Question 29

Which one of the following changes would alter the rate constant (k) for the reaction 2A + B $\rarr$ products

(Multiple Choice)

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Question 30

In general, to calculate the rate constant for a first order decomposition reaction, A $\rarr$ products, given the time needed to decrease the initial concentration by one half, which equation should be used

(Multiple Choice)

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Question 31

For the following exothermic reaction, the rate law at 298 K is rate = k [H₂][I₂].H₂(g) + I₂(g) $\rarr$ 2HI(g) Which of the following, if any, would cause the rate of the reaction to increase 1. Addition of hydrogen gas at constant temperature and volume 2. Increase in volume of the reaction vessel at constant temperature 3. Addition of a catalyst 4. Increase in temperature

(Multiple Choice)

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Question 32

The rate determining step must be the first step of a reaction mechanism in all cases.

(True/False)

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Question 33

A reaction is experimentally found to follow the rate law, Rate = k[A]² where k = 0.130 M^-1min^-1. Starting with [A]_o = 2.50 M, how many seconds will it take for [A]_t = 1.25 M

(Multiple Choice)

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Question 34

An experimental drug, D, is known to decompose in the blood stream. Tripling the concentration of the drug increases the decomposition rate by a factor of nine. Write the rate law for decomposition ofD.

(Multiple Choice)

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Question 35

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 Expt. \# [] Initial Rate 1 0.22 0.065 0.96/ 2 0.66 0.065 8.6/ 3 0.44 0.032 1.9/

(Multiple Choice)

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Question 36

At 700 K, the rate constant for the following reaction is 6.2 * 10^-4 min^-1. How many minutes are required for 20% of a sample of cyclopropane to isomerize to propene

(Multiple Choice)

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Question 37

Complete the following statement: A catalyst

(Multiple Choice)

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Question 38

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^$\circ$C. What is the value of k at 0^$\circ$C

(Multiple Choice)

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Question 39

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 increases the rate of reaction (linearly with increasing H⁺ concentration).

(True/False)

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Question 40

Showing 21 - 40 of 131

Exam 13: Chemical Kinetics

The first-order decomposition of SO2Cl2 to sulfur dioxide gas and chlorine gas at 320 ∘\circ∘ C has a half-life of 8.75 hr. If 600. mmHg of pure SO2Cl2 is placed in a 5.00-L flask at 320 ∘\circ∘ C, how long does it take for the total pressure in the flask to rise to 1.000 atm

The following initial rate data apply to the reaction below.F2(g) + 2Cl2O(g) →\rarr→ 2FClO2(g) + Cl2(g) () () (/) 1 0.05 0.010 5.0\times1 2 0.05 0.040 2.0\times1 3 0.10 0.010 1.0\times1 Which of the following is the rate law (rate equation) for this reaction

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed 2H2S(g) + O2(g) →\rarr→ 2S(s) + 2H2O(l)

A certain reaction A →\rarr→ products is second order with respect to A with a rate constant, k, 0.122 M-1min-1. Starting with [A]o = 1.01M, how many seconds will it take for A to reach a concentration of 0.750M

The activation energy for the reaction CH3CO →\rarr→ CH3 + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170 ∘\circ∘ C than at 150 ∘\circ∘ C

Appropriate units for a first-order rate constant are

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

In the reaction, 2N2O →\rarr→ 2N2 + O2, oxygen and nitrogen gases are formed at the same rate (mol/L·s).

Which one of the following changes would alter the rate constant (k) for the reaction 2A + B →\rarr→ products

In general, to calculate the rate constant for a first order decomposition reaction, A →\rarr→ products, given the time needed to decrease the initial concentration by one half, which equation should be used

The rate determining step must be the first step of a reaction mechanism in all cases.

A reaction is experimentally found to follow the rate law, Rate = k[A]2 where k = 0.130 M-1min-1. Starting with [A]o = 2.50 M, how many seconds will it take for [A]t = 1.25 M

An experimental drug, D, is known to decompose in the blood stream. Tripling the concentration of the drug increases the decomposition rate by a factor of nine. Write the rate law for decomposition ofD.

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 Expt. \# [] Initial Rate 1 0.22 0.065 0.96/ 2 0.66 0.065 8.6/ 3 0.44 0.032 1.9/

At 700 K, the rate constant for the following reaction is 6.2 * 10-4 min-1. How many minutes are required for 20% of a sample of cyclopropane to isomerize to propene

Complete the following statement: A catalyst

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 ∘\circ∘ C. What is the value of k at 0 ∘\circ∘ C

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The first-order decomposition of SO₂Cl₂ to sulfur dioxide gas and chlorine gas at 320^$\circ$C has a half-life of 8.75 hr. If 600. mmHg of pure SO₂Cl₂ is placed in a 5.00-L flask at 320^$\circ$C, how long does it take for the total pressure in the flask to rise to 1.000 atm

The following initial rate data apply to the reaction below.F₂(g) + 2Cl₂O(g) $\rarr$ 2FClO₂(g) + Cl₂(g) () () (/) 1 0.05 0.010 5.0\times1 2 0.05 0.040 2.0\times1 3 0.10 0.010 1.0\times1 Which of the following is the rate law (rate equation) for this reaction

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed 2H₂S(g) + O₂(g) $\rarr$ 2S(s) + 2H₂O(l)

A certain reaction A $\rarr$ products is second order with respect to A with a rate constant, k, 0.122 M^-1min^-1. Starting with [A]_o = 1.01M, how many seconds will it take for A to reach a concentration of 0.750M

The activation energy for the reaction CH₃CO $\rarr$ CH₃ + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170^$\circ$C than at 150^$\circ$C

In the reaction, 2N₂O $\rarr$ 2N₂ + O₂, oxygen and nitrogen gases are formed at the same rate (mol/L·s).

Which one of the following changes would alter the rate constant (k) for the reaction 2A + B $\rarr$ products

In general, to calculate the rate constant for a first order decomposition reaction, A $\rarr$ products, given the time needed to decrease the initial concentration by one half, which equation should be used

A reaction is experimentally found to follow the rate law, Rate = k[A]² where k = 0.130 M^-1min^-1. Starting with [A]_o = 2.50 M, how many seconds will it take for [A]_t = 1.25 M

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 Expt. \# [] Initial Rate 1 0.22 0.065 0.96/ 2 0.66 0.065 8.6/ 3 0.44 0.032 1.9/

At 700 K, the rate constant for the following reaction is 6.2 * 10^-4 min^-1. How many minutes are required for 20% of a sample of cyclopropane to isomerize to propene

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^$\circ$C. What is the value of k at 0^$\circ$C