Integrated Rate Laws - AP Chemistry

Card 0 of 65

Question

The rate constant for a second-order reaction is 0.15 M-1s-1. If the initial concentration of the reactant is 0.30 M, how long does it take for the concentration to decrease to 0.15 M?

Answer

$\frac{1}{[A]_t} = kt + \frac{ 1 }{[A]_o}$

$t =\frac{ \frac{1}{[A]_t} -\frac{1}{[A]_o}}{k} =\frac{\frac{1}{0.15} - \frac{1}{0.30}}{0.15}= 22.2 seconds$

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Question

Based on the figure above, what is the order of reaction?

Answer

For a first order reaction, the ln \[A\]t is linear with t.

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Question

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60 minutes, the half-life of the compound is?

Answer

$k = - \frac{ln[A]_t - ln[A]_o}{t}= - \frac{ln[75]-ln[100]}{60}= 4.79 x10^{-3}$

$t_{\frac{1}{2}}=\frac{ ln2 }{k} = \frac{ln2}{4.79x10^{-3}}= 145 minutes$

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Question

Cyclopentane is unstable and decomposes by a first order reaction. The rate constant for this reaction is 9.5 s-1. What is the half life of the reaction?

Answer

$t_{\frac{1}{2}}=\frac{ln2 }{k} = \frac{ln2}{9.5} = 0.0729 seconds$

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Question

The half life of a first order reaction is 1.5 hours. What is the rate constant of this reaction?

Answer

$t_{\frac{1}{2}} = \frac{ln2 }{k}$

$k =\frac{ln2}{t_{\frac{1}{2}}} = \frac{ln2}{1.5} = 0.46$

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Question

The rate constant for a second-order reaction is 0.15 M-1s-1. If the initial concentration of the reactant is 0.30 M, how long does it take for the concentration to decrease to 0.15 M?

Answer

$\frac{1}{[A]_t} = kt + \frac{ 1 }{[A]_o}$

$t =\frac{ \frac{1}{[A]_t} -\frac{1}{[A]_o}}{k} =\frac{\frac{1}{0.15} - \frac{1}{0.30}}{0.15}= 22.2 seconds$

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Question

Based on the figure above, what is the order of reaction?

Answer

For a first order reaction, the ln \[A\]t is linear with t.

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Question

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60 minutes, the half-life of the compound is?

Answer

$k = - \frac{ln[A]_t - ln[A]_o}{t}= - \frac{ln[75]-ln[100]}{60}= 4.79 x10^{-3}$

$t_{\frac{1}{2}}=\frac{ ln2 }{k} = \frac{ln2}{4.79x10^{-3}}= 145 minutes$

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Question

Cyclopentane is unstable and decomposes by a first order reaction. The rate constant for this reaction is 9.5 s-1. What is the half life of the reaction?

Answer

$t_{\frac{1}{2}}=\frac{ln2 }{k} = \frac{ln2}{9.5} = 0.0729 seconds$

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Question

The half life of a first order reaction is 1.5 hours. What is the rate constant of this reaction?

Answer

$t_{\frac{1}{2}} = \frac{ln2 }{k}$

$k =\frac{ln2}{t_{\frac{1}{2}}} = \frac{ln2}{1.5} = 0.46$

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Question

The rate constant for a second-order reaction is 0.15 M-1s-1. If the initial concentration of the reactant is 0.30 M, how long does it take for the concentration to decrease to 0.15 M?

Answer

$\frac{1}{[A]_t} = kt + \frac{ 1 }{[A]_o}$

$t =\frac{ \frac{1}{[A]_t} -\frac{1}{[A]_o}}{k} =\frac{\frac{1}{0.15} - \frac{1}{0.30}}{0.15}= 22.2 seconds$

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Question

Based on the figure above, what is the order of reaction?

Answer

For a first order reaction, the ln \[A\]t is linear with t.

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Question

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60 minutes, the half-life of the compound is?

Answer

$k = - \frac{ln[A]_t - ln[A]_o}{t}= - \frac{ln[75]-ln[100]}{60}= 4.79 x10^{-3}$

$t_{\frac{1}{2}}=\frac{ ln2 }{k} = \frac{ln2}{4.79x10^{-3}}= 145 minutes$

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Question

Cyclopentane is unstable and decomposes by a first order reaction. The rate constant for this reaction is 9.5 s-1. What is the half life of the reaction?

Answer

$t_{\frac{1}{2}}=\frac{ln2 }{k} = \frac{ln2}{9.5} = 0.0729 seconds$

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Question

The half life of a first order reaction is 1.5 hours. What is the rate constant of this reaction?

Answer

$t_{\frac{1}{2}} = \frac{ln2 }{k}$

$k =\frac{ln2}{t_{\frac{1}{2}}} = \frac{ln2}{1.5} = 0.46$

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Question

The rate constant for a second-order reaction is 0.15 M-1s-1. If the initial concentration of the reactant is 0.30 M, how long does it take for the concentration to decrease to 0.15 M?

Answer

$\frac{1}{[A]_t} = kt + \frac{ 1 }{[A]_o}$

$t =\frac{ \frac{1}{[A]_t} -\frac{1}{[A]_o}}{k} =\frac{\frac{1}{0.15} - \frac{1}{0.30}}{0.15}= 22.2 seconds$

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Question

Based on the figure above, what is the order of reaction?

Answer

For a first order reaction, the ln \[A\]t is linear with t.

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Question

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60 minutes, the half-life of the compound is?

Answer

$k = - \frac{ln[A]_t - ln[A]_o}{t}= - \frac{ln[75]-ln[100]}{60}= 4.79 x10^{-3}$

$t_{\frac{1}{2}}=\frac{ ln2 }{k} = \frac{ln2}{4.79x10^{-3}}= 145 minutes$

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Question

Cyclopentane is unstable and decomposes by a first order reaction. The rate constant for this reaction is 9.5 s-1. What is the half life of the reaction?

Answer

$t_{\frac{1}{2}}=\frac{ln2 }{k} = \frac{ln2}{9.5} = 0.0729 seconds$

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Question

The half life of a first order reaction is 1.5 hours. What is the rate constant of this reaction?

Answer

$t_{\frac{1}{2}} = \frac{ln2 }{k}$

$k =\frac{ln2}{t_{\frac{1}{2}}} = \frac{ln2}{1.5} = 0.46$

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