Explanation Given The rate constant for the reaction is 3.5 × 10 − 2 M − 1 ⋅ s − 1 . At a given time, the concentration of H 2 S is 2.0 × 10 − 4 M . At a given time, the concentration of Cl 2 is 0.025 M . It is given that rate of the reaction is first order in each reactant. The rate of a reaction at a given time is calculated by the formula, Rate = k [ H 2 S ] [ Cl 2 ] Where, Rate is the rate of the reaction at the given time. k is the rate constant for the reaction. [ H 2 S ] is the concentration of H 2 S at the given time. [ Cl 2 ] is the concentration of Cl 2 at the given time. Substitute the value of k , [ H 2 S ] and [ Cl 2 ] in the above equation. Rate = 3.5 × 10 − 2 M − 1 ⋅ s − 1 × 2

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Author: Brown

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Chapter 14, Problem 90AE

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To determine: The rate of formation of Cl− at a given time.

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Chapter 14, Problem 89AE

Chapter 14, Problem 91AE

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Chapter 14 Solutions

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Ch. 14.2 - If the experiment in Figure 14.2 is run for 60 s,...Ch. 14.2 - Prob. 14.1.2PE Ch. 14.2 - Which of the following could be the instantaneous...Ch. 14.2 - Using Figure 14.3, determine the instantaneous...Ch. 14.2 - At a certain time in a reaction, substance A is...Ch. 14.2 - Prob. 14.3.2PE Ch. 14.3 - Suppose the rate law for the reaction in this...Ch. 14.3 - Assuming that rate = k[A][B], rank the mixtures...Ch. 14.3 - Prob. 14.5.1PE Ch. 14.3 - Prob. 14.5.2PE

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The rate of formation of Cl − at a given time.

To determine: The rate of formation of Cl− at a given time.

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Chapter 14 Solutions