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ChemistryQ&A Library5. Consider the reaction:H2(e)HBr(g)Br2(g)+This reaction is first order reaction. k = .053s1a) Calculate the rate of the reaction when [HBr] 0.055Mb) Calculate the half-life of this reaction.c) What is the new rate for this reaction if the reaction was to be a second orderreaction?Question

Asked Sep 9, 2019

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Step 1

The rate of the reaction for the first order reaction is written in equation (1) in which k is the rate constant of the reaction and A is the concentration of the reactant.

The half-life for a first order reaction is given by the equation (2) in which t_{1/2} is the half-life and k is the rate constant.

The rate of reaction for a second order reaction for a single reactant is shown in equation (3) in which k is the rate constant of the reaction and A is the concentration of the reactant.

Step 2

(a) The reaction is written as follows:

HBr (g) ⇌ H_{2}(g) + N_{2}(g)

Use the equation (1) to determine the rate of the above reaction and substitute 0.055M for A and 0.053 s^{-1}for k as shown below.

Step 3

(b)

The half-life of the reaction is calculated by using the equation (...

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