Question
Asked Sep 9, 2019
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5. Consider the reaction:
H2(e)
HBr(g)
Br2(g)
+
This reaction is first order reaction. k = .053s1
a) Calculate the rate of the reaction when [HBr] 0.055M
b) Calculate the half-life of this reaction.
c) What is the new rate for this reaction if the reaction was to be a second order
reaction?
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5. Consider the reaction: H2(e) HBr(g) Br2(g) + This reaction is first order reaction. k = .053s1 a) Calculate the rate of the reaction when [HBr] 0.055M b) Calculate the half-life of this reaction. c) What is the new rate for this reaction if the reaction was to be a second order reaction?

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Expert Answer

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 t1/2 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.

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Rate k[A (1) 0.693 (2) Rate k[A (3)

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Step 2

(a) The reaction is written as follows:

HBr (g) ⇌ H2(g) + N2(g)

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

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Rate 0.053 s1x0.055 M 0.0029 Ms

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Step 3

(b)

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

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0.693 0.053 s 13.08 s

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