Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI, and the rate constant is 9.7×10−6M−1s−1. If the initial concentration of HI is 0.100 M. What is its molarity after a reaction time of 7.00 days? What is the time (in days) when the HI concentration reaches a value of 0.080 M?

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI, and the rate constant is 9.7×10−6M−1s−1. If the initial concentration of HI is 0.100 M. What is its molarity after a reaction time of 7.00 days? What is the time (in days) when the HI concentration reaches a value of 0.080 M?

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Step 1

The decomposition of hydrogen iodide is a second-order reaction. The rate constant for the second-order reaction is given by:

kt = 1A - 1Ao

where, k = rate constant = 9.7×10−6 M-1s-1

t = time = 7.00 days

[A] = concentration of the reactant after t time =?

[Ao] = initial concentration of the reactant = 0.100 M

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