Question

The gas phase decomposition of hydrogen peroxide at 400 °C

Answer 1

Answer:

t = 71.3 s

Explanation:

Hello there!

In this case, since the second-order integrated law is given by the following equation:

$\frac{1}{[H_2O_2]} =\frac{1}{[H_2O_2]_0}+kt$

Thus, given the initial and final concentration of hydrogen peroxide and the rate constant, we obtain the following time:

$\frac{1}{[0.0170M]}-\frac{1}{0.0800M}=0.650M^{-1}s^{-1}t\\\\t=\frac{46.32M^{-1}}{0.650M^{-1}s^{-1}} \\\\t=71.3s$

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