Question

The gas phase decomposition of nitrogen dioxide at 383 °C

Answer 1

Answer:

$[NO_2]=0.112M$

Explanation:

Hello there!

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

$\frac{1}{[NO_2]} =\frac{1}{[NO_2]_0}+kt$

Thus, given the initial concentration of the nitrogen dioxide gas, the rate constant and the elapsed time, we obtain:

$\frac{1}{[NO_2]}= \frac{1}{0.477M} +0.54M^{-1}s^{-1}\\\\\frac{1}{[NO_2]}=8.933M^{-1}$

$[NO_2]=\frac{1}{8.933M^{-1}} =0.112M$

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