Part D

What is the reaction rate at $1000K$ if $NO$ is decreased to $0\mathrm{.}014M$ and $H_2$ is increased to $0\mathrm{.}030M?$

Express the rate in moles per liter per second to two significant figures.

$\frac{M}{s}$

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The given concentrations along with the provided rate constant can be substituted into the rate law determined in Part A to calculate the overall reaction rate.

Review I Constants I Periodic Table

Part A

Consider the following reaction:

$2NO(g)+2H_2(g)N_2(g)+2H_{2}O(g).$

The rate law for this reaction is first order in $H_2$ and second order in $NO.$ Choose the rate law.

rate $=k[H_2][NO]$

rate $=k[H_2][NO{]}^2$

rate $=k[H_2{]}^2[NO{]}^2$

rate $=k[H_2]$

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Since the reaction is first order with respect to $H_2,$ its concentration will be raised to the first power. The reaction is also second order with respect to NO$,$ so its concentration is raised to the second power. Both reactant concentrations raised to their respective powers are then multiplied together, along with the rate constant $k,$ to give us the rate law of the

reaction.

rate $=k[H_2][NO{]}^{?}$

PLEASE SOLVE PART D IN THE DESCRIPTION