ANSWER B AND C PLEASE

Part B

Consider the following reaction:

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

If the rate constant for this reaction at $1000K$ is $6\mathrm{.}0{10}^4{M}^{-2}{s}^{-1},$ what is the reaction rate when

$[NO]=0\mathrm{.}021M$ and $[H_2]=0\mathrm{.}011M?$

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

rate :

$\frac{M}{s}$

Part C

What is the reaction rate at $1000K$ when the concentration of $NO$ is increased to $0\mathrm{.}10M$ while the

concentration of $H_2$ is $0\mathrm{.}014M?$

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

rate $=$

$\frac{M}{s}$