Consider the following reaction: 2NO(g)+2H2(g)N2(g)+2H2O(g)2NO(g)+2H2(g)N2(g)+2H2O(g).

Part A

Part complete

The rate law for this reaction is first order in H2H2 and second order in NONO. Write the rate law.

rate=k[H2][NO]rate=k[H2][NO]

rate=k[H2][NO]2rate=k[H2][NO]2

rate=k[H2]2[NO]2rate=k[H2]2[NO]2

rate=k[H2]rate=k[H2]

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Correct

Part B

If the rate constant for this reaction at 1000 KK is 6.0104M2s16.0104M2s1, what is the reaction rate when [NO]=[NO]= 2.6010² MM and [H2]=[H2]= 1.4010² MM?

Express your answer using two significant figures.

raterate =

nothing

M/sM/s

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Part C

What is the reaction rate at 1000 KK when the concentration of NONO is increased to 0.11 MM, while the concentration of H2H2 is 1.4010² MM?

Express your answer using two significant figures.