A pascous reaction occurs by a three-step mechanism, shown below what is the ral

Question

A pascous reaction occurs by a three-step mechanism, shown below what is the rale law for this reaction? C) Rate HNOP Rate (NoF Answer ) The relative initial rates of the reaction A2 +B2- products in vessels (a)-d) are 1:44 16 Unshad E) None of these pheres repesent Ag molecales, and shaded spheres represent B2 molecules present at the beginning reaction id) What is the overall order of reaction? A2 8)4 CS D)16E) none of these Answer. ( 7) Concening the rate law, Rate -K[AB,what are appropriate units for the rate constant k Answer( 5) The reaction rates of many spontancous reasctions are actually very slow Which of dhese statcments i oho best explanation for this observation? A) K, for the reaction is less than one C) AG for the reaction is positive E) The entropy change (4S) is negative B) The activation energy of the reaction is large D) Such reactions are endothermic Answer

Explanation / Answer

Ans 5

Rate law is determined by the slowest step of the reaction

The first reaction is fast equilibrium and the third reaction is fast.

Slow reaction is second reaction

N2O2 + H2 - - - > N2O + H2O

Rate = k2 [H2] [N2O2]....... Eq1

But N2O2 is an intermediate so

d[N2O2] / dt = k1[NO]2 - k-1[N2O2] - k2[N2O2] [H2]

From steady state approximation

k1[NO]2 - k-1[N2O2] - k2[N2O2] [H2] = 0

k1[NO]2 = k-1[N2O2] + k2[N2O2] [H2]

[N2O2] = k1[NO]2 / (k-1 + k2 [H2])

From eq1

Rate = (k1k2 [H2][NO]2) / (k-1 + k2 [H2])

Option E is the correct answer

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