1. Consider the following chemical reaction which is first order with respect to

Question

1. Consider the following chemical reaction which is first order with respect to H and second order with respect to NO: 2NO(g) + 2H(g) Ng) + 2H2O(g) (a) What is the rate law for this reaction? (b) What is the order of the reaction overall? (c) If the rate constant for this reaction at 1000 K is 6.0 x 10Ms1, what is the reaction rate if [N01-0.050 M and [H21-0.010 M? (d) What is the rate of this reaction at 1000 K if the concentration of H2 is doubled but the concentration of NO remains the same? (e) What is the rate of this reaction at 1000 K if the concentration of NO is doubled but the concentration of H2 remains the same?

Explanation / Answer

Ans 1 :

a) Since the order of reaction 2 with respect to NO and first order with respect to HI , the rate law will be given as :

rate = k [NO]2[H2]

b) The overall order of the reaction is the sum of individual orders.

So here it is : 2 +1 = 3

c) Putting all the values in rate law ;

rate = k [NO]2[H2]

rate = 6.0 x 104 (0.050)2(0.010)

= 1.5 M/s

d) If the concentration of H2 is doubled keeping that of NO constant , then the rate of reaction also doubles , since the order of reaction is 1 with respect to H2.

So here , the rate of reaction = 2 x 1.5 = 3.0 M/s

e) Now when the concentration of NO is doubled keeping that of H2 constant , the rate of reaction becomes four times , since the order of reation is 2 with respect to NO.

So here , the rate of reaction = 4 x 1.5 = 6.0 M/s.

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