Given a mechanism consisting of the following two elementary steps:_.
A (g)
B (g) C (g) fast equilibrium A (g)
C (g) 2
D (g) slow step write the rate law of the rate determining step, and then use the equilibrium condition to eliminate any intermediates.
Give the orders of the following substances which appear in the overall reaction:_.
{A} is order.
{B} is order.
{C} is order.
For example, zero, half, first, second, third, etc. (If it is negative, you would write, negative first, negative second, etc)

A non elementary reaction is a reaction that does not take place in a single reactive encounter. This implies that the reaction occurs in steps as shown in the question above.

C(g) is an intermediate, hence it does not occur in the overall reaction equation. The overall reaction equation is: 2A(g) + B(g) ---> 2D(g)

The rate law of the rate determining step is obtained from;

Rate= k1[A] [B] for fast step

Rate= k2 [A] [C] for slow step

But rate of forward reaction = rate of reverse reaction

k1[A] [B] = k-1 [C]

But [C] =k1 [A] [B]/k-1

Hence

Substitute into

Rate = k2 [A] [C]

Rate = k2k-1[A]^2 [B]/k-1

But k2k-1/k = K

Hence;

Rate = K [A]^2 [B]

tallinn tallinn · Answer 2 · 2022-02-16T08:33:29+01:00

The answer is when The reaction is second order in A(g), first-order in B(g), and zero-order in C(g)

Step-by-step explanation:

Elementary reaction

When A non-elementary reaction is a reaction that does not take place in a single reactive encounter. also, This implies that the reaction occurs in steps as shown in the question above.

Then C(g) is an intermediate, hence it does not occur in the overall reaction equation. also The overall reaction equation is: 2A(g) + B(g) ---> 2D(g)

Then The rate law of the rate-determining step is obtained from;

After that Rate= k1[A] [B] for fast step

Then Rate= k2 [A] [C] for slow step

But rate of forward reaction = rate of reverse reaction

k1[A] [B] = k-1 [C]

But [C] =k1 [A] [B]/k-1

Hence

Then Substitute into

Rate = k2 [A] [C]

Rate = k2k-1[A]^2 [B]/k-1

But k2k-1/k = K

Hence;

Thus, Rate = K [A]^2 [B]

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