✔ 最佳答案
Chemical equation : 2IBr(g) → I2(g) + Br2(g)
a.
1. IBr(g) → I(g)+Br(g) .... (fast)
2. IBr(g) + Br(g) → I(g)+Br2(g) .... (slow)
3. I(g) + I(g) → I2(g) .... (fast)
Step 2 is the rate determining step (r.d.s.). Hence,
Rate = k'[IBr(g)][Br(g)] .... (1)
Br(g) is an intermediate of the reaction, and thus it should not appear in the rate law.
Br(g) is formed in step 1.
Refer to step 1. [Br(g)] is directly proportional to [IBr(g)]. Hence,
[Br(g)] = k"[IBr(g)] .... (2)
Sub. (2) into (1):
Rate = k'[IBr(g)]•k"[IBr(g)] = k'k"[IBr(g)]^2
Hence, the rate law is :
Rate = k[IBr(g)]^2
b.
1. IBr(g) + IBr(g) → I2Br^+(g) + Br^-(g) .... (fast)
2. I2Br+(g) → Br^+(g) + I2(g) .... (slow)
3. Br^+ (g) + Br^-(g) → Br2(g) .... (fast)
Step 2 is the r.d.s. Hence,
Rate = k'[I2Br^+(g)] .... (1)
I2Br^+(g) is an intermediate of the reaction, and thus it should not appear in the rate law.
I2Br^+(g) is formed in step 1.
Refer to step 1. [I2Br^+(g)] is directly proportional to [IBr(g)]^2. Hence,
[I2Br^+(g)] = k"[IBr(g)]^2 .... (2)
Sub. (2) into (1):
Rate = k'•k"[IBr(g)]^2 = k'k"[IBr(g)]^2
Hence, the rate law is :
Rate = k[IBr(g)]^2