Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(g) 20(g) fast Step 2: O(g) + N₂(g) 2, NO(g) + N(g) slow K₂ Step 3: O(g) + N(g) NO(g) very fast 3 $ % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂1² C & 7 What is the rate law for the forward reaction in step 1? Rate =k,[0]² Rate = kr[0₂] Rate-k,[0]2 Rate=k,[O][N] Rate = klO₂/k,[012 Rate = k₂[0][N₂] Rate-k[0₂] MacBook Pro Rate = k0₂1² Rate =k,[0₂1² Rate = k/[0]2 Rate=k+[0₂] What is the overall rate law for this reaction? Rate k[N₂][O₂][N][O] 8 ( 9 ☆ BA

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Mechanism
Suppose a reaction occurs with the following mechanism. All are elementary steps.
Step 1: 0₂(9)
20(g)
fast
K₂
Step 2: O(g) + N₂(g)
Step 3: O(g) + N(g)
گی
3
NO(g) + N(g) slow
very fast
K3, NO(g)
$
4
%
5
6
What is the rate law for the rate-determining step?
Rate =k,[0₂]²
Rate = kr[O]²
Rate-k,[O][N]
Rate = kf[0₂]/k,[0]²
Rate = k₂[O][N₂]
Rate = K[0₂]
&
7
What is the rate law for the forward reaction in step 1?
Rate = kr[O]²
Rate = kr[0₂]
Rate =k+[0₂1²
Rate = kr[0₂1²
Rate = kf[0]²
Rate =k+[0₂]
What is the overall rate law for this reaction?
Rate = k[N₂][0₂][N][0]
MacBook Pro
8
(
9
☆
88
Transcribed Image Text:Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88
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