Question I (from the University of Arizona) Nitric oxide (NO) reacts with H2 to form N2O and H2O. It is known that there are two elementarysteps to this reaction:Step I: NO(g) + NO(g) ---> N2O2(g)Step II: N2O2(g) + H2(g) ---> N2O(g) + H2O(g)The measured rate law for this overall reaction is:Rate = k[NO]2 [H2]What can we conclude about the above elementary reaction steps based on this rate law?(A) Steps I & II are about the same rate.(B) Step I is much faster than step II.(C) Step II is much faster than step I.(D) Not enough information to tell. Question II (from the University of Guelph)Consider the possible mechanisms for the following reaction:2NO + O2 → 2NO21.NO(g) + NO(g) → N2O2(g) (slow)N2O2(g) + O2(g) → 2NO2(g) (fast)2. NO(g) + NO(g) → N2O2(g) (fast)N2O2(g) + O2(g) → 2NO2(g) (slow)3.NO(g) + O2(g) → NO2(g) + O(g) (slow)NO(g) + O(g) → NO2(g) (fast)Given that the empirical rate law for this reaction isfound to be rate = k[NO]2[O2]. Which mechanism(s) is consistant with the rate law?a. I and IIb. only IIIc. only IId. all three mechanisms are consistante. only If. II and IIIg. I and III Question IIII (from the University of Texas at Austin) Nitrogen gas N2N2 is formed by the reaction of NONO and H2H2. The proposed mechanism for the reaction is:2NO⇌N2O2(fast,equilibrium)N2O2+H2→N2O+H2O(slow)N2O+H2→N2+H2O(fast) What rate law is consistent with this mechanism? Question IV (from Texas A & M) Which equation is fast and which one is slow?A) 2 NO --> N2O2B) N2O2 +O2 --> 2 NO2
Question I (from the University of Arizona)
Nitric oxide (NO) reacts with H2 to form N2O and H2O. It is known that there are two elementary
steps to this reaction:
Step I: NO(g) + NO(g) ---> N2O2(g)
Step II: N2O2(g) + H2(g) ---> N2O(g) + H2O(g)
The measured rate law for this overall reaction is:
Rate = k[NO]2 [H2]
What can we conclude about the above elementary reaction steps based on this rate law?
(A) Steps I & II are about the same rate.
(B) Step I is much faster than step II.
(C) Step II is much faster than step I.
(D) Not enough information to tell.
Question II (from the University of Guelph)
Consider the possible mechanisms for the following reaction:
2NO + O2 → 2NO2
1.
NO(g) + NO(g) → N2O2(g) (slow)
N2O2(g) + O2(g) → 2NO2(g) (fast)
2.
NO(g) + NO(g) → N2O2(g) (fast)
N2O2(g) + O2(g) → 2NO2(g) (slow)
3.
NO(g) + O2(g) → NO2(g) + O(g) (slow)
NO(g) + O(g) → NO2(g) (fast)
Given that the empirical rate law for this reaction is
found to be rate = k[NO]2[O2].
Which mechanism(s) is consistant with the rate law?
a. I and II
b. only III
c. only II
d. all three mechanisms are consistant
e. only I
f. II and III
g. I and III
Question IIII (from the University of Texas at Austin)
Nitrogen gas N2N2 is formed by the reaction of NONO and H2H2. The proposed mechanism for the reaction is:
2NO⇌N2O2(fast,equilibrium)
N2O2+H2→N2O+H2O(slow)
N2O+H2→N2+H2O(fast)
What rate law is consistent with this mechanism?
Question IV (from Texas A & M)
Which equation is fast and which one is slow?
A) 2 NO --> N2O2
B) N2O2 +O2 --> 2 NO2
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