Which of the following rate laws is possible for the following two-step reaction?
1) NO(g) + NO(g) -- N2O2(g); FAST
2) N2O2(g) + O2(g) -- 2NO2(g); SLOW
Net: 2NO(g) + O2(g) -- 2NO2(g);

A. k[N2O2][O2]
B. k[NO][O2]
C. k[NO]2
D. k[N2O2][NO]

Question

Which of the following rate laws is possible for the following two-step reaction?
1) NO(g) + NO(g) --> N2O2(g);	FAST
2) N2O2(g) + O2(g) --> 2NO2(g);	SLOW
Net: 2NO(g) + O2(g) --> 2NO2(g);

 		A.	k[N2O2][O2]
 		B.	k[NO][O2]
 		C.	k[NO]2
 		D.	k[N2O2][NO]

vera_ewing · Answer

@aaronq A?

aaronq · Answer

nope, only the molecules reacting go into the rate law

vera_ewing · Answer

@aaronq So it's B?

aaronq · Answer

no sorry, you were right the first time, i thoght the slow step was the first step,