Question

For the reaction between O2 and NO, experiments showed the following results: When the initial concentration of oxygen doubled (keep [NOlo the same), the initial rate of reaction quadrupled; When the initial concentration of NO doubled (keep [O2lo the same), the initial rate of reaction doubled. Which of the following is the correct rate law of the reaction? O Rate k[NOJ[O212 ○ Rate-k[NO][02] 0 Rate-k[NO]2[O2]2 Rate kINO! [O2]

Answer 1

Let rate law be

rate = k [NO]^x [O2]^y

when [O2] doubles, rate became 4 times

So, order of O2 is 2

this means y=2.

when [NO] doubles, rate became 2 times

So, order of NO is 1

this means x = 1

Hence, the rate law is:

rate = k [NO] [O2]^2

Answer: option 1