Consider the following reaction: (a) The rate law for this reaction is first ord
ID: 912092 • Letter: C
Question
Consider the following reaction:
(a) The rate law for this reaction is first order in O2(g) and second order in NO(g). What is the rate law for this reaction?
Rate = k [O2(g)] [NO(g)]
Rate = k [O2(g)]2 [NO(g)]
Rate = k [O2(g)] [NO(g)]2
Rate = k [O2(g)]2 [NO(g)]2
Rate = k [O2(g)] [NO(g)]3
Rate = k [O2(g)]4 [NO(g)]
(b) If the rate constant for this reaction at a certain temperature is 7310, what is the reaction rate when [O2(g)] = 0.0189 M and [NO(g)] = 0.0288 M?
Rate = ???????M/s.
(c) What is the reaction rate when the concentration of O2(g) is doubled, to 0.0378 M while the concentration of NO(g) is 0.0288 M?
Rate = ????????? M/s
Explanation / Answer
a) Rate = k [O2] [NO]^2
b) Rate = 7310 * (0.0189) * (0.0288)^2
Rate = 0.1146 M/s
c) Rate = k [O2] [NO]^2
Rate = 7310 * (2 * 0.0189) *(0.0288)^2
Rate = 0.2292 M/s