Consider the following reaction: 2 NO2(g) + O3(g) N2O5(g) + O2(g) The rate law f
ID: 733936 • Letter: C
Question
Consider the following reaction:2 NO2(g) + O3(g) N2O5(g) + O2(g)
The rate law for this reaction is:
Rate = k [NO2(g)] [O3(g)]
If the rate constant for this reaction at a certain temperature is 6.34e+04 M-1 s-1, what is the reaction rate when [NO2(g)] = 0.553 M and [O3(g)] = 0.654 M?
a) The reaction rate is 1.75e+05 M s-1.
b) The reaction rate is 5.36e+04 M s-1.
c) The reaction rate is 2.29e+04 M s-1.
d) The reaction rate is 4.36e-05 M s-1.
e) The reaction rate is 5.71e-06 M s-1.
Please help and explain why! Thank you in advance!
Explanation / Answer
c) The reaction rate is 2.29e+04 M s-1. Rate = k [NO2(g)] [O3(g)] substitute the given values