Consider the following reaction: (a) The rate law for this reaction is first ord
ID: 886705 • Letter: C
Question
Consider the following reaction:
(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?
Rate = k [HBr(g)] [O2(g)]Rate = k [HBr(g)]2 [O2(g)] Rate = k [HBr(g)] [O2(g)]2Rate = k [HBr(g)]2 [O2(g)]2Rate = k [HBr(g)] [O2(g)]3Rate = k [HBr(g)]4 [O2(g)]
(b) If the rate constant for this reaction at a certain temperature is 8280, what is the reaction rate when [HBr(g)] = 0.00427 M and [O2(g)] = 0.00636 M?
Rate = M/s.
(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00854 M while the concentration of O2(g) is 0.00636 M?
Rate = M/s
Explanation / Answer
(a)
Rate = k [HBr(g)] [O2(g)]
(b)
[HBr(g)] = 0.00427 M and [O2(g)] = 0.00636 M
k = 8280
Rate = k [HBr(g)] [O2(g)]
= 8280 x 0.00427 x 0.00636
= 0.225 M/s
(c)
HBr(g) = 0.00854 M
O2(g)= 0.00636 M
Rate = k [HBr(g)] [O2(g)]
= 8280 x 0.00854 x 0.00636
= 0.450 M/s