The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results:

Experiment	[HBr(g)] (M)	[O2 (g)] (M)	Rate (M/s)
1	0.00305	0.00305	0.0913
2	0.00305	0.00610	0.183
3	0.00610	0.00305	0.183
4	0.00610	0.00610	0.365

(a) 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)]2

Rate = k [HBr(g)]2 [O2(g)]2

Rate = k [HBr(g)] [O2(g)]3

Rate = k [HBr(g)]4 [O2(g)]

(b) What is the value of the rate constant?

(c) What is the reaction rate when the concentration of HBr(g) is 0.00382 M and that of O2(g) is 0.00745 M if the temperature is the same as that used to obtain the data shown above?