Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this reaction is second order in NO(g) and first order in H2(g). What is the rate law for this reaction? Rate = k [NO(g)] [H2(g)] Rate = k [NO(g)]2 [H2(g)] Rate = k [NO(g)] [H2(g)]2 Rate = k [NO(g)]2 [H2(g)]2 Rate = k [NO(g)] [H2(g)]3 Rate = k [NO(g)]4 [H2(g)] Correct: Your answer is correct. (b) If the rate constant for this reaction at a certain temperature is 77700, what is the reaction rate when [NO(g)] = 0.0792 M and [H2(g)] = 0.144 M? Rate = M/s. (c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.158 M while the concentration of H2(g) is 0.144 M? Rate = M/s