The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H20(9) was studied at a certain temperature with the following results: Experiment [NO(9)] (M) [H2(g)] (M) Rate (M/s) 1 2 0.0559 0.0559 0.112 0.112 0.0559 0.112 0.0559 0.112 15.2 30.6 61.2 123 3 4 (a) What is the rate law for this reaction? O Rate = k [NO(9)] [H2(9)] O Rate = k [NO(g)]2[H2(9)] Rate = k [NO(9)] [H2(9)]2 O Rate = k [NO(9)12 [H2(9)12 O Rate = k [NO(9)] [H2(9)3 Rate = k [NO(9)]4 [H2(9)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of NO(g) is 0.110 M and that of H2(g) is 0.122 M if the temperature is the same as that used to obtain the data shown above? |M/s