Answer to Question #73226 in General Chemistry for Deven

Question

The initial rates listed in the table were determined for the reaction:
2 NO(g) + Cl2(g) → 2 NOCl(g)
Experiment Initial conc. of NO (M) Initial conc. of Cl2 (M) Initial Rate (M/s)
1 0.24 0.10 7.2 x10-6
2 0.12 0.10 3.6 x10-6
3 0.12 0.15 5.4 x10-6
What is the initial rate of reaction when the initial concentrations of both reactants are 0.96 M? (Hint: You must first determine the rate constant and the rate law.)
Enter the results in scientific notation and exponential format. Examples:
Enter for
7.2E-6 7.2x10-6
3.6E-6 3.6x10-6

Answer 1

when [NO] is doubled -> no change in rate -> [NO] zero order
when [Cl2] is doubled -> the rate is doubled -> [Cl2] first order
rate = k[Cl2]
k = rate / [Cl2]
k = 7.2x10-6 / 0.10 = 7.2x10-5 (1/s)
when [Cl2] = 0.96 M
rate = 7.2x10-5 x 0.96 = 6.9x10-5 M/s