The reaction 2N0(g) + C12(g) –+2NOCl(g) was studied at 1o°C. The following results were obtained where Δ[C12] Rate Initial Rate (mol/L-min) INOlo (mol/L) [Clalo (mol/L 0.10 0.10 0.20 0.10 0.20 0.20 0.18 0.36 1.45 a. What is the rate law? b. What is the value of the rate constant? (2) The rate law for the reaction at some temperature is: NOBr a. If the half-life for this reaction is 2.00 s when [NOBro 0.900 M, calculate the value of k for this reaction b. How much time is required for the concentration of NOBr to decrease to 0.100 M? (3) The activation energy for the decomposition of HI (g) to H2(g) and I-(g) is 186 kJ/mol. The rate constant at 555 K is 3.52 X 10-7 L/mol.s. What is the rate constant at 645 K?