Correct answers are given in second picture!!! Please show me how to get them and explain! 4) Given the reaction and data below:[NOCI]o (molecules.cm-³)3.00 x 10162.00 x 10161.00 x 10162 NOCI(g) 2 NO(g) + Cl₂ (g)4.00 x 1016a. m = 2, k = ~2 x 1013b. 2c. ~60000, -100000Initial rate (mol-L-¹.s-¹)5.98 x 1042.66 x 1046.64 x 1031.06 x 105 4) Given the reaction and data below:2 NOCL (g) → 2 NO(g) + Cl₂ (g)[NOCI]o (molecules-cm-3)3.00 x 10162.00 x 10161.00 x 10164.00 x 1016Initial rate (mol-L-¹.s-¹)5.98 x 1042.66 x 1046.64 x 1031.06 x 105a. Determine the rate law and value for the rate constant k, includingunits.b. What is the overall order of the reactions?c. What is the rate of appearance of Cl2 and the rate of disappearanceof NOCI for experiment 1?

a. Rate law can be determined from the order of reaction with respect to NOCl. Rate = k[NOCl]^x Where x is the order of reaction with respect to NOCl. b. Overall order here will be same as that of NOCl order as only one reactant is present. c. Rate of disappearance of NOCl and rate of appearance of Cl2 can be determined. a. 5.98*10^4 = k[3*10^16]^x ...(1) Also, 2.66*10^4 = k[2*10^16]^x ...(2) 1÷2, we have : 2.24 = 1.5^x or, (1.5)^2 = (1.5)^x or, x = 2 Rate = k [ NOCl]^2 k = (5.98*10^4)/(3*10^16)^2 = 6.6*10^-29 b. Overall order= 2. c. Rate = -1/2 d[NOCl]/dt = 1/2 d[NO]/dt = d[Cl2]/dt Rate of appearance of Cl2 = rate = 5.98*10^4 = 60000 Rate of disappearance of NOCl = rate*2 = 120000