Question

The reaction 2 HgCl2(aq) + C2042(aq) + 2Cl(aq) + 2 CO2(g) + Hg2Cl2(s) was studied at a certain temperature with the following results: Experiment [HgCl2(aq)] (M) [C2042(aq)] (M) Rate (M/s) 0.122 0.122 0.244 0.244 0.122 0.244 0.122 0.244 2.58e-05 0.000103 5.16e-05 0.000206 (a) What is the rate law for this reaction? Rate = k [HgCl2(aq)] [C2042-(aq)] Rate = k [HgCl2(aq)]? (C2042-(aq)] Rate = k [HgCl2(aq)] [C2042-(aq)]2 Rate = k [HgCl2(aq)]2 (C2042-(aq)]2 Rate = k [HgCl2(aq)] (C2042 (aq)]3 Rate = k [HgCl2(aq)] [C2042(aq)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of HgCl2(aq) is 0.233 M and that of C204(aq) is 0.266 M if the temperature is the same as that used to obtain the data shown above?

Answer 1

let; rate of the reaction is given as ; (a) rate = k l Hq elg ]" t qohlf ....) de ß are orders of reaction For experiment 2; 268x10-5 k 10.12274 [0:122] ...la) " 2 1 0.000103 = k t 0.1220d [ 0. zuuj B. (b) Dividing; (b) by (a); aß = 0.00 0.000103 3.99 2:58 X 10 -5 or; 2 4.00 ex beriment 3; 5:16X10.5. k [0.24478f 10.1223 p .... (1) Dividing (1) by (a) ; ad = 2 1b =. Rate law is ; Rate = k [ Hy elp] 1 [nou ] 02. (Answer) Pulting a = 1; p = 2 in (a) ; ks 2.58 x 1025 0.0142 MP3 0.122 x (01122)2 (c) Given; [ Hg ₂ (aq)] = 0.233 (M) y [com?] -0.266 (M) - Rate = 0.0142 x 0.233 (0.266)2 2.342 X10-4 M8nt. Hence; rate is 2.342 x 10-4 M 8-1