Question

Consider the following reaction: 2 HgCl2(aq) + C2042 (aq) 2 Cl(aq) + 2 CO2(g) + H92C12(s) (a) The rate law for this reaction is first order in HgCl2(aq) and second order in C2042(aq). What is the rate law for this reaction? Rate = k [HgCl2(aq)] (C2042 (aq)] 0 Rate = k [HgCl2(aq)]? (C2042(aq)] 0 0 Rate = k [HgCl(aq)] [C2042 (aq)]? Rate = k [HgCl2(aq)] (C2042-(aq)2 Rate = k [HgCl2(aq)] [C2042 (aq)] Rate = k [HgCl2(aq)]*[C2042 (aq)] (b) If the rate constant for this reaction at a certain temperature is 0.00890, what is the reaction rate when [HgCl2(aq)] = 0.191 M and (C204(aq)] = 0.250 M? Rate = M/S. (c) What is the reaction rate when the concentration of HgCl(aq) is doubled, to 0.382 M while the concentration of C2042 (aq) is 0.250 M? Rate = M/S

Answer 1

Dear student,

2 g le leg) + Cl2 ley) 240-lag) + 2002 ight Hage ch lat The rate law for a reaction is given as Rade= k [Reactant] whewe, K = Rato constant K- Onder of reaction with respect to read and Rede law foce above reaction Rade : * [Hg cos con I° [C202* my] The seedion is full oaden in ugch and second oeden. in our 30 a 1 and b=2 Rate = x [ugce coop] [le Qu? Tany) 7° above Deact LC) (b) K = 0.00890 [Halla legi] = Onaim and [Caoua (ago] = 0. 250 m

Rate = k [Hgla (ay) ] [one caqs] Rate = 0.0089 0 [0.191] [0.250] 2 Rate = 0.00 16 999 x 0.0625 Rate = 0.000 1062 M/s. Rate = 1.062x10 "M/s. (6) [HgCl2 lags] = 0.382 m. [C20, 2-Coqs ] = 0.250m Rate: 0.00890 x [0:382] [o1250]?. Rate = 0.0033998 x 0.0625 Rate = 0.00021248 MIS Rate = 2.125 x 104 ms.

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