Consider the following reaction: 2 HgCl2(aq) + C2O42-(aq) 2 Cl-(aq) + 2 CO2(g) +

Question

Consider the following reaction: 2 HgCl2(aq) + C2O42-(aq) 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) (a) The rate law for this reaction is first order in HgCl2(aq) and second order in C2O42-(aq). What is the rate law for this reaction? Rate = k [HgCl2(aq)] [C2O42-(aq)] Rate = k [HgCl2(aq)]2 [C2O42-(aq)] Rate = k [HgCl2(aq)] [C2O42-(aq)]2 Rate = k [HgCl2(aq)]2 [C2O42-(aq)]2 Rate = k [HgCl2(aq)] [C2O42-(aq)]3 Rate = k [HgCl2(aq)]4 [C2O42-(aq)] (b) If the rate constant for this reaction at a certain temperature is 0.00980, what is the reaction rate when [HgCl2(aq)] = 0.165 M and [C2O42-(aq)] = 0.290 M? Rate = M/s. (c) What is the reaction rate when the concentration of HgCl2(aq) is doubled, to 0.330 M while the concentration of C2O42-(aq) is 0.290 M? Rate = M/s

Explanation / Answer

Start with Rate = k reaction is first order in HgCl2(aq) so [HgCl2(aq) ] to the 1st power and second order in C2O42-(aq) so [C2O42-(aq)] is to the 2nd power Rate = k [HgCl2(aq)] [C2O42-(aq)]^2 (b) If the rate constant for this reaction at a certain temperature is 0.0169, what is the reaction rate when [HgCl2(aq)] = 0.158 M and [C2O42-(aq)] = 0.202 M? just plug in the numbers Rate = k [HgCl2(aq)] [C2O42-(aq)]^2 Rate = .0169 [.158] [.202]^2 Rate = 1.0895 x 10^(-4) M/s (c) What is the reaction rate when the concentration of HgCl2(aq) is doubled, to 0.316 M while the concentration of C2O42-(aq) is 0.202 M? Rate = M/s just plug in the numbers again (k is constant) Rate = k [HgCl2(aq)] [C2O42-(aq)]^2 Rate = .0169 [.316] [.202]^2 Rate = 2.1791 x 10^(-4) M/s

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