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Multiple Choice
The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl2(aq) + C2O4^2-(aq) β 2 Cl^-(aq) + 2 CO2(g) + Hg2Cl2(s). What is the rate law for the reaction?
A
Rate = k[C2O4^2-]^2
B
Rate = k[HgCl2][C2O4^2-]
C
Rate = k[HgCl2]^2
D
Rate = k[HgCl2]^2[C2O4^2-]
Verified step by step guidance
1
Understand the concept of rate law: The rate law expresses the rate of a chemical reaction as a function of the concentration of its reactants. It is determined experimentally and cannot be deduced from the stoichiometry of the reaction alone.
Examine the given data: You have a set of initial rates and corresponding concentrations of reactants. This data is used to determine the order of the reaction with respect to each reactant.
Identify the method of initial rates: This method involves measuring the initial rate of reaction for different initial concentrations of reactants. By comparing how the rate changes with concentration, you can deduce the order of the reaction with respect to each reactant.
Analyze the rate law options: The rate law can be expressed in several forms, such as Rate = k[C2O4^2-]^2, Rate = k[HgCl2][C2O4^2-], Rate = k[HgCl2]^2, and Rate = k[HgCl2]^2[C2O4^2-]. Each form represents different orders with respect to the reactants.
Determine the correct rate law: Compare the experimental data with each rate law option. The correct rate law will be the one that best fits the changes in rate observed with changes in reactant concentrations. This involves calculating the rate for each set of concentrations and matching it to the proposed rate laws.