How do you find rate of production of Cl? If you are given the inital rate to be 3.54e-5 and given measured data of .052[HgCl2] and .300[C204]? The equation is 2HgCl2(aq)+ C204(aq) goes to 2Cl+ 2Co2(g)+ Hg2Cl2(s). I thought that you may take the initial rate divided by the coefficent of Cl, but i'm not sure.
To find the rate of production of Cl, you need to calculate the rate of the overall reaction and then divide it by the stoichiometric coefficient of Cl in the balanced chemical equation.
Given that the initial rate is 3.54e-5, you need to find the rate expression for the reaction. From the balanced chemical equation, you can see that 2 moles of HgCl2 react to produce 2 moles of Cl. Therefore, the stoichiometric coefficient of Cl is 2.
To determine the rate expression, you need to relate the change in concentration of reactants with the rate of the reaction. In this case, you have measured data for the concentrations of HgCl2 and C204. Let's assume the change in concentration of HgCl2 is ∆[HgCl2] and the change in concentration of C204 is ∆[C204]. The rate expression can be written as:
rate = k * [HgCl2]^m * [C204]^n
By comparing the balanced equation to the rate expression, you can determine the values of m and n. Since you're trying to find the rate of production of Cl, which is on the reactant side in the balanced equation, the exponents for [HgCl2] and [C204] will be negative.
In this case, the rate expression for the reaction can be simplified to:
rate = k * [HgCl2]^-2 * [C204]^1
Now, if you're given the initial concentrations of HgCl2 and C204, let's say [HgCl2] = 0.052 M and [C204] = 0.300 M, you can substitute these values into the rate expression and solve for the rate constant (k).
Finally, to find the rate of production of Cl, you divide the overall rate (3.54e-5) by the stoichiometric coefficient of Cl (2). This will give you the rate of production of Cl in the units specified (e.g., M/s).