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I am confused in part c of this problem. When I solved for k i used the values from the first row of the table and got 2.85 however the answer is 2.85x10^12. I don't understand the solution for this and why everything is multiplied by .457 when that is nowhere in the problem. Is this because of units?
When you solve for k, remember that the concentrations have to be in mol/L; in the problem, the concentrations are in mmols, so you would have to convert the values to moles. I'm not sure what you mean by multiplying by .457, but looking at the problem, experiment 4 has a initial rate of 457 mmol/L*s, which when converted to moles is .457 mol/L*s.
The number value 0.457 that you're referring to from the solutions is probably the initial rate for experiment 4, except the data gives the initial rate as 457 mol•L^-1•s^-1. In order to find the rate constant of the reaction, you have to take the initial rate and divide it by the product of the reactants, A,B, and C. Be sure to check your units as the data provides them in mmol•L^-1.
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