Posted by elvis on Saturday, February 18, 2012 at 9:18pm.
Given this data in a study on how the rate of a reaction was affected by the concentration of the reactants
Initial Rate,
RUN #(A, M) (B, M) (C, M) (mol L1 s1
1 0.200 0.100 0.600 5.00
2 0.200 0.400 0.400 80.0
3 0.600 0.100 0.200 15.0
4 0.200 0.100 0.200 5.00
5 0.200 0.200 0.400 20.0
The rate constant for this reaction (all in the same units) is
a. 6667 b. 208 c. 2083 d. 139 e. 2500
help me!
chemistry  DrBob222, Friday, February 17, 2012 at 10:29pm
The secret here is to determine the order of the reaction. For example, it is zero order in C. Do you know how to do the others? After you determine the orders, then k is determined as in your post above.
Saw the other post didn't help at all but I need the answer and simple step by step solution

chemistry  DrBob222, Saturday, February 18, 2012 at 9:46pm
I don't remember all the posts you had yesterday. Did you read how to determine the rate law expression. Can you do that from these data? I seem to remember that it was zero with respect to C, 2nd order with respect to B and 1st order with respect to A. so the rate law expression is
rate = k(A)^1(B)^2(C)^0 which becomes simply rate = k(A)(B^2) since we don't need to show exponents of 1 (and remember anything to the zero power is 1)
Pick any trial in your post and plug the values into the rate law expression above. The only unknown is k. Solve for that.
For example, pick the first one.
rate = k*(A)(B)^2
5.00 = k*(0.200)(0.1)^2 and solve for k. 
chemistry  Frank A, Tuesday, February 12, 2013 at 4:29pm
2500