Finding the rate of A, B, and C

[Sydney Rohan 3G]

How would you start this equation? I am so confused on how to set up this equation, can someone please help me?

[Nika Kononov 3E]

First you would find the orders of each reactant by using the table. Changing the concentration of C doesn't change the rate therefore C is zero order. Doubling the concentration of A doubles the rate therefore A is first order. Doubling the concentration of B quadruples the rate therefore B is second order. Then you can use the numbers from one of the experiments to calculate k by using rate=k*[A][B]^2. This will be your rate law for this reaction.

[Alex FreeWolf 2E]

Similar to what was said above you find the orders of the reactants.

Then plug it into this equation: rate= k[A]^a[B]^b[C]^c
where a,b & c are the orders of the reactants A,B, C respectively

[Jose Angelo Grajeda 2D]

First, you need to determine the rate law by comparing different experiments of the reaction. We can see that changing [C] does not affect the rate, so we can remove it from the rate law (it is zero-order in terms of C). Comparing Experiments 1 and 2, we see that when [B] is held constant, [A] doubles, and so does the rate. Therefore, the rate law is first-order in terms of [A]. Likewise, comparing Experiments 2 and 3, we see that when [A] is held constant, [B] doubles and the initial rate is squared. Therefore, the rate law is second-order in terms of [B]. Putting this altogether, rate = k[A][B]².

Next, we need to find k, the rate constant, now that we have the rate law. We can select data from any experiment, in my case I chose Experiment 1:
2 = k(10)(100)² --> k = 2*10^-5. Finally, for the last part, we would just plug in the [A] and [B] from Experiment 5, along with the k (rate constant) we just calculated, to find the rate of Experiment 5. Hope this helps!

[LianaHernandez1F]

First, you would use the table to determine the ordering of each reactant. As changing the concentration of C has no effect on rate, it is of zero order. A is first order since the rate doubles when the concentration of A is doubled. B is second order because doubling the concentration of B causes a quadrupling of the rate. Therefore, using the data from one of the tests, you may determine k by applying the formula rate=k*[A][B]2. Your rate law for this reaction will be that.