Finding the rate of A, B, and C
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Finding the rate of A, B, and C
How would you start this equation? I am so confused on how to set up this equation, can someone please help me?
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Re: Finding the rate of A, B, and C
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.
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Re: Finding the rate of A, B, and C
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
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
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Re: Finding the rate of A, B, and C
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!
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!
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Re: Finding the rate of A, B, and C
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.
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