For the reaction A+B+CD+E, the initial reaction rate was measured for various in

Question

For the reaction A+B+CD+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected:

6.0×104

What is the reaction order with respect to A? 2

What is the reaction order with respect to B? 0

What is the reaction order with respect to C? 1

What is the value of the rate constant k for this reaction?k = 1.2×103 M2s1

I know all above are correct, but now I'm stuck...

***Given the data calculated in Parts A, B, C, and D, determine the initial rate for a reaction that starts with 0.65 M of reagent A and 0.90 M of reagents B and C?

Please show steps.

Trial [A]
(M) [B]
(M) [C]
(M) Initial rate
(M/s) 1 0.50 0.50 0.50 1.5×104 2 0.50 0.50 1.50 4.5×104 3 1.00 0.50 0.50 6.0×104 4 1.00 1.00 0.50

6.0×104

Explanation / Answer

Answer –

We are given , reaction –

A+B+C--->D+E

We also given order with respect to A, B and C and they are 2,0 and 1 respectively.

So that means reaction rate is depend on A and C and not on B, because the order with respect to B is zero. Overall reaction is 2+1 = 3 means third order reaction.

We also given rate constant for this reaction 1.2×103 M2s1

So rate law for this reaction –

Rate = k [A]2[C]1

Now, we need to calculate rate when [A] = 0.65 M, [C] = 0.90 M

We know rate law

Rate = k [A]2[C]1

         = 1.2×103 M2s1*(0.65 M)2*(0.90M)

         = 4.56*10-4 M.s-1

So, initial rate for a reaction that starts with 0.65 M of reagent A and 0.90 M of reagents B and C is 4.56*10-4 M.s-1

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