A reaction in which A, B, and C react to form products is first order in A, seco

Question

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.

Write a rate law for the reaction. Write a rate law for the reaction. Rate=k[A][B] Rate=k[A][B]2 Rate=k[A][B][C] Rate=k[A]2[B]3[C] Part B Part complete What is the overall order of the reaction?

Part C By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? Rate2Rate1 = 11 SubmitPrevious AnswersRequest Answer Incorrect;

Part D Part complete By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)? Rate2Rate1 = 4 SubmitPrevious

Part E By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)? Rate2Rate1 = c SubmitPrevious AnswersRequest Answer Incorrect;

Part F By what factor does the reaction rate change if the concentrations of all three reactants are doubled? Rate2Rate1 = 5.65 SubmitPrevious

Explanation / Answer

The answer to part A is rate=[A][B]2 because of the given information that rate is first order in A and second order in B and zero order in C which means independent of C.

Part b= overall order of reaction is sum of all the individual orders. Thus the answer is 2+1+0=3

Part c- because the reaction is first order in A the reaction rate increases by a factor of 2.

Part d- because the reaction is second order in B the reaction the reaction rate increases by a factor of 2*2=4

Part e- because the reaction rate is independent of the concentration of C it does not change at all.

Part f- because of the reasons stated above the reaction rate increases by a factor of 2*4= 8 times

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