Problem: 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.By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)?

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We are asked to determine by what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant given that 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.

We can calculate the reaction rate change of the reaction from its rate law.


Recall that the rate law only focuses on the reactant concentrations and has a general form of:

rate law=kAxBy

k = rate constant
A & B = reactants
x & y = reactant orders


From the given statement, we have:

x = 1

y = 2

hence we have the following rate law expression:

rate law=k[A][B]2


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Problem Details

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.

By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)?

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