Problem: For the reaction A + B -> C at a fixed concentration of A and [B] at the start is 0.10 M, the initial rate was measured. Another reaction was done at the same [A] but [B] was 0.20 M. The initial rate went up 4-fold. The rate law for this reaction isA. rate = k B. rate = k[B] C. rate = k[B]2D. rate = k[B]3E. cannot determine

FREE Expert Solution

We're being asked to determine the rate law of the reaction.

A + B → C

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

To calculate the order of the reaction with respect to each reactant, we will use the experimental data given:

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Problem Details

For the reaction A + B -> C at a fixed concentration of A and [B] at the start is 0.10 M, the initial rate was measured. Another reaction was done at the same [A] but [B] was 0.20 M. The initial rate went up 4-fold. The rate law for this reaction is

A. rate = k 

B. rate = k[B] 

C. rate = k[B]2

D. rate = k[B]3

E. cannot determine

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