# Problem: For the reaction A + B -&gt; 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:

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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Rate Law concept. You can view video lessons to learn Rate Law. Or if you need more Rate Law practice, you can also practice Rate Law practice problems.