Reaction Order

Question 1

Zero order

Answer 1

Increase the concentration of the reactant, but the rate doesn’t change, it’s zero order.

Question 2

First order

Answer 2

If the reaction rate goes up by the same multiplicity as the concentration of the reactant, then it is first order.
Ex. Trial 1: 0.1M, 4 M/s = Trial 2: 0.4, 16 M/s

Question 3

Second order

Answer 3

If the multiplicity of the reactant concentration squared = the multiplicity of the reaction rate, it’s second order.
Ex. Trial 1: 0.1M, 4.0M/s
Trial 2: 0.2 M, 16.0M/s

0.1*2 (the multiplicity) = 0.2
2^2 = 4 and 4.0 *4 = 16

If you’re multiplying the concentration by 2, you multiply the reaction by 4. Same for 3 and 9 and 4 and 16.

Question 4

For the overall reaction order

Answer 4

Find the reaction order for A and B by looking at where it changes, then plug it in to the exponent of this equation: Rate = k[A]^x[B]^x

So if the order for “A” is 1 and the order for “B” is 2, the overall reaction order is: Rate= k[A]^1[B]^2