Question

Given the data in the accompanying table, what is the reaction order for B?

Answer 1

Answer: The order with respect to B is

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$Rate=k[A]^x[B]^y$

k= rate constant

x = order with respect to A

y = order with respect to B

n = x+y = Total order

a) From trial 1: $20=k[0.20]^x[0.10]^y$    (1)

From trial 2: $40=k[0.20]^x[0.20]^y$    (2)

Dividing 2 by 1 :$\frac{40}{20}=\frac{k[0.20]^x[0.20]^y}{k[0.20]^x[0.10]^y}$

$2=2^y,2^1=2^y$ therefore y=1.

Thus order with respect to B is 1.

Answer 2

B
As the concentration of B was doubled, the reaction rate doubled.