The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
Experiment - A/mol L-1 - B/ mol L-1 - Initial rate/mol L-1 min-1
I - 0.1 - 0.1 - 2.0 x 10-2
II - .... - 0.2 - 4.0 x 10-2
III - 0.4 - 0.4 - .....
IV - .... - 0.2 - 2.0 x 10-2
The given reaction is of the first order with respect to A and of zero order with respect to B.
Therefore, the rate of the reaction is given by,
Rate = k [A]1 [B]0
⇒ Rate = k [A]
From experiment I, we obtain
2.0 x 10-2 mol L-1 min-1 = k (0.1 mol L-1)
⇒ k = 0.2 min-1
From experiment II, we obtain
4.0 x 10-2 mol L-1 min-1 = 0.2 min-1 [A]
⇒ [A] = 0.2 mol L-1
From experiment III, we obtain
Rate = 0.2 min-1 x 0.4 mol L-1
= 0.08 mol L-1 min-1
From experiment IV, we obtain
2.0 x 10-2 mol L-1 min-1 = 0.2 min-1 [A]
⇒ [A] = 0.1 mol L-1