Question

The rate of the reaction. (write the value to the nearest integer)
A + B $\to$ Products is given below as a function of different initial concentration of A and B.
The half-life(in min) of A in the reaction is

[A] $\left(moi{L}^{-1}\right)$	[B] $\left(moi{L}^{-1}\right)$	Initial rate $\left(mol{L}^{-1}mi{n}^{-1}\right)$
0.01	0.01	0.005
0.02	0.01	0.010
0.01	0.02	0.005

Answer 1

From careful observation of the given data, it can be concluded that doubling the concentration of A alone doubles the rate of the reaction, therefore order with respect to A is one. Doubling the concentration of B alone does not affect the rate of the reaction, therefore order with respect to B is zero.
Rate = $k\left[A\right][B{]}^0=k[A]$
or 0.005 = $k\times 0.01$
or $k=\frac{0.005}{0.01}=0.5mi{n}^{-1}$
Half life = $\frac{0.693}{k}=\frac{0.693}{0.5}=1.386min$