The rate equation for a reaction,
$${N_2}O \to {N_2} + \frac{1}{2}{O_2}$$
is Rate $$ = k{\left[ {{N_2}O} \right]^0} = k.$$ If the initial concentration of the reactant is $$a\,mol\,Li{t^{ - 1}},$$ the half-life period of the reaction is
A.
$${t_{\frac{1}{2}}} = \frac{a}{{2k}}$$
B.
$$ - {t_{\frac{1}{2}}} = ka$$
C.
$${t_{\frac{1}{2}}} = \frac{a}{k}$$
D.
$${t_{\frac{1}{2}}} = \frac{k}{a}$$
Answer :
$${t_{\frac{1}{2}}} = \frac{a}{{2k}}$$
Solution :
For a zero order reaction
$${t_{\frac{1}{2}}} = \frac{a}{{2k}}$$
Releted MCQ Question on Physical Chemistry >> Chemical Kinetics
Releted Question 1
If uranium (mass number 238 and atomic number 92) emits an $$\alpha $$ -particle, the product has mass no. and atomic no.