The reaction 2X $$ \to $$ B is a zeroth order reaction. If the initial concentration of X is 0.2 M, the half-life is 6 h. When the initial concentration of X is 0.5 M, the time required to reach its final concentration of 0.2 M will be:

If a reaction follows the Arrhenius equation, the plot ln k vs $${1 \over {\left( {RT} \right)}}$$ gives straight line with a gradient ($$-$$ y) unit.

The energy required to active the reactant is :

For an elementary chemical reaction,



the expression for $${{d\left[ A \right]} \over {dt}}$$ is

Consider the given plots for a reaction obeying Arrhenius equation (0^oC < T < 300^oC) : (K and Ea are rate constant and activation energy, respectively)



Choose the correct option :