Chemical Kinetics · Chemistry · AP EAPCET

The rate constant of a reaction at 500 K and 700 K are $$0.02 \mathrm{~s}^{-1}$$ and $$0.2 \mathrm{~s}^{-1}$$ respectively. The activation energy of the reaction (in $$\left.\mathrm{kJ} \mathrm{mol}^{-1}\right)$$ is $$\left(R=8.3 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$$

The time required for completion of $$93.75 \%$$ of a first order reaction is $$x$$ minutes. The half-life of it (in minutes) is

. The rate constant for a zero order reaction $$A \longrightarrow$$ products is $$0.0030 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~S}^{-1}$$. How long it will take for the initial concentration of $$A$$ to fall from 0.10 M to 0.075 M ?

Which statement among the following is incorrect?

For zero order reaction, a plot of $$t_{1 / 2}$$ versus $$[A]_0$$ will be

If the rate constant for a first order reaction is $$2.303 \times 10^{-3} \mathrm{~s}^{-1}$$. Find the time required to reduce $$4 \mathrm{~g}$$ of the reactant to $$0.2 \mathrm{~g}$$.