Isomerisation of gaseous cyclobutene to butadiene is first order reaction. At $T(\mathrm{~K})$. The rate constant of reaction is $33 \times 10^{-4} \mathrm{~s}^{-1}$. What is the time required (in min ) to complete $90 \%$ of this reaction at the temperature? $(\log 2=03)$
$5 \mathrm{Br}^{-}(a q)+\mathrm{BrO}_3^{-}(a q)+6 \mathrm{H}^{+}(a q) \longrightarrow 3 \mathrm{Br}_2(a q)+3 \mathrm{H}_2 \mathrm{O}(l)$ is $X$ $\mathrm{mol} \mathrm{L} \mathrm{min}^{-1}$. What is the rate (in $\mathrm{mol} \mathrm{L}^{-1} \mathrm{~min}^{-1}$ ) of this reaction?
For a first order reaction the concentration of reactant was reduced from $0.03 \mathrm{molL}^{-1}$ to $0.02 \mathrm{molL}^{-1}$ in 25 min . What is its rate (in $\mathrm{molL}^{-1} \mathrm{~s}^{-1}$ )?
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 $$0.2 \mathrm{~g}$$.