In a reaction,reactant $A$ decomposes $10 \%$ in $1 \ hour$,$20 \%$ in $2 \ hours$ and $30 \%$ in $3 \ hours$. The unit of rate constant of this reaction is
- A$sec^{-1}$
- B$mol \ L^{-1} \ sec^{-1}$
- C$L \ mol^{-1} \ sec^{-1}$
- D$L^{2} \ mol^{-2} \ sec^{-1}$
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Similar Questions
Which of the following is correct with respect to the graph given?
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$
At high pressure,the following reaction is zero order:
$2NH_{3(g)} \xrightarrow[Pt \ \text{catalyst}]{1130 \ K} N_{2(g)} + 3H_{2(g)}$
Choose the option which is not true with respect to the reaction,from the choices given below:
$2NH_{3(g)} \xrightarrow[Pt \ \text{catalyst}]{1130 \ K} N_{2(g)} + 3H_{2(g)}$
Choose the option which is not true with respect to the reaction,from the choices given below:
Difficult
View SolutionThe rate constant of a zero order reaction is $2.0 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,then find the initial concentration of the reactant. (in $M$)
For a zero-order reaction,the rate constant $K = 2 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,then its initial concentration must be ...... $M$.
Medium
View SolutionIn the following reaction $A \to B + C$,the rate constant is $0.001 \, M/sec$. If we start with $1 \, M$ of $A$,the concentrations of $A$ and $B$ after $10$ minutes are respectively:
Medium
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