In 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:
- A$0.5 \, M, 0.5 \, M$
- B$0.6 \, M, 0.4 \, M$
- C$0.4 \, M, 0.6 \, M$
- DNone of these
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If the rate of a reaction is equal to the rate constant,what is the order of the reaction?
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View SolutionFor a zero order reaction $A \longrightarrow \text{product}$,the concentration of $A$ decreases from $0.8 \ mol \ dm^{-3}$ to $0.2 \ mol \ dm^{-3}$ in $6 \ minute$. What is the rate constant of the reaction?
Consider the data given below for the hypothetical reaction $A \to X$:
$Time \ (s)$ $Rate \ (mol \ L^{-1} s^{-1})$ $0$ $1.60 \times 10^{-2}$ $10$ $1.60 \times 10^{-2}$ $20$ $1.60 \times 10^{-2}$ $30$ $1.60 \times 10^{-2}$
From the above data,the order of the reaction is:
| $Time \ (s)$ | $Rate \ (mol \ L^{-1} s^{-1})$ |
|---|---|
| $0$ | $1.60 \times 10^{-2}$ |
| $10$ | $1.60 \times 10^{-2}$ |
| $20$ | $1.60 \times 10^{-2}$ |
| $30$ | $1.60 \times 10^{-2}$ |
From the above data,the order of the reaction is:
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View SolutionAt $T \ K$,if the rate constant for a zero order reaction is $2.5 \times 10^{-3} \ M \ s^{-1}$,the time required for the initial concentration of reactant $R$ to fall from $0.10 \ M$ to $0.075 \ M$ at the same temperature in seconds is:
The reaction $A \to \text{Products}$ is a zero-order reaction. If the initial concentration of $A$ is $2 \ M$,then at time $t = 1/K$ (where $K$ is the rate constant),the concentration of $A$ will be ......... $M$.
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