The reaction $2A \rightarrow B + C$ follows zero-order kinetics when:
- AThe rate of reaction is proportional to the square of the concentration of $A$.
- BThe rate of reaction remains constant at any concentration of $A$.
- CThe rate does not change with the concentrations of $B$ and $C$.
- DThe rate of reaction doubles when the concentration of $A$ is doubled.
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Similar Questions
Identify the following statements as True $(T)$ or False $(F)$ for a zero-order reaction $R \to P$:
$(i) \ d[R] = -k dt$
$(ii) \ d[R] = +k dt$
$(i) \ d[R] = -k dt$
$(ii) \ d[R] = +k dt$
Easy
View SolutionFor a zero-order reaction with rate constant $k$,the slope of the plot of reactant concentration against time is
MediumKVPY 2013
View SolutionConsider 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:
Medium
View SolutionThe half-life period for a certain zero-order reaction is $10 \text{ min}$. How much time is required for this reaction to complete $100\%$ (in $\text{ min}$)?
DifficultGUJCET 2025
View SolutionWhich of the following plots is correct for a zero-order reaction?
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