For a zero order reaction:
- AThe concentration of the reactant does not change during the reaction.
- BThe concentration changes only when the temperature changes.
- CThe rate remains constant throughout.
- DThe rate of the reaction is proportional to the concentration.
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Similar Questions
The rate constant,$k$ of a zero order reaction $2 NH_{3(g)} \xrightarrow[1130 \ K]{Pt} N_{2(g)} + 3 H_{2(g)}$ is $y \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of hydrogen (in $mol \ L^{-1} \ s^{-1}$) is
The unit of rate constant for a zero order reaction is
Easy
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 SolutionMention True $(T)$ and False $(F)$ statements for the following equations related to the reaction $R \to P$:
$I. [R] = -kt + [R]_0$
$II. [R] = kt + [R]_0$
$I. [R] = -kt + [R]_0$
$II. [R] = kt + [R]_0$
Easy
View SolutionFor a reaction $A \rightarrow P$ at $T \text{ K}$, the half-life $(t_{1/2})$ is plotted as a function of initial concentration $[A]_0$ of $A$ as given below. The value of $x$ in the given figure is . . . . . . $\text{s}$ (Nearest integer).
DifficultJEE MAIN 2026
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