(A) The rate of reaction is given by the expression: $\text{Rate} = -\frac{1}{2} \frac{d[MnO_4^-]}{dt} = \frac{1}{5} \frac{d[I_2]}{dt}$.Given that the

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$1.14 \times 10^{-2} \ Ms^{-1}$

(A) The rate of reaction is given by the expression: $\text{Rate} = -\frac{1}{2} \frac{d[MnO_4^-]}{dt} = \frac{1}{5} \frac{d[I_2]}{dt}$.Given that the rate of disappearance of $MnO_4^-$ is $-\frac{d[MnO_4^-]}{dt} = 4.56 \times 10^{-3} \ Ms^{-1}$.Substituting this into the rate expression: $\frac{1}{2} \times (4.56 \times 10^{-3}) = \frac{1}{5} \frac{d[I_2]}{dt}$.Therefore,the rate of appearance of $I_2$ is $\frac{d[I_2]}{dt} = \frac{5}{2} \times 4.56 \times 10^{-3} \ Ms^{-1} = 1.14 \times 10^{-2} \ Ms^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56 \times 10^{-3} \ Ms^{-1}$,$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$. The rate of appearance of $I_2$ is

A
$1.14 \times 10^{-2} \ Ms^{-1}$
B
$5.7 \times 10^{-3} \ Ms^{-1}$
C
$4.56 \times 10^{-4} \ Ms^{-1}$
D
$1.14 \times 10^{-3} \ Ms^{-1}$

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Rate of a reaction

$R \longrightarrow P$ is a first order reaction. The concentration of $R$ changed from $0.04$ to $0.03 \ mol \ L^{-1}$ in $40 \ min$. What is the average velocity of the reaction in $mol \ L^{-1} \ s^{-1}$?

MediumAP EAMCET 2025

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$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:

MediumAP EAMCET 2021

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Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

MediumAP EAMCET 2021

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Consider the reaction given below:
$A + 2 B \longrightarrow 3 C + 2 D$.
If the rate of disappearance of $B$ is $x \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$,the ratio of the rate of reaction and the rate of appearance of $C$ is:

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Find the average rate of formation of $O_{2(g)}$ in the following reaction:
$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$
Given that $\left[-\frac{\Delta[NO_2]}{\Delta t}\right] = x \ mol \ dm^{-3} \ s^{-1}$

MediumMHT CET 2023

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The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56 \times 10^{-3} \ Ms^{-1}$,$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$. The rate of appearance of $I_2$ is

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$R \longrightarrow P$ is a first order reaction. The concentration of $R$ changed from $0.04$ to $0.03 \ mol \ L^{-1}$ in $40 \ min$. What is the average velocity of the reaction in $mol \ L^{-1} \ s^{-1}$?

$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:

Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

Consider the reaction given below:$A + 2 B \longrightarrow 3 C + 2 D$.If the rate of disappearance of $B$ is $x \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$,the ratio of the rate of reaction and the rate of appearance of $C$ is:

Find the average rate of formation of $O_{2(g)}$ in the following reaction: $2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$ Given that $\left[-\frac{\Delta[NO_2]}{\Delta t}\right] = x \ mol \ dm^{-3} \ s^{-1}$

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Consider the reaction given below:
$A + 2 B \longrightarrow 3 C + 2 D$.
If the rate of disappearance of $B$ is $x \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$,the ratio of the rate of reaction and the rate of appearance of $C$ is:

Find the average rate of formation of $O_{2(g)}$ in the following reaction:
$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$
Given that $\left[-\frac{\Delta[NO_2]}{\Delta t}\right] = x \ mol \ dm^{-3} \ s^{-1}$