The rate of disappearance of $MnO_4^-$ in the following reaction is $4.56 \times 10^{-3} \ M/s$.
$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$
The rate of appearance of $I_2$ is:

In a reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of appearance of $NH_3$ is $2.5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$. The rate of reaction and rate of disappearance of $H_2$ will be (in $mol \ L^{-1} s^{-1}$):

For the reaction $R \rightarrow P$,the concentration of a reactant changes from $0.03 \, M$ to $0.02 \, M$ in $25 \, minutes$. Calculate the average rate of reaction using units of time both in $minutes$ and $seconds$.

In the reaction,$BrO_{3(aq)}^{-} + 5Br_{(aq)}^{-} + 6H^{+} \to 3Br_{2(l)} + 3H_2O_{(l)}$. The rate of appearance of bromine $(Br_2)$ is related to the rate of disappearance of bromide ions as:

Assertion : The rate of the reaction is the rate of change of concentration of a reactant or a product.
Reason : Rate of reaction remains constant during the course of reaction.

In a catalytic conversion of $N_2$ to $NH_3$ by Haber's process,the rate of reaction was expressed as change in the concentration of ammonia per time is $40 \times 10^{-3} \ mol \ L^{-1} s^{-1}$. If there are no side reactions,the rate of the reaction as expressed in terms of hydrogen is (in $mol \ L^{-1} s^{-1}$)