Fill in the blanks:
$(a)$ Catalyst ......... the rate of reaction.
$(b)$ Inhibitor ......... the rate of the reaction.
$(c)$ If temperature increases,the rate of reaction ......... .
$(a)$ Catalyst ......... the rate of reaction.
$(b)$ Inhibitor ......... the rate of the reaction.
$(c)$ If temperature increases,the rate of reaction ......... .
(N/A) Catalyst increases the rate of reaction by providing an alternative pathway with lower activation energy.
$(b)$ Inhibitor decreases the rate of reaction by increasing the activation energy or by consuming the active species.
$(c)$ If temperature increases,the rate of reaction increases because the number of effective collisions increases.
$(b)$ Inhibitor decreases the rate of reaction by increasing the activation energy or by consuming the active species.
$(c)$ If temperature increases,the rate of reaction increases because the number of effective collisions increases.
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Similar Questions
In a reaction $R \to P$,the concentration $[M]$ obtained at different times $(t)$ are shown in the following table. Calculate the average rate $r_{av}$ of the reaction.
Time $t$ $(s)$ $0$ $5$ $10$ $20$ $30$ Concentration $(mol \ L^{-1})$ $160 \times 10^{-3}$ $80 \times 10^{-3}$ $40 \times 10^{-3}$ $10 \times 10^{-3}$ $3.5 \times 10^{-3}$
| Time $t$ $(s)$ | $0$ | $5$ | $10$ | $20$ | $30$ |
| Concentration $(mol \ L^{-1})$ | $160 \times 10^{-3}$ | $80 \times 10^{-3}$ | $40 \times 10^{-3}$ | $10 \times 10^{-3}$ | $3.5 \times 10^{-3}$ |
Medium
View SolutionObserve the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?
For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ L^{-1} \ h^{-1}$. The rate of consumption of $H_2$ under the same condition is $..... \ kg \ L^{-1} \ h^{-1}$.
Difficult
View SolutionThe 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:
$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$
The rate of appearance of $I_2$ is:
Medium
View Solution$A \rightarrow P$ 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:
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