Give examples of zero order reactions.
(N/A) Zero order reactions are relatively uncommon but they occur under special conditions.
Some enzyme-catalyzed reactions and reactions occurring on metal surfaces are examples of zero order reactions.
Example $1$: The decomposition of gaseous ammonia on a hot platinum surface is a zero order reaction at high pressure.
$2 NH_{3(g)} \xrightarrow{1130 \ K, Pt \text{ catalyst}} N_{2(g)} + 3 H_{2(g)}$
$Rate = k[NH_3]^0 = k$
In this reaction,platinum metal acts as a catalyst. At high pressure,the metal surface gets saturated with gas molecules. Therefore,further changes in concentration do not alter the amount of ammonia on the surface of the catalyst,making the rate of the reaction independent of its concentration.
Example $2$: The thermal decomposition of $HI$ on a gold surface is another example of a zero order reaction.
Some enzyme-catalyzed reactions and reactions occurring on metal surfaces are examples of zero order reactions.
Example $1$: The decomposition of gaseous ammonia on a hot platinum surface is a zero order reaction at high pressure.
$2 NH_{3(g)} \xrightarrow{1130 \ K, Pt \text{ catalyst}} N_{2(g)} + 3 H_{2(g)}$
$Rate = k[NH_3]^0 = k$
In this reaction,platinum metal acts as a catalyst. At high pressure,the metal surface gets saturated with gas molecules. Therefore,further changes in concentration do not alter the amount of ammonia on the surface of the catalyst,making the rate of the reaction independent of its concentration.
Example $2$: The thermal decomposition of $HI$ on a gold surface is another example of a zero order reaction.
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Similar Questions
For a reaction $A \to$ Products,a plot of $\log\,t_{1/2}$ versus $\log\,a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0,$ the order of the reaction is
DifficultAIEEE 2012
View SolutionWhich of the following is correct with respect to the graph given?
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$
The rates of a certain reaction $(dc/dt)$ at different times are as follows:
Time $(sec)$ Rate $(mole \ litre^{-1} \ sec^{-1})$ $0$ $2.8 \times 10^{-2}$ $10$ $2.78 \times 10^{-2}$ $20$ $2.81 \times 10^{-2}$ $30$ $2.79 \times 10^{-2}$
The reaction is:
| Time $(sec)$ | Rate $(mole \ litre^{-1} \ sec^{-1})$ |
|---|---|
| $0$ | $2.8 \times 10^{-2}$ |
| $10$ | $2.78 \times 10^{-2}$ |
| $20$ | $2.81 \times 10^{-2}$ |
| $30$ | $2.79 \times 10^{-2}$ |
The reaction is:
Medium
View SolutionWhich of the following is correct with respect to the graph given?
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$
For a zero order reaction,$A \longrightarrow \text{product}$,the concentration of $A$ decreases from $1.2 \ mol \ dm^{-3}$ to $0.4 \ mol \ dm^{-3}$ in $240 \ s$. What is the rate constant of the reaction?
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