$A$ reaction $2A \to$ products is found to follow zero order kinetics,then
- A$\frac{dx}{dt} = k[A]^2$
- B$\frac{dx}{dt} = k[A]^0$
- C$\frac{dx}{dt} = k[A]$
- D$\frac{dx}{dt} = k[2A]$
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Similar Questions
At high pressure,the following reaction is zero order:
$2NH_{3(g)} \xrightarrow[Pt \ \text{catalyst}]{1130 \ K} N_{2(g)} + 3H_{2(g)}$
Choose the option which is not true with respect to the reaction,from the choices given below:
$2NH_{3(g)} \xrightarrow[Pt \ \text{catalyst}]{1130 \ K} N_{2(g)} + 3H_{2(g)}$
Choose the option which is not true with respect to the reaction,from the choices given below:
Difficult
View SolutionThe rate equation for a reaction $A \rightarrow B$ is $r=k[A]^{0}$. If the initial concentration of the reactant is $a \ mol \ dm^{-3}$,the half-life period of the reaction is
What is the unit of $K$ for a zero-order reaction?
Easy
View SolutionWhich of the following is correct with respect to the graph given?
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$
Which among the following is an example of a zero order reaction?
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