Medium
The rate law for the reaction $A + B \rightarrow \text{product}$ is $\text{rate} = k[A][B]$. When will the rate of reaction increase by a factor of $2$?
- A$[A]$ and $[B]$ both are doubled
- B$[A]$ is doubled and $[B]$ is kept constant
- C$[B]$ is doubled and $[A]$ is halved
- D$[A]$ is kept constant and $[B]$ is halved
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For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:
DifficultJEE MAIN 2019
View SolutionFor a certain reaction,the expression for half-life is $t_{1/2} \propto \frac{1}{a^{n-1}}$. What is the order of the reaction?
Medium
View SolutionFor the reaction $A + B \rightarrow$ products,it is observed that
$(i)$ on doubling the initial concentration of $A$ only,the rate of reaction is also doubled and
$(ii)$ on doubling the initial concentration of both $A$ and $B$,there is a change by a factor of $8$ in the rate of the reaction.
The rate of this reaction is given by
$(i)$ on doubling the initial concentration of $A$ only,the rate of reaction is also doubled and
$(ii)$ on doubling the initial concentration of both $A$ and $B$,there is a change by a factor of $8$ in the rate of the reaction.
The rate of this reaction is given by
Which one of the following statements regarding the order of a reaction is not correct?
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