Medium
The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the
- ARate of formation of $C$ is twice the rate of disappearance of $A$
- B$t_{1/2}$ is a constant
- CUnit of $k$ must be $s^{-1}$
- DValue of $k$ is independent of the initial concentrations of $A$ and $B$
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Similar Questions
For the reaction $A + B \longrightarrow \text{product}$,the rate law equation is $\text{rate} = k[A]^2[B]$. If the rate of reaction is $0.22 \ mol \ L^{-1} \ s^{-1}$,calculate the rate constant $k$. Given: $[A] = 1 \ mol \ L^{-1}, [B] = 0.25 \ mol \ L^{-1}$.
Fill in the blanks:
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$
Difficult
View SolutionBy “the overall order of a reaction”,we mean
Easy
View SolutionFor a reaction $A + B \to$ product,it was found that the rate of reaction increases four times if the concentration of $A$ is doubled,but the rate of reaction remains unaffected if the concentration of $B$ is doubled. Hence,the rate law for the reaction is
Medium
View SolutionTotal order of reaction $X + Y \rightarrow XY$ is $3$. The order of reaction with respect to $X$ is $2$. State the differential rate equation for the reaction.
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