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Which of the following statements is false?
- AFor an endothermic reaction,energy of product is greater than that of reactant.
- BThe rate law for a reaction depends on the concentrations of all reactants that appear in the stoichiometric equation.
- CThe rate of a zero order reaction is independent of the concentration of the catalyst.
- DThe specific rate constant for a reaction is independent of the concentrations of the reacting species.
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Similar Questions
By “the overall order of a reaction”,we mean
Easy
View SolutionIf the relation between half-life time $(t_{1/2})$ and initial concentration $[R]_0$ is given by $t_{1/2} \propto \frac{1}{[R]_0^{n-1}}$,what is the order of the reaction?
For a reaction $A \rightarrow 2 B + C$ the half-lives are $100 \ s$ and $50 \ s$ when the concentration of reactant $A$ is $0.5 \ mol \ L^{-1}$ and $1.0 \ mol \ L^{-1}$ respectively. The order of the reaction is (Nearest Integer).
If a reaction occurs in the following two steps:
$i) \ 2 ClO^{-} \rightarrow ClO_2^{-} + Cl^{-}$
$ii) \ ClO_2^{-} + ClO^{-} \rightarrow ClO_3^{-} + Cl^{-}$
Find the reaction intermediate.
$i) \ 2 ClO^{-} \rightarrow ClO_2^{-} + Cl^{-}$
$ii) \ ClO_2^{-} + ClO^{-} \rightarrow ClO_3^{-} + Cl^{-}$
Find the reaction intermediate.
In a reaction between $A$ and $B$,the initial rate of reaction $(r_0)$ was measured for different initial concentrations of $A$ and $B$ as given below:
$A / mol \ L^{-1}$ $0.20$ $0.20$ $0.40$ $B / mol \ L^{-1}$ $0.30$ $0.10$ $0.05$ $r_0 / mol \ L^{-1} \ s^{-1}$ $5.07 \times 10^{-5}$ $5.07 \times 10^{-5}$ $1.43 \times 10^{-4}$
What is the order of the reaction with respect to $A$ and $B$?
| $A / mol \ L^{-1}$ | $0.20$ | $0.20$ | $0.40$ |
| $B / mol \ L^{-1}$ | $0.30$ | $0.10$ | $0.05$ |
| $r_0 / mol \ L^{-1} \ s^{-1}$ | $5.07 \times 10^{-5}$ | $5.07 \times 10^{-5}$ | $1.43 \times 10^{-4}$ |
What is the order of the reaction with respect to $A$ and $B$?
Difficult
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