For the reaction $A \to B$,the rate law expression is: $\text{Rate} = k[A]$. Which of the following statements is incorrect?
- AThe reaction is said to follow first-order kinetics.
- BThe half-life of the reaction will depend on the initial concentration of the reactant.
- C$k$ is constant for the reaction at a constant temperature.
- DThe rate law provides a simple way of predicting the concentration of reactants and products at any time after the start of the reaction.
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Similar Questions
For a first order reaction,the rate constant is given as $\log_{10} K = 12 - \frac{6 \times 10^3}{T}$. What will be the value of temperature if its half-life period is $6.93 \times 10^{-3} \, \text{min}$ (in $, K$)?
Difficult
View SolutionReaction $A_{(g)} \rightarrow 2B_{(g)} + C_{(g)}$ is a first order reaction. It was started with pure $A$.
$t/min$ Pressure of system at time $t/mm \ Hg$ $10$ $160$ $\infty$ $240$
Which of the following option is incorrect?
| $t/min$ | Pressure of system at time $t/mm \ Hg$ |
| $10$ | $160$ |
| $\infty$ | $240$ |
DifficultJEE MAIN 2025
View SolutionHalf life of a first order reaction is $20 \ min$. The time taken to reduce the initial concentration of reactant to $(1/10)^{th}$ is $\qquad$ (in $min$)
$PCl_{5(g)} \rightarrow PCl_{3(g)} + Cl_{2(g)}$
In the above first order reaction,the concentration of $PCl_{5}$ reduces from an initial concentration of $50 \ mol \ L^{-1}$ to $10 \ mol \ L^{-1}$ in $120 \ minutes$ at $300 \ K$. The rate constant for the reaction at $300 \ K$ is $X \times 10^{-2} \ min^{-1}$. The value of $X$ is $......$
$[$ Given $\log 5 = 0.6989 ]$
In the above first order reaction,the concentration of $PCl_{5}$ reduces from an initial concentration of $50 \ mol \ L^{-1}$ to $10 \ mol \ L^{-1}$ in $120 \ minutes$ at $300 \ K$. The rate constant for the reaction at $300 \ K$ is $X \times 10^{-2} \ min^{-1}$. The value of $X$ is $......$
$[$ Given $\log 5 = 0.6989 ]$
DifficultJEE MAIN 2021
View SolutionCalculate the time required for a reactant to decrease in concentration from $100 \%$ to $20 \%$,if the rate constant of the first-order reaction is $0.02303 \ hour^{-1}$. (in $hour$)
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