(B) For a first order reaction,the half-life $(t_{1/2})$ is given by the formula $t_{1/2} = \frac{\ln(2)}{k} \approx \frac{0.693}{k}$.Statement $1$: $

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(B) For a first order reaction,the half-life $(t_{1/2})$ is given by the formula $t_{1/2} = \frac{\ln(2)}{k} \approx \frac{0.693}{k}$.Statement $1$: $t_{1/2} = \frac{0.693}{2k}$ is False because the correct expression is $\frac{0.693}{k}$.Statement $2$: $t_{1/2} \propto k$ is False because $t_{1/2}$ is inversely proportional to the rate constant $(t_{1/2} \propto \frac{1}{k})$.Therefore,both statements are False $(F, F)$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Easy

Identify True $(T)$ and False $(F)$ statements for the following first order reaction $R \rightarrow P$:
$1. t_{1/2} = \frac{0.693}{2k}$
$2. t_{1/2} \propto k$

A
$1-T, 2-T$
B
$1-F, 2-F$
C
$1-T, 2-F$
D
$1-F, 2-T$

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Chemical Kinetics

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First Order reaction

In a first-order reaction,the rate constant $k = 70 \, s^{-1}$. How much time is required for the concentration to become $\frac{1}{18}$ of the initial concentration (in $, s$)?

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Initial concentration of reactant in a first order reaction is $0.08 \text{ mol dm}^{-3}$. What concentration would remain after $40 \text{ minutes}$? (Given $\frac{[A]_0}{[A]_t} = 5.00$)

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For two first-order reactions:
$A \rightarrow \text{Products}$
$B \rightarrow \text{Products}$
If at the same time,$50\% \, B$ has reacted and $94\% \, A$ has reacted,calculate the ratio $K_1/K_2$.

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Which of the following relations is correct for the given reaction orders?

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Mathematical representation for $t_{1/4}$ life for a first-order reaction is given by:

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Identify True $(T)$ and False $(F)$ statements for the following first order reaction $R \rightarrow P$:$1. t_{1/2} = \frac{0.693}{2k}$$2. t_{1/2} \propto k$

Similar Questions

In a first-order reaction,the rate constant $k = 70 \, s^{-1}$. How much time is required for the concentration to become $\frac{1}{18}$ of the initial concentration (in $, s$)?

Initial concentration of reactant in a first order reaction is $0.08 \text{ mol dm}^{-3}$. What concentration would remain after $40 \text{ minutes}$? (Given $\frac{[A]_0}{[A]_t} = 5.00$)

For two first-order reactions:$A \rightarrow \text{Products}$$B \rightarrow \text{Products}$If at the same time,$50\% \, B$ has reacted and $94\% \, A$ has reacted,calculate the ratio $K_1/K_2$.

Which of the following relations is correct for the given reaction orders?

Mathematical representation for $t_{1/4}$ life for a first-order reaction is given by:

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Identify True $(T)$ and False $(F)$ statements for the following first order reaction $R \rightarrow P$:
$1. t_{1/2} = \frac{0.693}{2k}$
$2. t_{1/2} \propto k$

For two first-order reactions:
$A \rightarrow \text{Products}$
$B \rightarrow \text{Products}$
If at the same time,$50\% \, B$ has reacted and $94\% \, A$ has reacted,calculate the ratio $K_1/K_2$.