An organic compound undergoes first order dec | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) For a first order reaction,the rate constant $k$ is given by $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$.For $t_{1/8}$,the remaining concentrat

Vedclass · Accepted Answer

$0.9$

Vedclass · Answer

(B) For a first order reaction,the rate constant $k$ is given by $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$.For $t_{1/8}$,the remaining concentration is $\frac{1}{8}$ of the initial concentration $[A]_0$,so $[A]_t = \frac{[A]_0}{8}$.$k t_{1/8} = 2.303 \log \frac{[A]_0}{[A]_0/8} = 2.303 \log 8 = 2.303 	imes 3 \log 2$.For $t_{1/10}$,the remaining concentration is $\frac{1}{10}$ of the initial concentration $[A]_0$,so $[A]_t = \frac{[A]_0}{10}$.$k t_{1/10} = 2.303 \log \frac{[A]_0}{[A]_0/10} = 2.303 \log 10 = 2.303 	imes 1$.Dividing the two equations:$\frac{t_{1/8}}{t_{1/10}} = \frac{3 \log 2}{1} = 3 	imes 0.30 = 0.9$.

An organic compound undergoes first order decomposition. The time taken for its decomposition to $\frac{1}{8}$ and $\frac{1}{10}$ of its initial concentration are $t_{1/8}$ and $t_{1/10}$ respectively. What is the value of $\frac{t_{1/8}}{t_{1/10}}$? $[\log 2 = 0.30]$

Similar Questions

Calculate the half-life of the first-order reaction $C_2H_4O_{(g)} \to CH_{4(g)} + CO_{(g)}$ if the initial pressure of $C_2H_4O_{(g)}$ is $80 \ mm$ and the total pressure at the end of $20 \ minutes$ is $120 \ mm$. (in $min$)

In a first-order reaction,the concentration of the reactant decreases from $1.0 \, M$ to $0.25 \, M$ in $20 \, \text{minutes}$. What will be the rate constant of the reaction?

For the reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$,the rate constant is $3.0 \times 10^{-5} \ s^{-1}$. If the rate of reaction is $2.40 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$,calculate the concentration of $N_2O_5$ in $mol \ L^{-1}$.

For a first-order reaction,it takes $20 \, \text{min}$ for the concentration to decrease from $1 \, M$ to $0.6 \, M$. How much time is required for the concentration to decrease from $0.6 \, M$ to $0.36 \, M$?

If the rate constant of a first-order reaction is $0.6932 \ hr^{-1}$,then its half-life period is .......... $hr$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module