(C) The reaction is $C_2H_4O_{(g)} \to CH_{4(g)} + CO_{(g)}$.Initial pressure $(t=0)$: $P_0 = 80 \ mm$,$P_{CH_4} = 0$,$P_{CO} = 0$.At $t = 20 \ min$:

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(C) The reaction is $C_2H_4O_{(g)} \to CH_{4(g)} + CO_{(g)}$.Initial pressure $(t=0)$: $P_0 = 80 \ mm$,$P_{CH_4} = 0$,$P_{CO} = 0$.At $t = 20 \ min$: $(80-x) + x + x = 120 \ mm \implies 80 + x = 120 \implies x = 40 \ mm$.The pressure of $C_2H_4O$ remaining is $80 - 40 = 40 \ mm$.Since the pressure reduced to half ($80 \ mm$ to $40 \ mm$) in $20 \ minutes$,the half-life $t_{1/2}$ is $20 \ min$.Thus,option $C$ is correct.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

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 $120 \ mm$,find the half-life in $\text{min}$.

A
$40$
B
$120$
C
$20$
D
$80$

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Chemical Kinetics

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First Order reaction

Consider the first order reaction $R \to P$. The fraction of molecules decomposed in the given first order reaction can be expressed as:

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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 $120 \ mm$,find the half-life in $\text{min}$.

Similar Questions

Consider the first order reaction $R \to P$. The fraction of molecules decomposed in the given first order reaction can be expressed as:

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 $mol \ L^{-1}$.

Half-life and rate constant for a first-order reaction are related by the equation:

For the first order reaction $A \rightarrow B$,the rate constant is $0.25 \ s^{-1}$. If the concentration of $A$ is reduced to half,the value of the rate constant will be: (in $s^{-1}$)

For a first order reaction,the rate constant is $0.6932 \ hr^{-1}$,then the half-life for the reaction is ......... $hr$.

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