(A) For a first-order reaction $R \rightarrow P$,the rate law is given by $\text{Rate} = k[R]^1$.Since the rate of disappearance of reactant $R$ is de

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(A) For a first-order reaction $R \rightarrow P$,the rate law is given by $\text{Rate} = k[R]^1$.Since the rate of disappearance of reactant $R$ is defined as $-\frac{d[R]}{dt}$,we have $\text{Rate} = -\frac{d[R]}{dt} = k[R]$.Therefore,Statement $I$ is True $(T)$.Statement $II$ suggests $\text{Rate} = -k[R]$,which is incorrect because the rate of a reaction must always be a positive quantity,and the rate constant $k$ is positive. Thus,Statement $II$ is False $(F)$.

Class 12 Chemistry Chemical Kinetics First Order reaction

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Identify True $(T)$ and False $(F)$ statements for the following expressions regarding a first-order reaction $R \rightarrow P$:
Statement $I$: $\text{Rate} = -\frac{d[R]}{dt} = k[R]$
Statement $II$: $\text{Rate} = -\frac{d[R]}{dt} = -k[R]$

A
$I-T, II-F$
B
$I-F, II-T$
C
$I-T, II-T$
D
$I-F, II-F$

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Chemical Kinetics

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First Order reaction

Consider a general first order reaction $A_{(g)} \rightarrow B_{(g)} + C_{(g)}$. If the initial pressure is $200 \ mm$ and after $20 \ minutes$ it is $250 \ mm$,then the half-life period of the reaction (in minutes) is. $(\log 2 = 0.30, \log 3 = 0.48, \log 4 = 0.60)$

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At $T(K)$,if the rate constant of a first order reaction is $4.606 \times 10^{-3} \ s^{-1}$,the time to reduce the initial concentration of the reactant to $1/10$ of its initial value in seconds is:

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For which of the following reactions is the half-life period independent of the initial concentration of the reactant?

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$A$ first order reaction has a rate constant of $1.5 \times 10^{-3} \ s^{-1}$. How long will $5.0 \ g$ of this reactant take to reduce to $3.0 \ g$?

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For the reaction $2A + B \to \text{product}$,the rate law is given by $\frac{-d[A]}{dt} = k[A]$. At a time $t = \frac{t_{1/2}}{\ln 2}$,what is the concentration of the reactant $A$?

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Identify True $(T)$ and False $(F)$ statements for the following expressions regarding a first-order reaction $R \rightarrow P$:Statement $I$: $\text{Rate} = -\frac{d[R]}{dt} = k[R]$Statement $II$: $\text{Rate} = -\frac{d[R]}{dt} = -k[R]$

Similar Questions

Consider a general first order reaction $A_{(g)} \rightarrow B_{(g)} + C_{(g)}$. If the initial pressure is $200 \ mm$ and after $20 \ minutes$ it is $250 \ mm$,then the half-life period of the reaction (in minutes) is. $(\log 2 = 0.30, \log 3 = 0.48, \log 4 = 0.60)$

At $T(K)$,if the rate constant of a first order reaction is $4.606 \times 10^{-3} \ s^{-1}$,the time to reduce the initial concentration of the reactant to $1/10$ of its initial value in seconds is:

For which of the following reactions is the half-life period independent of the initial concentration of the reactant?

$A$ first order reaction has a rate constant of $1.5 \times 10^{-3} \ s^{-1}$. How long will $5.0 \ g$ of this reactant take to reduce to $3.0 \ g$?

For the reaction $2A + B \to \text{product}$,the rate law is given by $\frac{-d[A]}{dt} = k[A]$. At a time $t = \frac{t_{1/2}}{\ln 2}$,what is the concentration of the reactant $A$?

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Identify True $(T)$ and False $(F)$ statements for the following expressions regarding a first-order reaction $R \rightarrow P$:
Statement $I$: $\text{Rate} = -\frac{d[R]}{dt} = k[R]$
Statement $II$: $\text{Rate} = -\frac{d[R]}{dt} = -k[R]$