(C) For a first order reaction,the rate equation is given by:$t = \frac{2.303}{k} \log \frac{a}{a-x}$Given that the reaction is $90 \%$ complete,we ha

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

(C) For a first order reaction,the rate equation is given by:$t = \frac{2.303}{k} \log \frac{a}{a-x}$Given that the reaction is $90 \%$ complete,we have $a = 100$ and $(a-x) = 100 - 90 = 10$.The rate constant $k = 6.93 \times 10^{-2} \ min^{-1}$.Substituting these values into the equation:$t = \frac{2.303}{6.93 \times 10^{-2}} \log \frac{100}{10}$$t = \frac{2.303}{0.0693} \times \log(10)$Since $\log(10) = 1$,we get:$t = \frac{2.303}{0.0693} \approx 33.23 \ min$.The nearest integer value is $33 \ min$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

If benzene diazonium chloride undergoes first order decomposition at $T \ K$ with a rate constant of $6.93 \times 10^{-2} \ min^{-1}$,the time for completion of $90 \%$ of the reaction (in $min$) is (nearest integer) $(\log 2 = 0.30, \log 3 = 0.477)$.

TS EAMCET 2023 All TS EAMCET

A
$15$
B
$30$
C
$33$
D
$43$

Explore More

Browse All

Question Bank

All Subjects

Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

First Order reaction

Previous Year

TS EAMCET 2023 Paper All TS EAMCET years →

The value of rate constant for a first order reaction is $2.303 \times 10^{-2} \text{ s}^{-1}$. What will be the time required to reduce the concentration to $\frac{1}{10}$th of its initial concentration (in $\text{ s}$)?

EasyGUJCET 2014

View Solution

In a first order reaction $A \to B,$ if $k$ is the rate constant and the initial concentration of the reactant $A$ is $0.5 \ M,$ then the half-life is:

Medium

View Solution

In a first-order reaction of the type: $A_{(g)} \to 2B_{(g)}$,the initial pressure is $P_i$ and the total pressure at time $t$ is $P_t$. The rate constant $k$ can be expressed as:

Medium

View Solution

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

Medium

View Solution

For the first order reaction $A \rightarrow 2B$,$1 \ mole$ of reactant $A$ gives $0.2 \ moles$ of $B$ after $100 \ minutes$. The half-life of the reaction is $..... \ min$. [Use: $\ln 2 = 0.69, \ln 10 = 2.3$]

DifficultJEE MAIN 2021

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

If benzene diazonium chloride undergoes first order decomposition at $T \ K$ with a rate constant of $6.93 \times 10^{-2} \ min^{-1}$,the time for completion of $90 \%$ of the reaction (in $min$) is (nearest integer) $(\log 2 = 0.30, \log 3 = 0.477)$.

Similar Questions

The value of rate constant for a first order reaction is $2.303 \times 10^{-2} \text{ s}^{-1}$. What will be the time required to reduce the concentration to $\frac{1}{10}$th of its initial concentration (in $\text{ s}$)?

In a first order reaction $A \to B,$ if $k$ is the rate constant and the initial concentration of the reactant $A$ is $0.5 \ M,$ then the half-life is:

In a first-order reaction of the type: $A_{(g)} \to 2B_{(g)}$,the initial pressure is $P_i$ and the total pressure at time $t$ is $P_t$. The rate constant $k$ can be expressed as:

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

For the first order reaction $A \rightarrow 2B$,$1 \ mole$ of reactant $A$ gives $0.2 \ moles$ of $B$ after $100 \ minutes$. The half-life of the reaction is $..... \ min$. [Use: $\ln 2 = 0.69, \ln 10 = 2.3$]

Vedclass Test Series

Exam Paper Generator

Online Exam Module