(C) The decomposition reaction is: $2NH_{3(g)} \rightarrow N_{2(g)} + 3H_{2(g)}$For a zero-order reaction,the rate of reaction is equal to the rate co

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(C) The decomposition reaction is: $2NH_{3(g)} \rightarrow N_{2(g)} + 3H_{2(g)}$For a zero-order reaction,the rate of reaction is equal to the rate constant $k$.$\text{Rate} = k = 2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$.The rate of reaction is expressed as: $\text{Rate} = -\frac{1}{2} \frac{d[NH_3]}{dt} = \frac{d[N_2]}{dt} = \frac{1}{3} \frac{d[H_2]}{dt}$.Therefore,the rate of production of $N_2$ is equal to the rate of the reaction.$\frac{d[N_2]}{dt} = \text{Rate} = 2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Zero order reaction

Easy

The decomposition of $NH_3$ on a platinum surface is a zero-order reaction. What is the rate of production of $N_2$ if $k = 2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$?

GSEB 2020 All GSEB

A
$7.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$
B
$8.3 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$
C
$2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$
D
$5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$

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Chemical Kinetics

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Zero order reaction

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The time for the half-life period of a certain reaction $A \rightarrow \text{Products}$ is $1 \ hr$. When the initial concentration of the reactant $A$ is $2.0 \ mol \ L^{-1}$,how many hours does it take for its concentration to decrease from $0.50 \ mol \ L^{-1}$ to $0.25 \ mol \ L^{-1}$ if it is a zero-order reaction?

DifficultAIEEE 2010

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$A \rightarrow B$
The above reaction is of zero order. The half-life of this reaction is $50 \ min$. The time taken for the concentration of $A$ to reduce to one-fourth of its initial value is $........... \ min$ (Nearest integer).

MediumJEE MAIN 2023

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Provide the graphs for a zero-order reaction and explain the information obtained from them.

Difficult

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Which of the following graphs represents a zero order reaction?
($a = $ initial concentration of reactant,
$x = $ concentration of reactant consumed,
$t = $ time)

EasyTS EAMCET 2018

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For the reaction $A \longrightarrow 3 B$,the rate is given by $rate = k[A]^0$. Based on the data provided in the table,what is the concentration of the product $B$ (in $mol \ L^{-1}$) after $20 \ s$?
Time $(s)$ Concentration of the reactant $(mol \ L^{-1})$
$0$ $0.1$
$15$ $0.05$
$20$ $0.1 - x$

DifficultAP EAMCET 2017

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Time $(s)$	Concentration of the reactant $(mol \ L^{-1})$
$0$	$0.1$
$15$	$0.05$
$20$	$0.1 - x$

The decomposition of $NH_3$ on a platinum surface is a zero-order reaction. What is the rate of production of $N_2$ if $k = 2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$?

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$A \rightarrow B$The above reaction is of zero order. The half-life of this reaction is $50 \ min$. The time taken for the concentration of $A$ to reduce to one-fourth of its initial value is $........... \ min$ (Nearest integer).

Provide the graphs for a zero-order reaction and explain the information obtained from them.

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$A \rightarrow B$
The above reaction is of zero order. The half-life of this reaction is $50 \ min$. The time taken for the concentration of $A$ to reduce to one-fourth of its initial value is $........... \ min$ (Nearest integer).

Which of the following graphs represents a zero order reaction?
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$x = $ concentration of reactant consumed,
$t = $ time)

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$0$ $0.1$
$15$ $0.05$
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