(C) The balanced chemical equation is $4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_{2}O_{(g)}$.According to the stoichiometry,$4 \ moles$ of $NH_{3}$ re

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All the oxygen will be consumed

(C) The balanced chemical equation is $4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_{2}O_{(g)}$.According to the stoichiometry,$4 \ moles$ of $NH_{3}$ require $5 \ moles$ of $O_{2}$.For $1 \ mole$ of $NH_{3}$,the required amount of $O_{2}$ is $\frac{5}{4} = 1.25 \ moles$.Since only $1 \ mole$ of $O_{2}$ is available,$O_{2}$ acts as the limiting reagent.Therefore,all the $O_{2}$ will be consumed in the reaction.

Class 11 Chemistry Some Basic Concepts of Chemistry Chemical equation and limiting reagent

Difficult

In the reaction,$4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_{2}O_{(g)}$,when $1 \ mole$ of ammonia and $1 \ mole$ of $O_{2}$ are made to react to completion:

A
$1.0 \ mole$ of $H_{2}O$ is produced
B
$1.0 \ mole$ of $NO$ will be produced
C
All the oxygen will be consumed
D
All the ammonia will be consumed

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Some Basic Concepts of Chemistry

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Chemical equation and limiting reagent

On reaction of $38.1 \ g$ iodine and $28.4 \ g$ chlorine,a mixture of $ICl$ and $ICl_3$ is obtained. What will be the total number of moles after the reaction?

Easy

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$8 \ L$ of $H_2$ and $6 \ L$ of $Cl_2$ react to the maximum extent. Find the final volume of the reaction mixture in $L$. Assume $P$ and $T$ remain constant throughout the process.

Easy

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If the heat of combustion of methane is $-100 \ kJ/mol$,then calculate the heat evolved when $32 \ g$ of methane reacts with $32 \ g$ of oxygen. (in $kJ$)

Medium

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When $22.4 \ L$ of $H_{2(g)}$ is mixed with $11.2 \ L$ of $Cl_{2(g)}$,each at $S.T.P.$,the moles of $HCl_{(g)}$ formed is equal to

MediumNEET 2014

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In the Haber process,$30 \ L$ of dihydrogen and $30 \ L$ of dinitrogen were taken for the reaction,which yielded only $50\%$ of the expected product. What will be the composition of the gaseous mixture under the aforesaid condition in the end?

DifficultAIPMT 2003

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In the reaction,$4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_{2}O_{(g)}$,when $1 \ mole$ of ammonia and $1 \ mole$ of $O_{2}$ are made to react to completion:

Similar Questions

On reaction of $38.1 \ g$ iodine and $28.4 \ g$ chlorine,a mixture of $ICl$ and $ICl_3$ is obtained. What will be the total number of moles after the reaction?

$8 \ L$ of $H_2$ and $6 \ L$ of $Cl_2$ react to the maximum extent. Find the final volume of the reaction mixture in $L$. Assume $P$ and $T$ remain constant throughout the process.

If the heat of combustion of methane is $-100 \ kJ/mol$,then calculate the heat evolved when $32 \ g$ of methane reacts with $32 \ g$ of oxygen. (in $kJ$)

When $22.4 \ L$ of $H_{2(g)}$ is mixed with $11.2 \ L$ of $Cl_{2(g)}$,each at $S.T.P.$,the moles of $HCl_{(g)}$ formed is equal to

In the Haber process,$30 \ L$ of dihydrogen and $30 \ L$ of dinitrogen were taken for the reaction,which yielded only $50\%$ of the expected product. What will be the composition of the gaseous mixture under the aforesaid condition in the end?

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