(C) The reaction is $2H_{2(g)} + O_{2(g)} \to 2H_2O$. $(i)$ At room temperature,$H_2O$ exists as a liquid and its volume is negligible. $H_2$ is the l

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$(i) \, 25 \, c.c., \, (ii) \, 75 \, c.c.$

(C) The reaction is $2H_{2(g)} + O_{2(g)} \to 2H_2O$. $(i)$ At room temperature,$H_2O$ exists as a liquid and its volume is negligible. $H_2$ is the limiting reagent ($50 \, mL$ of $H_2$ reacts with $25 \, mL$ of $O_2$). Remaining $O_2 = 50 - 25 = 25 \, mL$. Total volume of gas = $25 \, c.c.$ $(ii)$ At $110 \, ^oC$,$H_2O$ exists as a gas (steam). $2H_{2(g)} + O_{2(g)} \to 2H_2O_{(g)}$. Remaining $O_2 = 25 \, mL$,produced $H_2O_{(g)} = 50 \, mL$. Total volume of gas = $25 + 50 = 75 \, c.c.$

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

Difficult

An electric discharge is passed through a mixture containing $50 \, c.c.$ of $O_2$ and $50 \, c.c.$ of $H_2$. The volume of the gases formed $(i)$ at room temperature and $(ii)$ at $110 \, ^oC$ will be

A
$(i) \, 25 \, c.c., \, (ii) \, 50 \, c.c.$
B
$(i) \, 50 \, c.c., \, (ii) \, 75 \, c.c.$
C
$(i) \, 25 \, c.c., \, (ii) \, 75 \, c.c.$
D
$(i) \, 75 \, c.c., \, (ii) \, 75 \, c.c.$

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Some Basic Concepts of Chemistry

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Chemical equation and limiting reagent

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DifficultJEE MAIN 2025

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An electric discharge is passed through a mixture containing $50 \, c.c.$ of $O_2$ and $50 \, c.c.$ of $H_2$. The volume of the gases formed $(i)$ at room temperature and $(ii)$ at $110 \, ^oC$ will be

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One mole of calcium phosphide on reaction with excess water gives

Calculate the amount of carbon dioxide produced when:$(i)$ $1$ mole of carbon is burnt in air.$(ii)$ $1$ mole of carbon is burnt in $16 \ g$ of dioxygen.$(iii)$ $2$ moles of carbon are burnt in $16 \ g$ of dioxygen.

$250 \ mL$ of $0.5 \ M \ NaOH$ was added to $500 \ mL$ of $1 \ M \ HCl$. The number of unreacted $HCl$ molecules in the solution after complete reaction is $...... \times 10^{21}$. (Nearest integer) $(N_{A} = 6.022 \times 10^{23})$

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When $81.0 \ g$ of aluminium is allowed to react with $128.0 \ g$ of oxygen gas,the mass of aluminium oxide produced in grams is $..........$ $(Nearest \ integer)$. Given: Molar mass of $Al$ is $27.0 \ g \ mol^{-1}$,Molar mass of $O$ is $16.0 \ g \ mol^{-1}$.

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Calculate the amount of carbon dioxide produced when:
$(i)$ $1$ mole of carbon is burnt in air.
$(ii)$ $1$ mole of carbon is burnt in $16 \ g$ of dioxygen.
$(iii)$ $2$ moles of carbon are burnt in $16 \ g$ of dioxygen.