Mass of methane required to produce 22\, g of CO 2 after complete combustion is \ \ \ \ g. (Given molar mass in g\,mol -1 : C =12.0 , H =1.0 , O =16.0 )

Chemistry · Some Basic Concepts of Chemistry (Mole Concept) + Stoichiometry

JEE Main 2024 — 27 January, Shift 1 — Question 75

Mass of methane required to produce $22\,\mathrm{g}$ of $\mathrm{CO_2}$ after complete combustion is $\_\_\_\_$ g.

(Given molar mass in $\mathrm{g\,mol^{-1}}$ : $\mathrm{C}=12.0$ , $\mathrm{H}=1.0$ , $\mathrm{O}=16.0$ )

Numerical answer — enter this value.

Complete combustion of methane:

\mathrm{CH_4 + 2O_2 \xrightarrow{\Delta} CO_2 + 2H_2O}

From the balanced equation, we have

1\,\mathrm{mol\ CH_4} \rightarrow 1\,\mathrm{mol\ CO_2}

Moles of $\mathrm{CO_2}$ formed $= \frac{22}{44} = 0.5\,\mathrm{mol}$

Hence, moles of $\mathrm{CH_4}$ required $= 0.5\,\mathrm{mol}$

Molar mass of $\mathrm{CH_4}$ $= 12 + 4(1) = 16\,\mathrm{g\,mol^{-1}}$

Mass of $\mathrm{CH_4}$ required $= 0.5 \times 16 = 8\,\mathrm{g}$

Answer key and solution verified before publishing.

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