The volume of oxygen required for complete hydrogenation of $0.25 \mathrm{dm}^{3}$ of methane at S.T.P. is

The volume of oxygen required for complete hydrogenation of $0.25 \mathrm{dm}^{3}$ of methane at S.T.P. is
  1. $22.4 \mathrm{~dm}^3$
  2. $11.2 \mathrm{~dm}^3$
  3. $5.6 \mathrm{~dm}^3$
  4. $44.8 \mathrm{~dm}^3$

Solution

$\mathrm{CH}_{4}+2 \mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}$ 1 mole of methane required $=2 \times 22.4 \mathrm{dm}^{3}$ of $\mathrm{O}_{2}$ $\therefore \quad 0.25$ mole of methane required $=2 \times 22.4 \times 0.25=11.2 \mathrm{dm}^{3}$ of $\mathrm{O}_{2}$

Asked in: MHT CET 2020 (14 Oct Shift 2)

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