What volume of oxygen is required to burn completely a mixture of $22.4 d m^{3}$ of methane and $11.2 d m^{3}$ of hydrogen into carbon dioxide and steam?
$C H_{4} + 20_{2} \to C O_{2} + 2 H_{2} O 2 H_{2} + O_{2} \to 2 H_{2} O$

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Solution

$C H_{4} + 2 O_{2} \to C O_{2} + 2 H_{2} O 2 H_{2} + O_{2} \to 2 H_{2} O$
1 vol of methane requires 2 vol of oxygen.
$22.4 d m^{3}$ of methane requires $2 \times 22.4 d m^{3}$ oxygen.
$22.4 d m^{3}$ of methane requires $44.8 d m^{3}$ oxygen.
2 vol of hydrogen requires 1 vol of oxygen.
$11.2 d m^{3}$ of hydrogen requires $5.6 d m^{3}$ of oxygen.
Total oxygen required = $(44.8 + 5.6) d m^{3}$ = $50.4 d m^{3}$

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What volume of oxygen is required to burn completely a mixture of 22.4 dm³ of methane and 11.2 dm³ of hydrogen into carbon dioxide and steam?

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CH₄ + 2O₂ → CO₂ +2H₂O

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What volume of oxygen is required to burn completely a mixture of 22.4dm3 of methane and 11.2dm3 of hydrogen into carbon dioxide and steam? CH4+202→CO2+2H2O2H2+O2→2H2O

What volume of oxygen is required to burn completely a mixture of $22.4 d m^{3}$ of methane and $11.2 d m^{3}$ of hydrogen into carbon dioxide and steam?
$C H_{4} + 20_{2} \to C O_{2} + 2 H_{2} O 2 H_{2} + O_{2} \to 2 H_{2} O$