What volume of oxygen would be required for complete combustion of 100 litres of ethane according to the following equation?
2C₂H₆ + 7O₂ $\overset{}{\to}$ 4CO₂ + 6H₂O

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Solution

Number of moles of ethane in 100 L = $\frac{Volume of ethane}{Molar volume of ethane} = \frac{100}{22.4} = 4.46 L$
According to the balanced chemical equation, two moles of ethane require seven moles of oxygen for complete combustion.
Moles of oxygen required by 4.46 moles of ethane = $\frac{7}{2} \times \frac{100}{22.4}$
Volume of oxygen required = Number of moles $\times$ Molar volume = $(\frac{7}{2} \times \frac{100}{22.4}) \times 22.4 = 350 L$ (22.4)

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2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O

What volume of oxygen would be required for the complete combustion of 100 litres of ethane? The following equation is as follows:

$2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O$

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2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O

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2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O; Δ H = - 745.6 k c a l

2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O; Δ H = - 745.6

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