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Standard XIII

Chemistry

Enthalpy of Combustion

When 5 litres...

Question

When 5 litres of a gas mixture of methane and propane is perfectly combusted at $0^{\circ} C$ and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in $k J (Δ H_{c o m b .} (C H_{4}) = 890 k J m o l^{- 1}, Δ H_{c o m b .} (C_{3} H_{8}) = 2220 k J m o l^{- 1})$ is

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Solution

The correct option is B 317
$C H_{4} + 20_{2} \to C O_{2} + 2 H_{2} O$
$C_{3} H_{8} + 50_{2} \to 3 C O_{2} + 4 H_{2} O$
$C H_{4} + C_{3} H_{8} = \frac{5}{22.4} = 0.22 m o l e s$
$O_{2} = \frac{16}{22.4} = 0.71 m o l e s$
$2 x + (0.22 - x) 5 = 0.71$
$x = 0.13$
$H e a t l i b e r a t e d = 0.13 \times 890 + 0.09 \times 2220 = 316 k J$

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Similar questions

Q. When 5 litres of a gas mixture of methane and propane is perfectly combusted at

0^{\circ} C

and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in

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When 5 litres of a gas mixture of methane and propane is perfectly combusted at $0^{\circ} C$ and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion is

$k J (Δ H_{c o m b .} (C H_{4}) = 890 k J m o l^{- 1}, Δ H_{c o m b .} (C_{3} H_{8}) = 2220 k J m o l^{- 1})$ is

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16 l i t e r

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When 5 litres of a gas mixture of methane and propane is perfectly combusted at 0∘C and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in kJ(ΔHcomb.(CH4)=890 kJ mol−1, ΔHcomb.(C3H8)=2220 kJ mol−1) is

The correct option is B 317CH4+202→CO2+2H2O C3H8+502→3CO2+4H2O CH4+C3H8=522.4=0.22 moles O2=1622.4=0.71 moles 2x+(0.22−x)5=0.71 x=0.13 Heat liberated=0.13×890+0.09×2220=316 kJ