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Standard XII

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

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

Q. When

5 l i t r e s

of a gas mixture of methane and propane is perfectly combusted at

0^{\circ} C

and

1

atmosphere,

16 l i t e r

of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in

k J

is:

(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}

Q. When

6.81 L

of a gas mixture of methane and propane is perfectly combusted at

0^{\circ} C

and

1

bar,

15.89 L

of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in

kJ is : (Δ H_{comb} (C H_{4}) = 890 {kJ mol}^{- 1}, Δ H_{comb} (C_{3} H_{8}) = 2220 {kJ mol}^{- 1})

Q. A gas mixture of

3.67

litre of ethylene and methane on complete combustion at

25^{o} C

produces

6.11

litre of

{C O}_{2}

. Find out the heat evolved on burning

1

litre of the gas mixture. The heats of combustion of ethylene and methane are

- 1423

and

- 891 k J

{m o l}^{- 1}

25^{o} C

Q. A gas mixture of

3.67

lit of ethylene & methane on complete combustion at

25^{o}

C produces

6.11 L

C O_{2}

. Find out the amount of heat evolved on burning one litre of the gas mixture. The heat for combustion of ethylene and methane are

- 1423

- 891 k J m o l^{- 1}

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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