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Question

A gas mixture 3.67 L in volume contains C2H4 and CH4 is proportion of 2:1 by moles and is at 25C and 1 atm. If the ΔHC (C2H4) and ΔHC (CH4) are 1400 and 900 kJ/mol find heat evolved on burning this mixture


A

20.91 kJ

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B

50.88 kJ

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C

185 kJ

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D

160 kJ

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Solution

The correct option is C

185 kJ


Volume of C2H4 = 3.67 × 23 = 2.45Lit

Volume of CH4 = 1.22 Lit

Mole of C2H5 = PV = nRTn = PVRT

= 1 × 2.450.082 × 298 = n = 0.1mole

Mole of CH4 = nCH4 = 1 × 1.220.082 × 298 = 0.05mole

Energy released due to combusting 1 mole C2H4 = 1400 KJ

Energy released due to combusting 1 mole C2H4 = 1400 × 0.1 = 140 kJ

Similar energy released in combusting 0.05 mole

CH4 = 900 × 0.05 = 45

So that heat realized = 140 + 45 = 185 kJ/mole


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