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प्रश्न
A gas mixture of 3.67 lit of ethylene and methane on complete combustion at 25°C and at 1 atm pressure produce 6.11 lit of carbon dioxide. Find out the amount of heat evolved in kJ, during this combustion. (ΔHC(CH4)) = − 890 kJ mol−1 and (ΔHC(C2H4)) = − 1423 kJ mol−1
उत्तर
Given, ΔHC(CH4) = − 890 kJ mol−1
ΔHC(C2H4) = − 1423 kJ mol−1
Let the mixture contain x lit of CH4 and (3.67 − x) lit of ethylene.
\[\ce{\underset{\text{x lit}}{CH4} + 2O2 -> \underset{\text{x lit}}{CO2} + 2H2O}\]
\[\ce{\underset{\text{(3.67 − x) lit}}{C2H4 + 3O2} -> \underset{\text{2 (3.67 − x) lit}}{2CO2 + 2H2O}}\]
Volume of Carbon dioxide formed = x + 2 (3.67 − x) = 6.11 lit
x + 7.34 − 2x = 6.11
7.34 − x = 6.11
x = 1.23 lit
Given mixture contains 1.23 lit of methane and 2.44 lit of ethylene, hence
ΔHC = `[(Δ"H"_"C" ("CH"_4))/(22.4 "lit") xx ("x") "lit"] + [(Δ"H"_"C" ("C"_2"H"_4))/(22.4 "lit") xx (3.67 - "x") "lit"]`
ΔHC = `[(-890 "kJ mol"^-1)/(22.4 "lit") xx 1.23 "lit"] + [(-1423)/(22.4 "lit") xx (3.67 - 1.23) "lit"]`
ΔHC = [−48.87 kJ mol−1] + [−155kJ mol−1]
ΔHC = −203.87 kJ mol−1
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