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6.53 Compute the standard free energy of the reaction at 27°C for the combustion of methane CH4(g) + 2O2(g) → CO2(g) + 2H2O(1) using the following data : Species CH4 (g) 02 (g) CO2 (g) H2O(1) AfHº (k) mol! -74.8 - 1-393.5 -285.8 Sº K moll) 186 205 214 70 Also comment on the feasibility of the reaction. (Ans. -817,7 kl mol', feasible]

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Q1

The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, −890.3kJ mol−1–393.5kJ mol−1, and –285.8 kJ mol−1 respectively. Enthalpy of formation of CH4(g) will be
(i) –74.8kJ mol−1
(ii) –52.27kJ mol−1
(iii) +74.8kJ mol−1
(iv) +52.26kJmol−1

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Q2

Standard enthalpy of combustion of CH4 is −890 kJ mol−1 and standard enthalpy of vaporisation of water is 40.5 kJ mol−1. Calculate the enthalpy change for the reaction :
CH4(g)+2O2(g)→CO2(g)+2H2O(g)


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Q3
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Q4
The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are - 890.3 kl/mol, - 393 kj/mol and 285.8 kj/mol respectively. Enthalpy of formation of $$CH_{4(g)}$$ will be
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Q5
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