Consider the reaction. CH4(g)+2 O2(g) CO2(g)+2 H2 O() Delta Ho=-606.9 kJ mol-1 Assuming ideal behaviour… · ABC26PH0643

Subject: Physical Chemistry · Chapter: Chemical Equilibrium · Topic: Chemical Equilibrium – General · Exam: JAM 2001-2022 · Marks: 2 · Difficulty: Hard

Consider the reaction.
\[ \mathrm{CH}_{4}(\mathrm{g})+2 \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\ell) \quad \Delta \mathrm{H}^{\mathrm{o}}=-606.9 \mathrm{kJ} \mathrm{mol}^{-1} \]
Assuming ideal behaviour, calculate $\Delta \mathrm{U}^{\circ}$ when 1 mol of $\mathrm{CH}_{4}$ is completely oxidized at STP.
Answer
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