Question

What is the A,G for the following reaction (in kJ molt) at 298 K? CH4 (g) + 2 O2(g) = CO2 (g) + 2 H20 (g) The conditions for this reaction are: PCH4 = 1.51 bar Po2 = 1.33 bar Pco2 = 0.21 bar PH2O = 0.62 bar You will also need to use Appendix Il in your textbook (containing standard Gibbs energies of formation).

Answer 1

Where, Solutions The following reaction is CHA (9) + 202 () = CO2(g) + 2 H2O (8) The relationship between the free energy of reaction at any moment in time (AG) and the standard -state free energy of reaction (aco) is deseribe by the following equation. 49 = 46° +RT in R = ideal gas corytant in unit of J/mol-k T Temperature in Kelvin In represents a logarithm to the base e 8 >> Reaction quotient at that moment in time. AGS (kJ/mol) of H2O(g) ² -228.61 kJ/mol Aas (25/mol) of 02 (9) 1 0 Auf (kJ/mol) of CO2 (8) > -394.39 kJ/mol AG (kJ/mol) of Cha (g) ² - 50.8 kJ/mol "Change in standard Gibbs free energy of the reaction Cocos = Apaº) is – Argºs AGE (COL) + 2 44% C8O) – ANG (CMa) -auf (o) = [- 394.39+ 2 (-228.61) -(-50.8 ) - 0] kJ/mol = -800.81 kJ/mol. Reaction g= quotient at 298k, bcozig] Puola Penula) Polo

→ Q = 0.21 bar x (0.62 bam)? Pertan = 1.51 bar 1.51bar x (1.33 bar)? | P₂ = 1:33 bar 0.080724 (bay Pro₂ = 0.21 bar Po = 0.62 bar 2. 671039 (barys = 0.03022 At 298k, Ara of the reaction, Ara= ArGo + RT in = [- 80081x10° + 8.314x298 In (0.03022) 75ml = [ - 800810 + (-8669.6 5)] J/mol = – 809 47 9.647 J/mol = - 809.479647 kJ/mol Hence ArG of the following reaction is -809, 479647 kJ/mol.