9. Calculate ΔG0 at 820C for reactions in which
(a) ΔH0= 293 kJ; ΔS0 = -695 J/K
(b) ΔH0= -1137 kJ; ΔS0= 0.496 kJ/K
G^{0} = H^{0} -TS^{0}
We use this formula for both the below questions
T = 82^{0}C = (82+273)K = 355K
(a) H^{0} = 293kJ = 293000J [Since 1kJ = 1000J]
G^{0} = H^{0} -TS^{0}
G^{0} = 293000J - (355K x -695J/K)
G^{0} = 293000J + 246725J = 539725J
(b) H^{0} = -1137kJ
G^{0} = H^{0} -TS^{0}
G^{0} = -1137kJ - (355K x 0.496kJ/K)
G^{0} = -1137kJ - 176.08kJ
G^{0} = 1313.08kJ = 131080J
9. Calculate ΔG0 at 820C for reactions in which (a) ΔH0= 293 kJ; ΔS0 = -695...
At what temperatures are the following reactions spontaneous? a) ΔH0 = -35 kJ/mol; ΔS0 = -75 j/Kˑmol b) ΔH0 = -35 kJ/mol; ΔS0 = +75 j/Kˑmol c) ΔH0 = +35 kJ/mol; ΔS0 = -75 j/Kˑmol d) ΔH0 = +35 kJ/mol; ΔS0 = +75 j/Kˑmol
(2 pts) Calculate the equilibrium pressure of CO2 in the system at 3000C. ΔH0 = 88.3 kJ and ΔS0 = 151.3 J/K. R = 8.314 J/mol K PbCO3(s) ® PbO(s) + CO2(g) ΔH0f(kJ/mol) -699.1 -217.3 -393.5 S0(J/mol K) 131 68.7 213.6
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Calculate the ΔH0 for the following reaction: NH4Cl(s) → NH3(g) + HCl(g) Given the following standard enthalpies of formation ΔHf0 (298 K, 1 atm) NH3(g) -46.2 kJ mol-1 ; HCl(g) -92.3 kJ mol-1 ; NH4Cl(s) -315.0 kJ mol-1
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