Calculate the standard free energy change for the formation of methane at `300K`:
`C("graphite") +2H_(2) (g) rarr CH_(4)(g)`
The following data are given:
`Delta_(f)H^(Theta) (kJ mol^(-1)): CH_(4)(g) =- 74.81`
`Delta_(f)S^(Theta)(kJ mol^(-1)): C("graphite") = 5.70, H_(2)(g) = 130.7 CH_(4)(g) = 186.3`

Calculate the standard free energy change for the formation of methane at 300K : C("graphite") +2H_(2) (g) rarr CH_(4)(g) The following data are given: Delta_(f)H^(Theta) (kJ mol^(-1)): CH_(4)(g) =- 74.81 Delta_(f)S^(Theta)(JK^(-1) mol^(-1)): C("graphite") = 5.70, H_(2)(g) = 130.7 CH_(4)(g) = 186.3

Calculate the standard free energy change for the formation of methane at 300K : C("graphite") +2H_(2) (g) rarr CH_(4)(g) The following data are given: Delta_(f)H^(Theta) (kJ mol^(-1)): CH_(4)(g) =- 74.81 Delta_(f)S^(Theta)(JK^-1 mol^(-1)): C("graphite") = 5.70, H_(2)(g) = 130.7, CH_(4)(g) = 186.3

Calculate the standard molar entropy change for the formation of gaseous propane (C_(3)H_(8)) at 293K . 3C("graphite") +4H_(2)(g) rarr C_(3)H_(8)(g) Standard molar entropies S_(m)^(Theta) (JK^(-1)mol^(-1)) are: C("graphite") = 5.7, H_(2)(g) = 130.7,C_(3)H_(5)(g) = 270.2

Calculate the standard molar entropy change for the formation of gaseous propane (C_(3)H_(8)) at 293K . 3C("graphite") +4H_(2)(g) rarr C_(3)H_(8)(g) Standard molar entropies S_(m)^(Theta) (JK^(-1)mol^(-1)) are: C("graphite") = 5.7, H_(2)(g) = 130.7,C_(3)H_(5)(g) = 270.2

Calculate the standard Gibbs energy change for the formation of propane at 298 K: 3C("graphite") + 4H_(2)(g) to C_(3)H_(8)(g) Delta_(f)H^(@) for propane, C_(3)H_(8)(g) = -103.8 kJ mol^(-1) . Given : S_(m)^(0)[C_(3)H_(8)(g)] = 270.2 J K^(-1) "mol"^(-1) S_(m)^(@)("graphite") = 5.70 J K^(-1) "mol"^(-1) and S_(m)^(0)[H_(2)(g)] = 130.7 J K^(-1) "mol"^(-1) .

Calculate the standard Gibbs free energy change from the free energies of formation data for the following reaction: C_(6)H_(6)(l) +(15)/(2)O_(2)(g) rarr 6CO_(2)(g) +3H_(2)O(g) Given that Delta_(f)G^(Theta) =[C_(6)H_(6)(l)] = 172.8 kJ mol^(-1) Delta_(f)G^(Theta)[CO_(2)(g)] =- 394.4 kJ mol^(-1) Delta_(f)G^(Theta) [H_(2)O(g)] =- 228.6 kJ mol^(-1)

Calculate the standard Gibbs free energy change from the free energies of formation data for the following reaction: C_(6)H_(6)(l) +(15)/(2)O_(2)(g) rarr 6CO_(2)(g) +3H_(2)O(g) Given that Delta_(f)G^(Theta) =[C_(6)H_(6)(l)] = 172.8 kJ mol^(-1) Delta_(f)G^(Theta)[CO_(2)(g)] =- 394.4 kJ mol^(-1) Delta_(f)G^(Theta) [H_(2)O(g)] =- 228.6 kJ mol^(-1)