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1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)

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Presentation on theme: "1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)"— Presentation transcript:

1 1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)
Enthalpy of Reaction: kJ     (exothermic) [2ΔHf(Fe (s)) + 3ΔHf(CO2 (g))] - [1ΔHf(Fe2O3 (s)) + 3ΔHf(CO (g))] [2(0) + 3( )] - [1( ) + 3( )] = kJ

2 1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)
Entropy Change: 14.50 J/K     (increase in entropy) [2S°(Fe (s)) + 3S°(CO2 (g))] - [1S°(Fe2O3 (s)) + 3S°(CO (g))] [2(27.28) + 3(213.68)] - [1(87.4) + 3(197.9)] = J/K

3 1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)
Free Energy of Reaction (at K): From ΔGfo values: kJ     (spontaneous) [2ΔGf(Fe (s)) + 3ΔGf(CO2 (g))] - [1ΔGf(Fe2O3 (s)) + 3ΔGf(CO (g))] [2(0) + 3( )] - [1( ) + 3( )] = kJ

4 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)
Enthalpy of Reaction: kJ     (exothermic) [4ΔHf(NO (g)) + 6ΔHf(H2O (g))] - [4ΔHf(NH3 (g)) + 5ΔHf(O2 (g))] [4(90.25) + 6( )] - [4(-46.11) + 5(0)] = kJ

5 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)
Entropy Change: J/K     (increase in entropy) [4S°(NO (g)) + 6S°(H2O (g))] - [4S°(NH3 (g)) + 5S°(O2 (g))] [4(210.65) + 6(188.72)] - [4(192.34) + 5(205.03)] = J/K

6 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)
Free Energy of Reaction (at K): From ΔGfo values: kJ     (spontaneous) [4ΔGf(NO (g)) + 6ΔGf(H2O (g))] - [4ΔGf(NH3 (g)) + 5ΔGf(O2 (g))] [4(86.57) + 6( )] - [4(-16.48) + 5(0)] = kJ

7 SO2 (g) + 2 Cl2 (g) → SOCl2 (g) + Cl2O (g)
Enthalpy of Reaction: kJ     (endothermic) [1ΔHf(SOCl2 (g)) + 1ΔHf(Cl2O (g))] - [1ΔHf(SO2 (g)) + 2ΔHf(Cl2 (g))] [1( ) + 1(80.33)] - [1( ) + 2(0)] = kJ

8 SO2 (g) + 2 Cl2 (g) → SOCl2 (g) + Cl2O (g)
Entropy Change: J/K     (decrease in entropy) [1ΔSf(SOCl2 (g)) + 1ΔSf(Cl2O (g))] - [1ΔSf(SO2 (g)) + 2ΔSf(Cl2 (g))] [1(309.66) + 1(267.86)] - [1(248.11) + 2(222.97)] = J/K

9 SO2 (g) + 2 Cl2 (g) → SOCl2 (g) + Cl2O (g)
Free Energy of Reaction (at K): From ΔGfo values: kJ     (nonspontaneous) [1ΔGf(SOCl2 (g)) + 1ΔGf(Cl2O (g))] - [1ΔGf(SO2 (g)) + 2ΔGf(Cl2 (g))] [1( ) + 1(97.49)] - [1( ) + 2(0)] = kJ

10 2 MgO (s) + 2 SO2 (g) + O2 (g) → 2 MgSO4 (s)
Enthalpy of Reaction: kJ     (exothermic) [2ΔHf(MgSO4 (s))] - [2ΔHf(MgO (s)) + 2ΔHf(SO2 (g)) + 1ΔHf(O2 (g))] [2( )] - [2( ) + 2( ) + 1(0)] = kJ

11 2 MgO (s) + 2 SO2 (g) + O2 (g) → 2 MgSO4 (s)
Entropy Change: J/K     (decrease in entropy) [2ΔSf(MgSO4 (s))] - [2ΔSf(MgO (s)) + 2ΔSf(SO2 (g)) + 1ΔSf(O2 (g))] [2(91.63)] - [2(26.94) + 2(248.11) + 1(205.03)] = J/K

12 2 MgO (s) + 2 SO2 (g) + O2 (g) → 2 MgSO4 (s)
Free Energy of Reaction (at K): From ΔGfo values: kJ     (spontaneous) [2ΔGf(MgSO4 (s))] - [2ΔGf(MgO (s)) + 2ΔGf(SO2 (g)) + 1ΔGf(O2 (g))] [2( )] - [2( ) + 2( ) + 1(0)] = kJ

13 6 UF4 (s) + 4 Br2 (ℓ) + 9 O2 (g) → 6 UO3 (s) + 8 BrF3 (ℓ)
Enthalpy of Reaction: 1133 kJ     (endothermic) [6DHf(UO3 (s)) + 8DHf(BrF3 (ℓ))] - [6DHf(UF4 (s)) + 4DHf(Br2 (ℓ)) + 9DHf(O2 (g))] [6( ) + 8( )] - [6( ) + 4(0) + 9(0)] = 1133 kJ

14 6 UF4 (s) + 4 Br2 (ℓ) + 9 O2 (g) → 6 UO3 (s) + 8 BrF3 (ℓ)
Entropy Change: -1, J/K     (decrease in entropy) [6ΔSf(UO3 (s)) + 8ΔSf(BrF3 (ℓ))] - [6ΔSf(UF4 (s)) + 4ΔSf(Br2 (ℓ)) + 9ΔSf(O2 (g))] [6(98.62) + 8(178.24)] - [6(151.04) + 4(152.23) + 9(205.03)] = J/K

15 6 UF4 (s) + 4 Br2 (ℓ) + 9 O2 (g) → 6 UO3 (s) + 8 BrF3 (ℓ)
Free Energy of Reaction (at K): From ΔGfo values: 1, kJ     (nonspontaneous) [6ΔGf(UO3 (s)) + 8ΔGf(BrF3 (ℓ))] - [6ΔGf(UF4 (s)) + 4ΔGf(Br2 (ℓ)) + 9ΔGf(O2 (g))] [6( ) + 8( )] - [6( ) + 4(0) + 9(0)] = kJ


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