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1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g) Enthalpy of Reaction:-24.66 kJ (exothermic) [2ΔH f (Fe (s)) + 3ΔH f (CO2 (g))] - [1ΔH f (Fe2O3 (s)) + 3ΔH.

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Presentation on theme: "1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g) Enthalpy of Reaction:-24.66 kJ (exothermic) [2ΔH f (Fe (s)) + 3ΔH f (CO2 (g))] - [1ΔH f (Fe2O3 (s)) + 3ΔH."— Presentation transcript:

1 1 Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g) Enthalpy of Reaction: kJ (exothermic) [2ΔH f (Fe (s)) + 3ΔH f (CO2 (g))] - [1ΔH f (Fe2O3 (s)) + 3ΔH f (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 ΔG f o values: kJ (spontaneous) [2ΔG f (Fe (s)) + 3ΔG f (CO2 (g))] - [1ΔG f (Fe2O3 (s)) + 3ΔG f (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) [4ΔH f (NO (g)) + 6ΔH f (H2O (g))] - [4ΔH f (NH3 (g)) + 5ΔH f (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 ΔG f o values: kJ (spontaneous) [4ΔG f (NO (g)) + 6ΔG f (H2O (g))] - [4ΔG f (NH3 (g)) + 5ΔG f (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) [1ΔH f (SOCl2 (g)) + 1ΔH f (Cl2O (g))] - [1ΔH f (SO2 (g)) + 2ΔH f (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) [1ΔS f (SOCl2 (g)) + 1ΔS f (Cl2O (g))] - [1ΔS f (SO2 (g)) + 2ΔS f (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 ΔG f o values: kJ (nonspontaneous) [1ΔG f (SOCl2 (g)) + 1ΔG f (Cl2O (g))] - [1ΔG f (SO2 (g)) + 2ΔG f (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) [2ΔH f (MgSO4 (s))] - [2ΔH f (MgO (s)) + 2ΔH f (SO2 (g)) + 1ΔH f (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) [2ΔS f (MgSO4 (s))] - [2ΔS f (MgO (s)) + 2ΔS f (SO2 (g)) + 1ΔS f (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 ΔG f o values: kJ (spontaneous) [2ΔG f (MgSO4 (s))] - [2ΔG f (MgO (s)) + 2ΔG f (SO2 (g)) + 1ΔG f (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) [6  Hf(UO3 (s)) + 8  Hf(BrF3 ( ℓ ))] - [6  Hf(UF4 (s)) + 4  Hf(Br2 ( ℓ )) + 9  Hf(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) [6ΔS f (UO3 (s)) + 8ΔS f (BrF3 (ℓ))] - [6ΔS f (UF4 (s)) + 4ΔS f (Br2 (ℓ)) + 9ΔS f (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 ΔG f o values: 1, kJ (nonspontaneous) [6ΔG f (UO3 (s)) + 8ΔG f (BrF3 (ℓ))] - [6ΔG f (UF4 (s)) + 4ΔG f (Br2 (ℓ)) + 9ΔG f (O2 (g))] [6( ) + 8( )] - [6( ) + 4(0) + 9(0)] = kJ


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