Chapter 4 Chemical equilibria, entropy and Gibbs function X$4.1 The standard equilibrium constant X 4.2 The application of the standard equilibrium constant x 4.3 The shift of a chemical equilibrium x 4.4 Spontaneous reactions and entropy x§4.5 Gibbs function
Chapter 4 Chemical equilibria, entropy and Gibbs function §4.3 The shift of a chemical equilibrium §4.2 The application of the standard equilibrium constant §4.1 The standard equilibrium constant §4.5 Gibbs function §4.4 Spontaneous reactions and entropy
4.1 The standard equilibrium constant 4.1.1 The basic features of a chemical equilibrium 4.1.2 The standard equilibrium constant expression 4.1.3 Experimental measurement of the standard equilibrium constant
§4.1 The standard equilibrium constant 4.1.3 Experimental measurement of the standard equilibrium constant 4.1.2 The standard equilibrium constant expression 4.1.1 The basic features of a chemical equilibrium
4.1.1 The basic features of a chemical equilibrium Most reactions are reversible,an example is emo1-EH,(g)+1,(g)=2Hg×10ux10 mol.L.s-1 t/s 0 0.0100 0.0100 0 7.60 0 2000 0.003970.003970.0121 1.20 2.04 4850 0.002130.002130.0157 0.3453.43 85000.002130.002130.01570.345 3.43
4.1.1 The basic features of a chemical equilibrium 0 0.0100 0.0100 0 7.60 0 2000 0.00397 0.00397 0.0121 1.20 2.04 4850 0.00213 0.00213 0.0157 0.345 3.43 Most reactions are reversible, an example is t/s 1 / mol L− c ⋅ 6 υ + ×10 7 υ − ×10 1 1 mol L s − − ⋅ ⋅ H (g) I (g) 2HI(g) 2 + 2 8500 0.00213 0.00213 0.0157 0.345 3.43
Initially,concentrations of H,and I,are large,only the forward reaction occurs;As time passes,the concentrations of H,and I, decrease and in result the forward reaction slows down.The concentrations of HI increase and in result the reverse reaction speeds up. The reaction mixture is at equilibrium until the forward and reverse reactions go at the same rate
Initially, concentrations of H2 and I 2 are large, only the forward reaction occurs; As time passes, the concentrations of H2 and I2 decrease and in result the forward reaction slows down. The concentrations of HI increase and in result the reverse reaction speeds up. The reaction mixture is at equilibrium until the forward and reverse reactions go at the same rate
正 H H2,l t/s t/s H,(g)+I,(g)=2HI(g) Conc HI 2HI(g）≠H2(g）+I2(g) H,2 t/s
υ 正 υ 逆 υ 正 =υ 逆 H (g) I (g) 2HI(g) 2 + 2 2HI(g) H2 (g) + I2 (g) Conc