Question

The lattice enthalpy (formation of ionic solid from ions in the gas phase) for AgCl(s) is...

The lattice enthalpy (formation of ionic solid from ions in the gas phase) for AgCl(s) is -916 kJ/mol and the hydration enthalpy (dissolution of gaseous ions into water) is - 850 kJ/mol. How much heat (in Joules) is involved in forming 1L of saturated AgCl solution (1.8 × 10-4 g / 100 mL water) by dissolving AgCl(s)? Assume solution volume does not change much upon dissolution. The equations are given below. Ag+ (g) + Cl− (g) Æ AgCl(s) Ag+ (g) + Cl- (g) Æ Ag+ (aq) + Cl- (aq)

Homework Answers

Answer #1

1. Ag+ (g) + Cl− (g) ===> AgCl(s)    dH = -916kJ/mol

2. Ag+ (g) + Cl- (g) ===> Ag+ (aq) + Cl- (aq)      dH = -850kJ/mol

3. Ag+ (aq) + Cl- (aq) ===> Ag+ (g) + Cl- (g)    dH = 850kJ/mol

So, 1 + 3 equations

gives Ag+ (aq) + Cl- (aq) ===> AgCl(s) dH = -66kJ/mol

100mL water has mass AgCl = 1.8 x 10^-4grams

1L water has mass AgCl = 1.8 x 10^-3 grams

moles = mass/molar mass = 1.8 x 10^-3 grams/ 143.32g/mol = 1.2559 x10^-5moles

So, heat released in 1 mol = 66kJ = 66000J

heat released in 1.2559 x10^-5moles = 1.2559 x10^-5moles x 66000 = 0.83J

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