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1) Derive the Clausius-Clapeyron equation for an ideal gas and ideal liquid: Liquid (Phase A) ↔...

1) Derive the Clausius-Clapeyron equation for an ideal gas and ideal liquid: Liquid (Phase A) ↔ Gas (Phase B) Begin with the equation relating chemical potential of the two phases (?A , ?B ), assuming these phases are at equilibrium (as they are assumed to be along the liquid-gas coexistence curve on a P-T phase diagram) Include all necessary detail in your derivation to demonstrate your understanding.

Then, Using the equation you derived in number 1, determine at which pressure and temperature water assumes the triple point. Assume ideal behavior. One-liquid-gas equilibrium point is (698 Pa, 275 K) and one solid-gas equilibrium point is (511 Pa, 271 K). Note: ΔHvap= 40 kJ/mol, ΔHfus= 6 kj/mol)

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