Question

2. The change in enthalpy of solution (ΔHsolution) after two liquids are mixed is −93.8 kJ/mol....

2. The change in enthalpy of solution (ΔHsolution) after two liquids are mixed is −93.8 kJ/mol.

Use the equation and values provided to determine the energy released by the solute-solvent interaction (ΔH3).

ΔHsolution = ΔH1 + ΔH2 + ΔH3

solute-solute interaction (ΔH1) = +226.7 kJ/mol

solvent-solvent interaction (ΔH2) = +525.0 kJ/mol

______ kJ/mol

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Answer #1

ΔHsolution = ΔH1 + ΔH2 + ΔH3

solute-solute interaction (ΔH1) = +226.7 kJ/mol

solvent-solvent interaction (ΔH2) = +525.0 kJ/mol

The change in enthalpy of solution (ΔHsolution) after two liquids are mixed is −93.8 kJ/mol.

ΔHsolution = ΔH1 + ΔH2 + ΔH3

-93.8       = 226.7 + 525 + ΔH3

ΔH3        = -845.5KJ/mole

The equation and values provided to determine the energy released by the solute-solvent interaction (ΔH3) = -845.5KJ/mole >>>>answer

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