How much heat is required to melt 5.00 g of ice at 0 °C? ΔHf°(ice) = 6.01 kJ/mol; M = 18.015 g/mol

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Multiple Choice

How much heat is required to melt 5.00 g of ice at 0 °C? ΔHf°(ice) = 6.01 kJ/mol; M = 18.015 g/mol

Explanation:
Melting at the melting point uses latent heat, so the heat added goes into changing the phase rather than raising temperature. Convert the mass of ice to moles and multiply by the enthalpy of fusion: n = 5.00 g / 18.015 g/mol ≈ 0.278 mol. q = n × ΔHf° = 0.278 mol × 6.01 kJ/mol ≈ 1.67 kJ. This rounds to about 1.66 kJ with the given data, matching the choice.

Melting at the melting point uses latent heat, so the heat added goes into changing the phase rather than raising temperature. Convert the mass of ice to moles and multiply by the enthalpy of fusion: n = 5.00 g / 18.015 g/mol ≈ 0.278 mol. q = n × ΔHf° = 0.278 mol × 6.01 kJ/mol ≈ 1.67 kJ. This rounds to about 1.66 kJ with the given data, matching the choice.

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