How much heat is required to convert 5.0g of ice at 0 ° C to water at the boiling point? (Specific latent heat…

Analyze the question: We need the total heat to (1) melt 5.0 g of ice at 0 °C into water at 0 °C, then (2) heat that water from 0 °C to 100 °C (boiling point).

Concept:

• Heat to melt: Q₁ = m × L
• Heat to warm water: Q₂ = m × c × Δθ

Solution:

Step 1: Melting the ice Q₁ = 5.0 × 336 = 1680 J

Step 2: Heating the water from 0 °C to 100 °C Q₂ = 5.0 × 4.2 × (100 − 0) = 5.0 × 4.2 × 100 = 2100 J

Step 3: Total heat Q = Q₁ + Q₂ = 1680 + 2100 = 3780 J

Answer: 3780 J, which is option E.

Tip: When a question says "ice to water at boiling point," always count two stages: melting (latent heat, no temperature change) and heating (specific heat capacity, with a temperature change). Option B (1680 J) and option D (2100 J) are the traps for students who do only one stage. Always check whether you have included every stage!