Answer: 2,448 J
Step-by-step explanation:
1) The process in which the 12.4 g gold sample was melted can be splited in two differentiated stages: i) the increase of temperature from 26°C to 1064°C, and ii) the melting perse, which is at constant temperature.
Each stage is ruled by it specific thermodynamic model, which you can use to compute how much energy the gold gained.
2) Rising temperature
The heat energy gained by the gold to increase the temperature is given by the equation Q₁ = mCΔT.
Where m is the mass of gold, 12.4g, C is the specific heat, 0.1291 J/g°C, and ΔT is the change of temperature, 1,064°C - 26°C. Hence:
Q = 12.4g × 0.1291 J/g°C × (1,064°C - 26°C) = 1,661 J.
3) Melting
The heat energy during this stage is computed with the formula for the latent heat of fusion:
Q₂ = m × latent heat of fusion = 12.4 g × 63.5 J/g = 787.4 J ≈ 787 J.
3) The total heat energy gained, Q, is the sum of the energy gained during the two stages:
Q = Q₁ + Q₂ = 1,661 J + 787 J = 2,448 J ← answer