Problem
A blacksmith dunks a red-hot horseshoe into a large bucket of $22^{\circ} \mathrm{C}$ water. How much heat is lost by the horseshoe vaporizing $0.01 \mathrm{~kg}$ of water? $\left(c_{\text {water }}=4180 \mathrm{~J} / \mathrm{kg} \mathrm{C}, 1_{\text {water to steam }}=2.26 \times 10^{6} \mathrm{~J} / \mathrm{kg}\right)$
Solution
Step 1 ：Given mass of water (m) = 0.01 kg and latent heat of vaporization (L) = 2.26 * 10^6 J/kg
Step 2 ：Calculate heat transfer (Q) using the formula Q = m * L: \(Q = 0.01 \times 2.26 \times 10^6\)
Step 3 ：\(Q = 22600\)
Step 4 ：\boxed{22600 \text{ J}}
