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)

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Accepted Answer

Step:1 ：Given mass of water (m) = 0.01 kg and latent heat of vaporization (L) = 2.26 * 10^6 J/kgStep: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}}

Answer

Step: 1 ：Given mass of water (m) = 0.01 kg and latent heat of vaporization (L) = 2.26 * 10^6 J/kgStep: 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}}

A blacksmith dunks a red-hot horseshoe into a large bucket of $22^{\circ} C$ water. How much heat is lost by the horseshoe vaporizing $0.01 kg$ of water? $(c_{water} = 4180 J / kg C, 1_{water to steam} = 2.26 \times 10^{6} J / kg)$

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Popular Problems

A blacksmith dunks a red-hot horseshoe into a large bucket of 22∘C water. How much heat is lost by the horseshoe vaporizing 0.01 kg of water? (cwater =4180 J/kgC,1water to steam =2.26×106 J/kg)

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A blacksmith dunks a red-hot horseshoe into a large bucket of $22^{\circ} C$ water. How much heat is lost by the horseshoe vaporizing $0.01 kg$ of water? $(c_{water} = 4180 J / kg C, 1_{water to steam} = 2.26 \times 10^{6} J / kg)$