1kg of copper is transferred quickly from boiling water to a block of ice. Calculate the mass of ice melted, neglecting heat loss. [specific heat capacity o...

When 1kg of copper is transferred from boiling water to ice, it will first cool down from 100°C to 0°C, giving off heat to the surroundings, and then it will transfer heat to the ice, melting some of it. To calculate the mass of ice melted, we need to use the specific heat capacity of copper and the latent heat of fusion of ice. The amount of heat lost by the copper as it cools from 100°C to 0°C can be calculated as: Q1 = mCΔT where m is the mass of copper, C is its specific heat capacity, and ΔT is the change in temperature. ΔT = (100°C - 0°C) = 100°C Substituting the values, we get: Q1 = (1kg)(400Jkg-1K-1)(100°C) = 40,000J This heat is absorbed by the ice to melt it. The amount of heat required to melt a given mass of ice can be calculated as: Q2 = mL where m is the mass of ice and L is the latent heat of fusion of ice. L = 333 x 10³ Jkg-1 Substituting the values, we get: Q2 = (m)(333 x 10³ Jkg-1) Since the heat lost by the copper (Q1) is equal to the heat gained by the ice (Q2), we can equate the two equations: Q1 = Q2 mCΔT = mL Substituting the values, we get: (1kg)(400Jkg-1K-1)(100°C) = m(333 x 10³ Jkg-1) Solving for m, we get: m = 1.2 kg or 1200g Therefore, the mass of ice melted is 1200g, which is equivalent to 1.2 kg. Answer: 120g