An insulated container holds 1.00 L of warm water at an initial temperature of 3

Question

An insulated container holds 1.00 L of warm water at an initial temperature of 37.0 C. Then 825 g of ice, initially at 0C, iss added to the water. The ice begins to melt as the water cools, and eventually equilibrium is reached with both ice and water present at 0 C. What mass of ice remains unmelted. (Assume that no heat is lost or gained from the surroundings)

Densities: ice=0.917 g/cm^3 liquid water=1.00g/mL

Heat capacities: ice=37.5 J/mol/K=2.08 J/g/C liquid water=75.3 J/mol/K=4.18 J/g/C

Heat of fusion of ice=6.01 kJ/mol Heat of vaporization of water=40.7 kJ/mol

Explanation / Answer

energy released from water Q= m x Cp x delta T

mass of water m = density x volume = 1g/mL x 1L = 1000g

Q = 1000g x 4.18 J/g/oC x (37 -0) = 154660J

This heat = mass of ice x (heat fusion)

154660 = mass x 6010J

mass of ice = 25.73g

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