Question

What is the temperature at which ice and water are in equilibrium at a pressure of 1 atm? Calculate the amount of heat in joules required to melt 100 g of ice at this temperature assuming no change in pressure. (Hint: use the heat of fusion for water, which is 6.01 kJ/mol).

Answer 1

At a pressure of 1 atm, ice and water are in equilibrium at 0C  32F .To calculate the amount of heat required to melt 100 g of ice at this temperature, we first need to determine the number of moles of ice. The molar mass of water is 18.015 g/mol.Number of moles =  mass of ice  /  molar mass of water Number of moles = 100 g / 18.015 g/mol  5.55 molNow, we can use the heat of fusion for water  6.01 kJ/mol  to calculate the amount of heat required to melt the ice.Heat required =  number of moles    heat of fusion Heat required = 5.55 mol  6.01 kJ/mol  33.36 kJSince 1 kJ = 1000 J, the heat required to melt 100 g of ice at 0C and 1 atm pressure is:33.36 kJ  1000 J/kJ = 33,360 J