A 38-g ice cube floats in 250 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 90°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33  105 J/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg · °C, respectively.) (kg)

In an insulated vessel, 239 g of ice at 0°C is added to 635 g of water at 15.0°C. (Assume the latent heat of fusion of the water is 3.33 x 10° J/kg and the specific heat is 4,186 J/kg · °C.) (a) What is the final temperature of the system? °C (b) How much ice remains when the system reaches equilibrium?

A 20-g ice cube floats in 150 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 86°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 x 105 J/kg and 4,186 J/kg °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg °C, respectively.) kg Need Help? Read It Master It

"A person pours 330 g of water at 45°C into an 855-g aluminum container with an initial temperature of 10°C. The specific heat of aluminum is 900 J/kgK and that of water is 4190 J/kgK. What is the final temperature of the system, assuming no heat is exchanged with the surroundings?"