If 100 g of Cu at 80°C is dropped into 50 g of water at 20°C, what will be the final T of the water & copper? (The heat capacity of water is 75.3 J/mol/K and that of copper is 24.435 J/mol/K.)

A 232 mL soft drink (that contains mostly water) initially at 11.0 °C is cooled by adding 156.3 g of ice cubes at 0.0 °C. What mass of ice remains (in grams) when the temperature of the drink reaches equilibrium (water and ice at 0.0 °C)? The enthalpy of fusion of water (i.e., the heat required to melt ice) = 6.007 kJ/mol. Assume the density of soft drink is the same as the density water = 1.00 g/mL. Assume the specific heat capacity of soft drink is the same as water = 4.184 J/g/K.

You see a gold ring in a flea market that you’d like to have, and the price seems right, so you buy it. On the drive home you wonder if it’s really gold. You do a quick experiment and find it takes 38.7 J of heat to raise the temperature of the 6.00 g ring from 25oC to 75oC. You know that the specific heat of gold is 0.128 J/goC; is your ring really made of gold?

A hot lump of 47.547.5 g of iron at an initial temperature of 51.5 °C51.5 °C is placed in 50.0 mL H2OH2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g·°C)?0.449 J/(g·°C)? Assume no heat is lost to surroundings.