A 2.54 g lead weight, initially at 10.3 °C, is submerged in 7.47 g of water at 52.5 °C in an insulated container. What is the final temperature of both substances at thermal equilibrium? Express the temperature in degrees Celsius.

A 140.0 g sample of water at 20.0 °C is mixed with 100.0 g of a certain metal at 95.0 °C. After thermal equilibrium is established, the temperature of the mixture is 24.6 °C. What is the specific heat capacity of the metal?

A 140.0 g sample of water at 20.0 °C is mixed with 100.0 g of a certain metal at 95.0 °C. After thermal equilibrium is established, the temperature of the mixture is 24.6 °C. What is the specific heat capacity of the metal?

A 2.10 g sample of lead, initially at 51.0 °C, is submerged into 76.1 g of water at 17.8 °C in an insulated container. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of lead is 0.128 J/g°C and the specific heat capacity of water is 4.18 J/g°C.)

A 2.32 g lead weight, initially at 10.1 °C, is submerged in 7.61 g of water at 53.0 °C in an insulated container. What is the final temperature of both the weight and the water at thermal equilibrium?

A 32.8 g iron rod, initially at 22.8 °C, is submerged into an unknown mass of water at 64.0 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.5 °C. What is the mass of water?

A calorimeter contains 365 g of water at 30.0 °C. A 29.3-g sample of ice (at -11.0 °C) is added to the water in the calorimeter, and eventually all of the ice melts. Calculate the final temperature of the water. Assume no heat is lost to the calorimeter.

A 1.3 g wafer of pure gold initially at 69.8 °C is submerged into 64.1 g of water at 26.9 °C in an insulated container. The specific heat capacity for gold is 0.128 J/g°C and the specific heat capacity for water is 4.18 J/g°C. What is the final temperature of the system when thermal equilibrium is reached?

A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron is 0.449 J/g·K and the specific heat capacity of water is 4.18 J/g·K.