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 copper cube with an edge measuring 1.55 cm and an aluminum cube with an edge measuring 1.62 cm are both heated to 55.0 °C and submerged in 100.0 mL of water at 22.2 °C. What is the final temperature of the water when equilibrium is reached? (Assume a density of 0.998 g/mL for water.)

A pure gold ring and a pure silver ring have a total mass of 14.9 g. The two rings are heated to 62.0 °C and dropped into 15.0 mL of water at 23.5 °C. When equilibrium is reached, the temperature of the water is 25.0 °C. What is the mass of each ring? (Assume a density of 0.998 g/mL for water.)

A 10.69-g block of solid platinum at 66.41°C is immersed in a 23.93-g pool of liquid ethanol with a temperature of 12.95°C. When thermal equilibrium is reached, what is the final temperature of the platinum and ethanol? Specific heat capacities: platinum = 0.133 J/g°C, ethanol = 2.44 J/g°C.

A 14.4 g sample of granite initially at 75.0 °C is immersed into 30.0 g of water initially at 21.0 °C. Assuming the specific heat capacity of granite is 0.79 J/g°C, what is the final temperature of both substances when they reach thermal equilibrium?

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 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.