A metal object with mass of 21.7 g is heated to 97.0 °C and then transferred to an insulated container containing 83.5 g of water at 20.5 °C. The water temperature rises and the temperature of the metal object falls until they both reach the same final temperature of 24.0 °C. What is the specific heat of this metal object? Assume that all the heat lost by the metal object is absorbed by the water. specific heat: cal g. °C

A 50.8 g sample of an unknown metal was heated to 700.0 ˚C then placed into 100.0 g of water (specific heat: 4.184) initially at 25.0 ˚C. The water and the unknown metal reach equilibrium when both are at 78.3 ˚C. What was the specific heat of the unknown metal?

17. An ice cube is placed in a sealed insulated container of hot water at 80°C. After five minutes, the ice cube disappears. Ice Cube Heat ener Hot Water 5 min. Water Which best describes the change that took place inside the container? The total heat energy in the container was reduced by the ice cube. The hot water lost the same amount of heat energy as the ice cube gained. in the hot water was reduced by kinetic energy in the ice cube. O Heat energy in the ice cube was dissipated into the hot water.

10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C

A 19.3 g sample of beryllium at 96.7°C is placed into 46.2 mL of water at 20.2°C in an insulated container. The temperature of the water at thermal equilibrium is 32.0°C. What is the specific heat of beryllium? Assume a density of 1.00 g/mL for water. (See this table.)  J/(g·°C)

Calculate the specific heat capacity of an unknown metal if 30 grams of the unknown metal at 24.5°C is placed in a container containing 68.0 grams of water at 85°C. Then the water cools down and the metal warms up until thermal equilibrium is achieved at 79.1°C. Assume all the heat lost by the water is gained by the metal and the container is insulated. The specific heat capacity of water is 4.18 J g-1°C-1 1.02 5.32 2.81 0.45

A 120.0 g sample of a metal at 75.0 °C is added to 150.0 g H20 at 15.0 °C. The temperature of the water rises to 18.3°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. Specific heat capacity for water is 4.18 J / °C g.

A metal object with mass of 21.4 g is heated to 97.0 °C and then transferred to an insulated container containing 81.7 g of water at 20.5°C. The water temperature rises and the temperature of the metal object falls until they both reach the same final temperature of 23.1 °C. What is the specific heat of this metal object? Assume that all the heat lost by the metal object is absorbed by the water. cal specific heat: