A hot 122.8 g lump of an unknown substance initially at 154.8 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 56.9 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. graphite zinc aluminum titanium tungsten rhodium Substance Specific heat (J/(g•°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 0.132 0.388 4.184 tungsten zinc water

A particular sample of cold graphite at 10.20 °C was added to 988.5 g of water at 25.31 °C in a constant pressure calorimeter. If the final temperature of the graphite and water was 25.17 °C, what was the mass of the graphite sample? Assume no heat was lost to the surroundings. The specific heat for water is 4.184 J/g•°C and the specific heat for this graphite is 0.7069 J/g•°C.

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.

8. Heat is applied to 50g of water (specific heat of 4.18J/°C) at 25°C.  The temperature of the water increases to 98°C.  What was the total amount of heat energy that was applied?

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

When a 0.740-g sample of trinitrotoluene (TNT), C,H,N,O, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter and its content is 3.35 kJ/°C. How much heat was produced by the combustion of the TNT sample? O 34.2 kJ O 11.7 kJ O 101.5 kJ

The specific heat of substance C is 0.93 J/(g K) and that of substance D is 1.8 J/(g K). You are given an unknown that could be pure substance C, pure substance D, or a homogeneous mixture of C and D. In the lab you determine that it requires 23.3 J of heat energy to raise the temperature of a 25.0 g sample of the unknown by 1.0 K. What conclusions can you make about the identity of your unknown, from this data?

3. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal.

A 135.0-g piece of iron is heated to 225 ℃ in an oven.  It is then dropped into a calorimeter containing 250.0-mL of glycerol (d = 1.261 g/mL) at 23.5 ℃.  The temperature of glycerol rises to a maximum value of 44.7 ℃.  Determine the specific heat of glycerol.

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: