An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal equilibrium at 10°C. Two metallic blocks are placed into the water. One is a 47.9-g piece of silver at 80°C. The other has a mass of 345 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of 20°C.   (a) Determine the specific heat of the unknown sample.

A lab instructor performs an experiment using an aluminum cup that contains 225 g of water and a 130 g copper stirrer, all initially at 27.0°C. (Note that the student wears insulated gloves when handling the stirrer.) The lab instructor then adds a sample of silver to the water. The sample has a mass of 446 g and is initially at a temperature of 85.0*C. After stirring the mixture until it reaches thermal equilibrium, the lab instructor measures a final temperature of 32.0°C. What is the mass (in g) of the aluminum cup? Need Help? Read

An unknown substance has a mass of 0.250 kg and an initial temperature of 90.0°C. The substance is then dropped into a calorimeter made of aluminum containing 0.300 kg of water initially at 25.0°C (assume the water and calorimeter start in thermal equilibrium). The mass of the aluminum container is 0.200 kg, and the temperature of the calorimeter increases to a final equilibrium temperature of 32.0°C. Assuming no thermal energy is transferred to the environment, calculate the specific heat of the unknown substance.  The specific heat of water is 4186 J/(K*mol)  and aluminum is 900 J/(K*mol).

A block of metal of mass 0.360 kg is heated to 144.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.170 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 44.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 x 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K). J/(kg · K)

A 155 g copper bowl contains 230 g of water, both at 20.0°C. A very hot 300 g copper cylinder is dropped into the water, causing the water to boil, with 4.05 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? 8.6 X kcal (b) How much energy (in calories) is transferred to the bowl? 55 X kcal (c) What is the original temperature of the cylinder? 553.6 X °C Did you use the idea of conservation of energy? That is, did you equate the sum of the energy transfers to zero? For the bowl and cylinder, did you substitute the expression relating an energy transfer, the specific heat, the mass, and the temperature change? For the water, did you use the same expression to get the water to the boiling point? Did you also include an expression for the heat of vaporization? Did you use the given final temperature for each of the three materials?

A block of metal of mass 0.280 kg is heated to 148.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.190 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 44.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 x 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K). 3/(kg K)

A 0.100 kg piece of ice at initial temperature −5.00 ◦C is placed in a perfectly insulated container with 1.00 kg (1 L) of water at initial temperature 20.0 ◦C. The container absorbs or releases no heat. All of the ice melts as the system reaches an equilibrium temperature Tf .  How much heat must the ice exchange with the rest of the system to raise its temperature to the melting point, 0.00 ◦C? Would this heat exchanged be positive, zero, or negative? Once the ice reaches its melting point, how much heat must the ice exchange with the rest of the system to melt? Would this heat exchanged be positive, zero, or negative? Once the ice melts, it is liquid water at 0.00 ◦C. Write an expression for the heat exchanged by the newly-melted ice QI to reach the equilibrium temperature Tf . Would you expect QI to be positive, zero, or negative? Write an expression for the heat exchanged by the original water QW to reach the equilibrium temperature Tf from its initial temperature. Assuming no…