3. A 74.5 g piece of metal at 86.0°C is placed in 133 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 24.2°C. How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.) J What is the specific heat (in J/g·°C) of the metal? J/g·°C

specific heat of gold is 0.129J/g C. what is molar heat capacity of gold?

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

1 A piece of metal with a specific heat of 1.011 J/gºC is heated to 123.1ºC and then placed in 111.031 g of water which is at a temperature of 3.6 ºC. After a minute, the temperature of the water has stopped changing and is now 55.8ºC. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

3. We all know that the hood of a car gets extremely hot in the summertime when a bright sun is shining on it. Suppose that a certain hood weighs 22.8 pounds and is composed of pure iron. If the specific heat of the iron is 0.450 J/g °C, what is the final temperature of the hood if it is heated from 20.0 °C by the addition of 4.0 x 102 kJ of sunlight? (Recall that 1 pound = 0.4536 kg)

A gas expands and does work on the surroundings equal to 4.92 Latm. At the same time, it releases 98.6 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)

A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C.   If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt?   How many moles of the unknown salt were used in the reaction ?     _______ J?

4. Determine the final temperature of water if 9.2 kJ of heat is added to 250 mL of 17°C water (the specific heat capacity of water is 4.184 J/g°C).

The specific heat of aluminum is 0.897 J/g·°C and the specific heat of water is 4.18 J/g·°C.  If a 3.00 g piece of aluminum at 300.0°C is immersed in 10.0 mL of water at 30.0°C, predict the final temperature of the mixture.