A silver block, initially at 58.5 °C, is submerged into 100.0 g of water at 24.8 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.2 °C. What is the mass of the silver block?

A hot lump of 25.4 g of aluminum at an initial temperature of 83.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.

A 1095 g piece of iron initially at 1371 °C is submerged in 1000.0 g of water initially at 20.0 °C. The temperature of the water increases, and some of the water evaporates. At thermal equilibrium, the final temperature of the iron, water, and water vapor (steam) is 100.0 °C. How many moles of water evaporated to reach thermal equilibrium? The specific heat capacity of iron is Cs, Fe = 0.449 J /g.°C The specific heat capacity of liquid water is Cs, water = 4.18 J/g.°C The enthalpy of vaporization of water is AHvap :40.7 kJ/mol Circle your answer on the written template. Be sure that it is in the correct units (mol) and has the correct number of significant figures.

A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol

A 395.7 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 was established, the temperature of the mixture is 24.6 °C. What is the specific heat capacity of the metal?

A 350.0 g iron pot is heated on a stove for a period of time until it is hot. The stove is turned off and 516 g of cold water (10.0 °C) is added to the pot. When thermal equilibrium is reached, the temperature of the water is  28.4 ° C. What was the initial temperature of the iron pot, assuming heat was exchanged between these two objects and none was lost to the surroundings? (The specific heat capacity of iron is 0.450 J/g °C. The specific heat capacity of water is 4.184 J/g °C) Give only the numerical answer in the box and not units. Give 4 sig figs in your answer. Show the calculations for the problem by writing it on a paper, upload the image file/pdf file in the question for file upload.

A 32.5-g iron rod, initially at 22.7 °C, is submerged into an unknown mass of water at 63.2 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.5 °C. What is the mass of the water?

A 1.261 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 25.39 °C to 28.44 °C. The heat capacity (calorimeter constant) of the calorimeter is 27.69 kJ/ °C, what is the heat of combustion per gram of the material? heat of combustion: kJ/g

A student transferred 50.0 ml 1.00 M HCl into a coffee-cup calorimeter, which had a temperature of 25.5 °C. He then added this to 50.0 ml 1.00 M NaOH which also had a temperature of 25.5 °C and stirred the mixture quickly. The resulting solution was found to have a temperature of 32.5 °C. The calorimeter constant for the coffee-cup calorimeter used was 15.0 J/°C. Calculate the heat of reaction. Please include the full solution.

2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?