Having just invented a new type of calorimeter, Dr. Campbell needs to determine the heat capacity of the calorimeter.  She carries out the following experiment to do this: She puts 20.0 grams of water in her empty calorimeter and it is allowed to stabilize at a temperature of 25.0ºC.  She then adds 35.586 grams of water at a temperature of 83ºC to the calorimeter.  After a few minutes the final temperature of the calorimeter stabilizes at 47.8ºC.   Based on this experiment, what is the heat capacity of her calorimeter assuming units of J/ºC? Enter your answer with at least 3 sig figs.

air at dry ball temperature 90 ° C and RH 8% is passed over the cooling coil so that the air dry ball temperature becomes 45 ° C. How much heat is released from the air in the process? = answer (kJ / kg)

2-37 Water is being heated in a closed pan on top of a range while being stirred by a paddle wheel. During the process, 30 kJ of heat is transferred to the water, and 5 kJ of heat is lost to the surrounding air. The paddle-wheel work amounts to 500 Nm. Determine the final energy of the sys- tem if its initial energy is 10 kJ. Answer 35.5 kJ 5 kJ 500 N-m 30 kJ

Insulated Sample Burning outside dish sample chamber Steel bomb Combustion (bomb) calorimeter. In an experiment, a 0.6629 g sample of phthalic acid ( C8H604) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.046 x 10³ g of water. During the combustion the temperature increases from 24.04 to 26.63 °C. The heat capacity of water is 4.184 J-g¹. C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 788.9 J. ˚C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phthalic acid based on these data. C8 H6 O4(s) + (15/2) O2(g) → 3H₂O(l) + 8CO2 (g) + Energy kJ/mol Molar Heat of Combustion =