Assume that a particular reaction evolves 229 kJ of heat and that 27 kJ of PV work is gained by the system. What is the value of ΔE for the system? What is the value of ΔH for the system? What is the value of ΔE for the surroundings?

3 If we measure the heat change (q) of everything in a system except the calorimeter, we can use the first law of thermodynamics (∆Euniverse = 0) to calculate the heat change of the calorimeter (qcal).  In this reaction, we combine 5.75 g of 67.4 ºC water with 6.67 g of 19 ºC water in a calorimeter.  Since some of the heat is absorbed by the calorimeter, the final temperature of the water is 25.4ºC.  Since the hot and cold water are combined, the final temp of the water is the final temp for the hot water and the cold water.  Calculate the heat change of the calorimeter in J. Remember that all of the heat changes must add up to zero so you can calculate the heat change of the hot water (qhotwater) and the heat change of the cold water (qcoldwater) using for each where Cs = 4.186 J/gºC.  The first law of thermodynamics tells us that all of these changes sum up to zero so   Enter your answer to one decimal place (tenths)

A 0.576 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.957 kJ °C^-1. If the temperature inside the calorimeter increased from 25.0 °C to 35.1 °C, determine A,U for this reaction in kl mol (with respect to C3H12). Do not worry about how realistic the final answer is.

How much work, w, must be done on a system to decrease its volume from 18.0 L to 11.0 L by exerting a constant pressure of 6.0 atm? w = kJ