.Two moles of an ideal monoatomic gas (CV=20.9JK-1mol-1)are heated from 300K to 350K.The volume of the gas changes from 0.02m3 to 0.2m3.Assuming that the heat capacity remains constant in this temperature change for the system, calculate; i. Entropy change for the system. ii. Entropy change for the surroundings. iii. Entropy change for the universe.

a) Explain how the gas equation PV=nRT has been modified to take account of the behavior of the real gases.(5marks)
b) Explain the significance o f the symbols in the equation PV=nRT and state any two of the gas laws it summarizes.(5marks)
c) Two moles of an ideal gas initially at 270c and one atmosphere are compressed reversibly to half the initial volume. Calculate the value of q, w, ?E and ?H when the process is carried on isothermally. (8marks)
d) A steel bottle contains 20 liters of hydrogen at 270c and a pressure of 50 atm. The gas expands isothermally and reversibly to 100 liters. Calculate:
1) How much heat had to be supplied? (4 marks) 2)The pressure of the hydrogen after expansion. (4 marks) 3)How much work was performed by the gas during expansion .(4 marks)
1. A)Explain with an example each of the following :
a) An adiabatic process .(2 marks)
b) An isochoric process.(2 marks)
c) Isothermal process.(2 marks)
d) Systems and surroundings.( 2 marks)
e) Closed system and isolated system.( 2 marks)
B)One mole of a diatomic gas at 300k and 5 atm expands to 1 atm. Assuming ideal behavior, calculate w, q, ?E and ?H if the expansion carried out was adiabatic and reversible.
Given CV=20.9JK-1mol-1
Cp=29.9JK-1mol-1 (20 marks)





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