Question
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1. Calculate the work required to expand 1.3 moles of an ideal gas reversibly and atmospheres. 2. Suppose a gas is compressed from 20.1 liters to 10.3 liters against a pressure which is asonnernels fiom Viters to 3.I V, itr a 298'C. Report your answer in lir given by the formula presisting 10.3/V where the pressure is given in atmospheres and the volume is given in liters. What is the amount of work done on the gas? 3. Suppose 0.01 moles of an ideal gas is compressed from 20.1 liters to 10.3 liters isothermally (at 100°C) and reversibly. What is the amount of work done on the gas? 4. 3.2 moles of an ideal gas at 1 atm pressure and 23°C are heated at a constant pressure until the final temperature is 81°C. For the gas Cv (7.50+ 0.0032T) cal/(mole-°C). Note, the T in the above formula is in Kelvin!), i.e., the units apply to the entire formula! Calculate q (in calories) for the process. 5. Calculate the final temperature (in C) achieved in expanding 1.3 moles of an ideal gas reversibly and adiabatically from 2 liters to 3.1 liters if the original temperature is 298oC. Assume -5/3;
Explanation / Answer
Q1.
work required for
n = 1.3 mol
ideal gas
reversibly and isothermally
V1 = V1 to V2 = 3.1V1
T = 298°C = 571 K (note that this could be given as Kelvin, since 25°C, a very common temperature, is typically reportes as 298K)
Wrev = -n*R*T*ln(V2/V1)
Wrev = -1.3*8.314*571*ln(3.1)
Wrev = -6982.427 J
Wrev = -6.98 kJ
