(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

One mole of a monatomic ideal gas is taken through the reversible cycle shown below.

http://img508.imageshack.us/img508/2595/newbitmapimageqm.png [Broken]

process bc is an adiabatic expansion, with P_b = 10.00 atm and V_b = 10^-3 m^3.

Find (a) the energy added to the gas as heat. (b) find the energy leaving the gas as heat, (c) the net work done by the gas, and (d) the efficiency of the cycle.

2. Relevant equations

PV=nRT (ideal gas)

PV^(gamma) = constant

gamma = C_p/C_v

V^(gamma-1)T = constant

U = (3/2)nRT (for a monatomic gas)

3. The attempt at a solution

I really dont know how to start this problem

I know for the bc section of the cycle Q = 0 because its an adiabatic expansion.

I also solved for the temperature at point b T = PV/(nR) = (1.0132*10^6Pa)(10^-3m^3)/(1mole)(8.315) = 121.85 K

from here im not sure what to do because I am not given gamma or the pressure at a or c

Your help is much appreciated

1. The problem statement, all variables and given/known data

2. Relevant equations

3. The attempt at a solution

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# Homework Help: Reversable process with adiabatic expansion

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