the same .0500 mole of ideal gas is now expanded at constant temperature (t=244
ID: 886542 • Letter: T
Question
the same .0500 mole of ideal gas is now expanded at constant temperature (t=244 k) from 1 l to 2 Liters . How much works is done ? And what are the initial and final pressures .I got w=0 joules and p1= 1.002 ATM and P2=.501 the same .0500 mole of ideal gas is now expanded at constant temperature (t=244 k) from 1 l to 2 Liters . How much works is done ? And what are the initial and final pressures .
I got w=0 joules and p1= 1.002 ATM and P2=.501 the same .0500 mole of ideal gas is now expanded at constant temperature (t=244 k) from 1 l to 2 Liters . How much works is done ? And what are the initial and final pressures .
I got w=0 joules and p1= 1.002 ATM and P2=.501
Explanation / Answer
n = 0.05 mol
T = 244 K
V1 = 1 L
P1 = n*R*T/V1
= 0.05*0.0821*244/1
=1.00162 atm <-- initial pressure
V2 = 2L
P2 = n*R*T/V2
= 0.05*0.0821*244/2
= 0.050081 atm <-- final pressure
work done = n*R*T * ln (Vf/Vi)
= 0.05*8.314*244* ln(2/1)
= 70.31 J
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