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amdma2003
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Homework Statement
5.00 g of nitrogen gas at 22.0 deg C and an initial pressure of 2.00 atm undergo an isobaric expansion until the volume has tripled.
A. How much heat energy is transferred to the gas to cause this expansion?
Homework Equations
Equation of Isobaric thermodynamic: W = -p(delta V)
Ideal Gas Law: PV=nRT
The Attempt at a Solution
Get the number of moles of the N2 gas: N2 = 28 g/mol ; moles = 5/28
Convert 22 deg C to Kelvin: 273.15 + 22 = 295.15 K
Convert 2.00 atm to Pascals: 2 atm = 202 650 pascals
R is 8.31
Find V initial:
PV = nRT
(202650)V = 0.1786(8.31)295.15
Vi = 0.0022
Find V final: Vf = 3(Vi) = 0.0065
Now Find the Work done:
W = -p(DELTA V)
Since pressure stays constant at 202,650 Pascals then:
W = -202650(0.0065-0.0022) = 871.395 J
However this is wrong, and I do not understand why. Can someone walk me through this problem?