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

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?

2. Relevant equations

Equation of Isobaric thermodynamic: W = -p(delta V)

Ideal Gas Law: PV=nRT

3. 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?

**Physics Forums | Science Articles, Homework Help, Discussion**

Dismiss Notice

Join Physics Forums Today!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

# Homework Help: Isobaric Expansion

**Physics Forums | Science Articles, Homework Help, Discussion**