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?