Problem

Problem 115 A flask containing 2.0 moles of He gas at 1.0 atm and 300 K is connected to another flask containing N2(g) at the same temperature and pressure by a narrow tube of negligible volume. Volume of the nitrogen flask is three times volume of He-flask. Now the He-flask is placed in a thermostat at 200 Kand N2-flask in another thermostat at 400 K. Determine final pressure and final number of moles in each flask.

Answer

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Answer

6. Solve for n: n=3(400)2003001

Steps

Step 1 :1. Use ideal gas law to find volume of He flask: VHe=nHeRTP

Step 2 :2. Calculate volume of N2 flask: VN2=3VHe

Step 3 :3. Determine total volume after temperature change: VHe=nHeR(200)1.0

Step 4 :VN2=3nHeR(400)1.0

Step 5 :4. Calculate final pressure: Pfinal=nHeRT1+3nHeRT2VHe+VN2

Step 6 :5. Update the number of moles: nHe=21+n

Step 7 :nN2=2n1+n

Step 8 :6. Solve for n: n=3(400)2003001

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