A sample of nitrogen gas occupies a volume of 2.55 L when it is at 755 mm Hg and 23 degrees Celsius. Use this information to determine the moles of nitrogen gas present. Volume is increased to 4.10 L and temperature is decreased to 18 degrees Celsius. Calculate the final pressure

The final pressure is 461.6 mm Hg

Explanation:

Step 1:Data given

Volume of N2 = 2.55L

Pressure N2 = 755 mm Hg

Temperature = 23.0 °C

New volume = 4.10 L

Temperature = 18.0 °C

Step 2: Calculate the fina pressure

P1V1/T1 = P2V2/T2

P2 = P1V1/T1 * T2/V2

⇒ with P1 = initial pressure = 755/760 atm =0.993421 atm

⇒ with V1 = the initial volume = 2.55L

⇒ with T1 = the initial temperature = 23.0 °C = 296 K

⇒ with P2 = The final pressure

⇒with V2 = the new volume = 4.10 L

⇒with T2 = the new temperature = 18.0 °C = 291 K

P2 = 755 mm *2.55 L *296K/(291 K* 4.10 L) = 461.6 mm Hg

The final pressure is 461.6 mm Hg

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