Using room temperature calculate the number of moles in the pressure/volume expe

Question

Using room temperature calculate the number of moles in the pressure/volume experiment when the pressure is 1.00 atm. Pressure-Volume Relationship in Gases Wernier Pressure Probe) 3.1 Set up a Vernier pressure sensor to a Vernier Lab Quest and change the units to atm with the stylus. Adjust the syringe volume to 10.0 mL and then connect to the pressure sensor. 3.2 Record the pressure values for 6 volumes (approx. 20, 16, 12, 9, 6, 4 mL). 3.3 Disconnect the syringe, adjust the volume to 5.0 mL and reconnect to the pressure sensor. Record the pressure for 5.0 mL. Increase the volume to 10 mL and then to 20 mL recording the pressure at each volume. 3.4 Repeat 3.3 starting at a volume of 20.0 mL and adjusting the volume to 10.0 mL recording the pressure at each volume.

Explanation / Answer

According to Boyle's law pressure and volume are inversely proportional for a fixed amount of the ideal gas kept at fixed temperature.

P.V = k

(k =proportionality constant)

If k shows constant or nearly constant value, then the above relationship is correct between pressure and volume.

From the first table, we can see all the values of k are similar it means we have established inverse relationship between P and V.

In the next table we can see as the volume is increasing, pressure is decreasing. When volume is doubled, the pressure nearly got half.

In the last table it is shown when volume is decreased, pressure increases. When volume decreased to half, pressure becomes nearly double.

Ideal gas law, PV = nRT

Boyle's law follow this law, as we know R is gas constant and n, T are kept constant. Therefore nRT whole is a constant.

Lets say room temperature is 25 oC or 298 K

R = 0.08205 L.atm/mol.K, P = 1 atm and V = 0.005 L

n = PV/RT = 1 x 0.005 / 0.08205 x 298 = 0.000204 moles = 2.04 x 10-4 moles

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