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# application of ideal gas law

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Convert the following pressure into atmospheres.
781 torr
781 mm Hg

A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L. What will be the pressure in the expnaded gas sample at a constant temperature.

At conditions of constant temperature and pressure, the volume of a sample of ideal gas is proportional to the number of moles of gas present.

If 3.25 mol of argon gas occupies a volume of 100L at a particular temperature and pressure, what volume does 14.15 mol of argon occupy under the same conditions.

Suppose a 24.3-ml sample of helium gas at 25 degrees C and 1.01 atm is heated to 50 degrees C and compressed to a volume of 15.2 ml. What will the pressure of the sample be.

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## SOLUTION This solution is FREE courtesy of BrainMass!

convert the following pressure into atmospheres.

1. 1 torr = 1 mmHg
1 atm = 760 mmHg
So 1 mmHg = atm
Then 781 torr = 781 mmHg = 781 * atm = 1.0276 atm

2. A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L. What will be the pressure in the expnaded gas sample at a constant temperature.
According to Boyle's law, at the constant temperature,

At conditions of constant temperature and pressure, the volume of a sample of ideal gas is proportional to the number of moles of gas present.
By ideal gas law,

Where is constant with constant temperature and pressure.
So V is directly proportional to the number of moles of the gas.

If 3.25 mol of argon gas occupies a volume of 100L at a particular temperature and pressure, what volume does 14.15 mol of argon occupy under the same conditions.
From the above equation, we know that with constant temperature and pressure:
So

The volume is 435.38 L.

Suppose a 24.3-ml sample of helium gas at 25 degrees C and 1.01 atm is heated to 50 degrees C and compressed to a volume of 15.2 ml. What will the pressure of the sample be.
By ideal gas law, is constant for certain moles of gas.
The unit of the temperature T is Kelvin.
So 25 C = 25 + 273.15 K
50 C = 50 + 273.15 K

The pressure is 1.75 atm.

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