If 7.54 moles of an ideal gas has a pressure of 3.95 atm, and a volume of 66.93

Question

If 7.54 moles of an ideal gas has a pressure of 3.95 atm, and a volume of 66.93 L, what is the temperature of the sample in degrees Celsius? If 85.5 mol of an ideal gas occupies 76.5 L at 75.00 °C, what is the pressure of the gas?A sample of an ideal gas at 1.00 bar and a volume of 1.14 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 85.0 bar, what was the volume of the sample? Assume that the temperature was held constant.

Explanation / Answer

1st part:

no of moles = 7.54

Pressure = 3.95

volume = 66.93 L

Using Ideal gas equation

Pv = nRT

3.95 * 66.93 = 7.54 * 0.083 * T

T = 422 K

Second part:

no of moles = 85.5

volume of the gas given = 76.5 L

Temperature = 348 K

Pv =nRT

P* 76.5 = 85.5 * 0.083 * 348

P = 32.282 atm

Third part:

Boyle's law states that when temperature is constant

Pi vi = Pf Vf

Intial pressure = 1 bar . initial volume = 1.14 L

Final pressure = 85 bar final volume = ?

1*1.14 = 85 * Vf

Vf = 0.0134 litres.

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