Question

a sample of hydrogen gas occupies a volume of 300 ml at 1.2 bar pressure and 5 degree Celsius calculate its volume at 0.45 by pressure and 70 degree Celsius

Answer 1

P1*V1/T1 =P2*V2/T2

1.2*300/278 =0.45*V2/343

123480/125

=987 ml=v2

Answer 2

Concept:

• Ideal gas laws
• PV = nRT where P is the pressure, V is the volume, n is the number of moles, R is the gas constant and T is the temperature in Kelvin

Given:

• Initial volume V1 = 300 mL
• Initial pressure P1 = 1.2 bar
• Initial temperature T1 = 5 degrees celsius = 278 K
• Final Pressure P2 = 0.45 bar
• Final temperature T2 = 70 degrees celsius = 343 K

Find:

• The final volume V2

Solution:

PV = nRT

If the the number of moles are the same

P1V1/T1 = P2V2/T2

V2 = P1V1T2/T1P2

300* 1.2 / 278 = 0.45 V2/ 343

360/278 * (343/0.45) = V2

V2 = 987 mL

The volume of the gas is 987 mL.

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