1 . A sample of gas has an initial volume of 14.0 L at a pressure of 1.37atm. A)

Question

1 . A sample of gas has an initial volume of 14.0 L at a pressure of 1.37atm.

A)If the sample is compressed to a volume of 10.5 L , what will its pressure be

2. What is the volume occupied by 10.4 { m g} of argon gas at a pressure of 1.05 atm and a temperature of 452 K?

3. A weather balloon is inflated to a volume of 27.0 L at a pressure of 737 Hg and a temperature of 25.3 { m ^circ { m C}} . The balloon rises in the atmosphere to an altitude where the pressure is 390. Hg and the temperature is -13.6 { m ^circ { m C}} .

Explanation / Answer

1. Using

P1V1 = P2V2

where,

P1 = 1.37 atm

P2 = unknown

V1 = 14 L

V2 = 10.5 L

Feed values,

P2 = 1.37 x 14/10.5 = 1.83 atm will be the final pressure

2. Using,

PV = nRT

where,

P = 1.05 atm

V = unknown

n = 10.4 g/molar mass = 10.4/39.948 = 0.26 mols

R = 0.0821 L.atm/K.mol

T = 452 K

Feed values,

V = 0.26 x 0.0821 x 452/1.05 = 9.19 L will be the volume occupied by the gas

3. Calculate moles of gas

n = PV/RT

where,

P = 737 mmHg = 0.96974 atm

V = 27 L

R = 0.0821 L.atm/K.mol

T = 25.3 oC = 25.3+273 = 298.3 K

Feed values,

n = 0.96974 x 27/0.0821 x 298.3 = 1.07 mols

Now for the baloon at altitude,

V = nRT/P

where,

n = 1.07 mols

R = 0.0821 L.atm/K.mol

T = -13.6 oC = -13.6 + 273 = 259.4 K

P = 390 mmHg = 0.51316 atm

Feed values,

V = 1.07 x 0.0821 x 259.4/0.51316 = 44.41 L will be the volume of gas at altitude

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