Unit Conversions & Gas Laws

a) 850 mm Hg to atm

Solution: Atm = mm of Hg / 760
Atm = 850 / 760 = 1.12 atm

b) 205000 Pa to atm

Solution: Pa / 101325 = 2.02 atm

c) 560 torr to cm Hg

Solution: torr × 0.01 = 56 cm Hg

d) 1.25 atm to Pa

Solution: Atm × 101325 = 126656 Pa

a) 750°C to K

Solution: K = °C + 273 = 750 + 273 = 1023 K

b) 150°C to K

Solution: K = 150 + 273 = 423 K

c) 100 K to °C

Solution: °C = 100 - 273 = -173°C

d) 172 K to °C

Solution: °C = 172 - 273 = -101°C

A gas at pressure 912 mm of Hg has volume 450 cm³. What will be its volume at 0.4 atm?

Solution: V₂ = 1350 cm³

A gas occupies a volume of 800 cm³ at 1 atm. When it is allowed to expand to 1200 cm³, what will be its pressure in mm Hg?

Solution: P₂ = 506.66 mm Hg

It is desired to increase the volume of a fixed amount of gas from 87.5 to 118 cm³ while holding the pressure constant. The initial temperature is 23°C.

Solution: T₂ = 399 K = 126°C

A sample of gas is cooled from 30°C to 10°C at constant pressure.

Solution: The volume decreases in the ratio 1:0.93.

A balloon with a volume of 1.6 dm³ at standard temperature and pressure is taken underwater to a depth where its pressure increases to 3.0 atm. Temperature remains unchanged.

Solution: The volume decreases to 0.53 dm³, and the balloon contracts.

A sample of neon gas occupies 75.0 cm³ at 0.4 atm. What would be the volume at 1.0 atm if temperature remains constant?

Solution: V₂ = 30.0 cm³

A gas occupies 35.0 dm³ at 17°C. If the temperature rises to 34°C at constant pressure, would you expect the volume to double?

Solution: The volume will not double. V₂ = 37.05 dm³

The atmospheric pressure on Titan is 1.50 atm. Express this pressure in torr.

Solution: P = 1140 torr