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If 110.4 grams of oxygen gas exerts 101.3 kPa of air pressure at 0°C, what volume would the gas occupy?

Answer 1

Wyatt Adkins

#154.69"L"#

We use the Ideal Gas Law:

#PV=nRT#

First we must convert the mass to moles. The molar mass of oxygen is #15.999"g/mol"#, so:

#n=110.4/15.999=6.9"mol"#

Here,

#P=101.3"kPa"#

#n=6.9"mol"#

#T=273.15"K"#

#R=8.314"L kPa K"^-1"mol"^-1#

Rearranging the equation to solve for #V#:

#V=(nRT)/P# and inputting:

#V=(6.9*8.314*273.15)/101.3#

#V=154.69"L"#

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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