How would you determine the volume that 1 mol of a gas at 0°C and 1 atm occupies?

Answer 1

By means of the Ideal gas law.

#PV = nRT#; where #P# is pressure; #V# is volume; #R# is the appropriate gas constant (usefully #R# #=# #0.0821# #L*atm*K^(-1)*mol^(-1)#), and #T# is the absolute temperature in Kelvin, #K#.

These constants will always be provided to you; however, you will need to work with them in order to obtain an answer with the correct units.

If #V# #=# #(nRT)/P#, then #V# #=# #(1*molxx0.0821*L*atm*K^(-1)*mol^(-1)xx273K)/(1*atm)# will give me an answer in litres.

Alternatively, it is a given that 1 mole of ideal gas will occupy a volume of #22.4# #dm^3# at #273# #K#. And #1# #dm^3# #=# #{1xx10^(-1)m}^3# #=# #1xx10^(-3)*m^3# #=# #1# #L# (a litre is a 1000th of a cubic metre).

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Answer 2

Henry Antrim

Use the Ideal Gas Law: V = RT/P, where V is volume, R is the ideal gas constant, T is temperature in Kelvin, and P is pressure. At 0°C, convert to Kelvin (273 K), and for standard pressure, use 1 atm.

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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.