`suppose you have a fixed container containing 19.08 grams of one of the diatomic (elemental) gases. if the container volume is 3.82 l, and the pressure is 4.78 atm, and the temperature is 100°c, which gas is it? (r = 0.0821 l∙atm/mol∙k)

solution:

First we calculate the number of mole of gas as follows:

PV = n RT

Here temperature; T= 100°C or 373 K

n = PV/ RT

= 4.78 atm * 3.82 L / 0.0821 L ∙ atm / mol ∙ K * 373 K

= 0.596 Moles

Now determine the molar mass of gas as follows:

Number of moles = amount in g/ molar mass

Molar mass = 19.08 grams / 0.596 Moles

= 32.013 g/ mole

This the molar mass of O2 hence the gas is oxygen

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