What molar quantity of dinitrogen gas is present in a #300*mL# volume under standard conditions of temperature and pressure?

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1 Answer
anor277
Jul 23, 2017

Volume is a state function, of number of gaseous molecules......I gets approx. #0.01*mol#.

Explanation:

....and the pressure of those molecules, .......and the temperature of those molecules.........I will use #"STP"# as #105*kPa# and a temperature of #0# #""^@C#, i.e. #273.15*K#.

We use of course employ the Ideal Gas equation.........and the only difficulty is in finding the appropriate gas constant, #R#. This site lists the various gas constants, including the one I use here.

#R=8.3144598(48)xx10^-2*L*"bar"*K^-1*mol^-1#

#n=(PV)/(RT)=(1*"bar"xx300*mLxx10^-3*L*mL^-1)/(8.31xx10^-2*(L*"bar")/(K*mol)xx273.15*K)#

#=0.0132*mol# of #"dinitrogen gas"#. What is the mass of this gas?

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