If an ideal gas has a pressure of 4.97 atm, a temperature of 481 K, and has a volume of 29.83 L, how many moles of gas are in the sample?

1 Answer
anor277
May 13, 2016

#n~=4*mol#

Explanation:

The Ideal Gas Law explicitly states that:

#n=(PV)/(RT)# #=# #(4.97*cancel(atm)xx29.83*cancelL)/(0.0821*cancel(L)*cancel(atm)*cancel(K^-1)*mol^-1xx481*cancelK)# #=# #??*mol#.

Note that the only problem in solving this problem is choosing an appropriate gas constant, #R#. For chemists, #R=0.0821*L*atm*K^-1*mol^-1#, is very useful because it uses the units that chemists would typically use, i.e. #"atmospheres, litres, etc."#. Is the equation correct dimensionally?

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