Question

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?

Answer 1

`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?