Answer:
It takes 1,068.76 grams of nitrogen to fill an 855 L tank at STP.
Explanation:
The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C or 273.15 °K are used and are reference values for gases.
On the other side, the pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:
P*V = n*R*T
where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.
So, in this case:
Replacing:
1 atm* 855 L= n* 0.082 [tex]\frac{atm*L}{mol*K}[/tex] * 273.15 K
Solving:
[tex]n=\frac{1 atm* 855 L}{0.082\frac{atm*L}{mol*K} *273.15 K }[/tex]
n= 38.17 moles
Being the molar mass of nitrogen N2 equal to 28 g / mol, you can apply the following rule of three: if there are 28 grams in 1 mole, how much mass is there in 38.17 moles?
[tex]mass=\frac{38.17 moles*28 grams}{1 mole}[/tex]
mass= 1,068.76 grams
It takes 1,068.76 grams of nitrogen to fill an 855 L tank at STP.
