How do you calculate the density of carbon dioxide at 546 K and 4.00 atmospheres pressure?
1 Answer
Jun 13, 2017
Explanation:
The equation for the density of a gas is given by the equation
where

#rho# (the lowercase Greek letter rho) is the density, in#"g"/"L"# , 
#M# is the molar mass of the gas (for#"CO"_2# , this is#44.01"g"/"mol"# ), 
#P# is the pressure exerted by the gas (#4.00# #"atm"# ), 
#R# is the universal gas constant, equal to#0.082057 ("L"·"atm")/("mol"·"K")# , and 
#T# is the absolute temperature of the gas (#546# #"K"# ).
Plugging in known values, we have
The density of the gas is thus