Answer is: the pressure of carbon dioxide is 2.41 atm.
n(CO₂) = m(CO₂) ÷ M(CO₂),
n(CO₂) = 4.35 g ÷ 44 g/mol.
n(CO₂) = 0.098 mol; amount of substance.
V = 1.00, volume of
gas.
T = 300 K; temperature.
R = 0.08206 L·atm/mol·K, universal gas constant.
Ideal gas law: p·V = n·R·T.
p = n·R·T / V.
p = 0.098 mol · 0.08206 L·atm/mol·K · 300 K / 1.00 L.
p = 2.41 atm.
