Answer:
139.9 g ≅ 140.0 g.
Step-by-step explanation:
- We can use the general law of ideal gas: PV = nRT.
where, P is the pressure of the gas in atm (P = 1.0 atm, standard P).
V is the volume of the gas in L (V = 98.0 L).
n is the no. of moles of the gas in mol (n = ??? mol).
R is the general gas constant (R = 0.0821 L.atm/mol.K),
T is the temperature of the gas in K (T = 273 K, standard T).
∴ n = PV/RT = (1.0 atm)((98.0 L)/(0.0821 L.atm/mol.K)(273 K) = 4.37 mol.
- To find the grams of O₂, we can use the relation:
n = mass/molar mass.
∴ mass of O₂ = (n)*(molar mass) = (4.37 mol)(32.0 g/mol) = 139.9 g ≅ 140.0 g.