Answer:
2.84g of O₂ / L
Explanation:
Density is defined as the ratio between mass of substance per unit of volume.
Using ideal gas law, PV = nRT (Where P is pressure in atm, V is volume in L, n are moles, T is gas constant 0.082atmL/molK and T is absolute temperature.
70.0°C are 273.15 + 70.0 = 343.15K. Replacing:
[tex]\frac{P}{RT} = \frac{n}{V}[/tex]
[tex]\frac{2.50atm}{0.082atmL/molK*343.15K} = \frac{n}{V}[/tex]
0.0888mol / L = n/V.
Using molar mass of O₂ -32g/mol-:
0.0888 mol/L × (32g / mol) = 2.84g of O₂ / L - The density of the gas-
The density of the oxygen gas at 70[tex]\rm ^\circ C[/tex], and 2.50 atm is 2.84 g/L.
The moles of oxygen per L can be calculated by the ideal gas equation.
PV = nRT
P = pressure = 2.50 atm
n = moles
V = volume
R = constant = 0.0821
T = temperature = 70[tex]\rm ^\circ C[/tex] = 343.15 K
Substituting the values:
[tex]\rm \dfrac{n}{V}\;=\;\dfrac{2.5}{0.0821\;\times\;343.15}[/tex]
moles per liter = 0.08 moles/L.
weight/liter can give density.
The weight can be obtained by multiplying the moles with the molecular weight.
Molecular weight of oxygen gas = 32 g/mol
Weight/ Liter of Oxygen gas = 0.08 mole/L [tex]\times[/tex] 32 g/mol
Weight/ Liter of Oxygen gas = 2.84 g/L.
Thus, the density of the oxygen gas at 70[tex]\rm ^\circ C[/tex], and 2.50 atm is 2.84 g/L.
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