Final answer:
To find the density of oxygen gas at 5.0 atm and 27°C, we can use the Ideal Gas Law equation. The density is approximately 6.5 g/L.
Step-by-step explanation:
To find the density of oxygen gas at 5.0 atm and 27°C, we can use the Ideal Gas Law equation:
Density = (molar mass of oxygen)/(molar volume)
First, we need to calculate the molar volume of oxygen at the given conditions. The molar volume (V) can be found using the equation:
V = (R*T)/(P)
Where R is the ideal gas constant (0.08206 L·atm/mol·K), T is the temperature in Kelvin (27+273 = 300 K), and P is the pressure in atm (5.0 atm). Substitute the values into the equation: V = (0.08206 L·atm/mol·K * 300 K)/(5.0 atm) = 4.9236 L/mol.
Next, we need to calculate the molar mass of oxygen, which is 32 g/mol.
Finally, substitute the molar mass and molar volume into the density equation:
Density = 32 g/mol / 4.9236 L/mol ≈ 6.5 g/L