The density of O₂ gas at 16°C and 1.27 atm is A)31 g/L. B)28.4 g/L. C)1.71 g/L. D)88.7 g/mL. E)0.584 g/L.

Question

Quizplus · Accepted Answer

To calculate the density of the gas, we use the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature. Solving for n/V, we get: n/V = P/RT The molar mass of O₂ gas is needed to calculate the density. This is not provided in the question, so we cannot calculate the exact density. However, we can use the molar mass of air (approximately 28.8 g/mol) as an estimate. Using the given values and the ideal gas law: n/V = P/RT = (1.27 atm) / (0.0821 L·atm/mol·K * 289 K) = 0.0529 mol/L The density can be calculated by multiplying the molar mass by the number of moles per liter: density = (28.8 g/mol) * (0.0529 mol/L) = 1.52 g/L This is closest to choice C, 1.71 g/L.

The Density of O2 Gas at 16°C and 1

The Density of O₂ Gas at 16°C and 1