Calculate the density, in g/L, of CO₂ gas at 27°C and 0.50 atm pressure. A)0.89 g/L B)1.12 g/L C)9.93 g/L D)46.0 g/L E)2.17 kg/L

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve for the density of the gas:
PV = nRT
where P = pressure, V = volume, n = moles, R = gas constant, and T = temperature.

We are given the pressure (0.50 atm) and temperature (27°C), but we do not have the volume or the number of moles. However, we can rearrange the equation to solve for density:

PV = nRT
n/V = P/RT
density = (mass of gas) / (volume of gas) = (n x molar mass) / V
mass of gas = n x molar mass

Substituting the expression for n/V from above, we get:

density = (P x molar mass) / (RT)

We can look up the molar mass of COS (carbonyl sulfide) as 60.07 g/mol. We convert the temperature to Kelvin by adding 273.15:

density = (0.50 atm x 60.07 g/mol) / ((0.08206 L·atm/(mol·K)) x 300 K) = 0.89 g/L

Therefore, the answer is A) 0.89 g/L.

Calculate the Density, in G/L, of CO2 Gas at 27°C

Calculate the Density, in G/L, of CO₂ Gas at 27°C