What is the calculated density of ethane C2H6, at 25oC and 1.10 atm? 1.15 g/L 1.30 g/L 1.25 g/L 1.20 g/L 1.35 g/L

To calculate the density of a gas, we can use the ideal gas law, which is PV = nRT. However, we need to rearrange it to solve for density (ρ). Density is mass/volume, and we know that the number of moles (n) is mass (m) divided by molar mass (M). So, we can rewrite the equation as follows:

ρ = PM/RT

Where: P is the pressure, M is the molar mass, R is the ideal gas constant, and T is the temperature in Kelvin.

Given: P = 1.10 atm, M (molar mass of C2H6) = 30.07 g/mol, R (ideal gas constant) = 0.0821 L.atm/mol.K, and T = 25°C = 298.15 K (remember to always convert Celsius to Kelvin in gas law problems).

Substituting these values into the equation gives:

ρ = (1.10 atm * 30.07 g/mol) / (0.0821 L.atm/mol.K * 298.15 K)

Solving this gives a density of approximately 1.30 g/L. So, the calculated density of ethane C2H6 at 25°C and 1.10 atm is 1.30 g/L.