Question

The density of ethane, c2h6 (30.1 g/mol), at 27°c and 1.27 atm pressure is ___. (r = 0.08206 l⋅atm/mol⋅k)

A) 1.11 g/L
B) 0.87 g/L
C) 1.35 g/L
D) 1.02 g/L

Answer 1

The density of ethane (C2H6) at 27°C and 1.27 atm pressure was calculated using the ideal gas law; however, the result obtained (1.553 g/L) is not among the provided options, suggesting there may be a calculation error or a misunderstanding in the given values or question.

Step-by-step explanation:

The question asks for the density of ethane (C2H6) at a specific temperature and pressure. We can use the ideal gas law to find the molar volume and then calculate the density by taking the molar mass into account. The ideal gas law is given by PV = nRT, where:

• P is the pressure,
• V is the volume,
• n is the number of moles,
• R is the ideal gas constant,
• T is the temperature in Kelvin.

First, we convert the temperature from Celsius to Kelvin: T = 27°C + 273 = 300K. Then, we solve the ideal gas law for the volume (V) when n = 1 mole:

V = (nRT)/P

Then calculate the density (ρ) using the molar mass (M) of ethane: ρ = M/V

Using the provided values:

V = (1 mole * 0.08206 L·atm/mol·K * 300K) / 1.27 atm = 19.38 L

Then, ρ = 30.1 g/mol / 19.38 L/mol = 1.553 g/L, which is not one of the provided options, indicating a possible mistake in calculation or misunderstanding of the question's conditions.