Question

At a certain temperature and pressure, one liter of CO2 gas weighs 1.95 g.

What is the mass of one liter of C2H6 gas at the same temperature and pressure?

Answer 1

Answer:

1.332 g.

Explanation:

• We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.

• At the same T and P and constant V (1.0 L), different gases have the same no. of moles (n):

∴ (n) of CO₂ = (n) of C₂H₆

∵ n = mass/molar mass

∴ (mass/molar mass) of CO₂ = (mass/molar mass) of C₂H₆

mass of CO₂ = 1.95 g, molar mass of CO₂ = 44.01 g/mol.

mass of C₂H₆ = ??? g, molar mass of C₂H₆ = 30.07 g/mol.

∴ mass of C₂H₆ = [(mass/molar mass) of CO₂]*(molar mass) of C₂H₆ = [(1.95 g / 44.01 g/mol)] * (30.07 g/mol) = 1.332 g.

Answer 2

The mass of 1 L of C₂H₆ at the same temperature and pressure with 1 L of CO₂ gas is 1.33 g

From the ideal gas, we understood that the same temperature and pressure different gases have the same number of mole.

From the above statement, we can say that 1.95 g of CO₂ will have the same number of mole as C₂H₆.

Now, we shall obtain the number of mole in 1.95 g of CO₂. This can be obtained as follow:

Mass of CO₂ = 1.95 g

Molar mass of CO₂ = 12 + (2×16) = 44 g/mol

Mole of CO₂ =?

Mole = mass / molar

Mole of CO₂ = 1.95 / 44

Mole of CO₂ = 0.0443 mole

Finally, we shall determine the mass of C₂H₆ at the same temperature and pressure with CO₂

Mole of C₂H₆ = Mole of CO₂ = 0.0443 mole

Molar mass of C₂H₆ = (12×2) +(1×6) = 30 g/

Mass of C₂H₆ =?

Mass = mole × molar mass

Mass of C₂H₆ = 0.0443 × 30

Mass of C₂H₆ = 1.33 g

Therefore, the mass of 1 L of C₂H₆ at the same temperature and pressure with 1 L of CO₂ gas is 1.33 g

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