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?

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 = mass / molar

Mole of CO₂ = 1.95 / 44

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 = mole × molar mass

Mass of C₂H₆ = 0.0443 × 30

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

Learn more: link

1.332 g.

Explanation:

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.

∴ (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.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm