Question

A 2.35 g sample of an unknown gas at 55 ∘C and 1.05 atm is stored in a 1.85 L flask.

Answer 1

Answer:

Molar mass =  32.64 g / mol.

The density of gas is 1.3 × 10⁻³g/mL.

Explanation:

Given data:

Mass of sample = 2.35 g

Pressure = 1.05 atm

Volume = 1.85 L    (1.85 × 1000 = 1850 ml)

Temperature = 55 °C    (55+ 273.15 = 328.15 K)

Density = ?

Formula:

d = m/ v

The volume of flask would be the volume of gas.

d = 2.35 g / 1850 mL = 0.0013 g/mL or 1.3 × 10⁻³g/mL

The density of gas is 1.3 × 10⁻³g/mL.

Molar mass:

Now we will calculate the moles of a gas first in order to find the molar mass of a gas.

Formula:

PV =nRT

n = number of moles.

n = PV / RT

n = 1.05 atm × 1.85 L / 0.0821 atm. dm³. K⁻¹ . mol⁻¹ × 328.15 K

n = 1.9425 atm . L / 26.941115 atm . dm.³mol⁻¹

n = 0.072 mol

Now we will find the molar mass.

Number of moles = mass / molar mass

0.072 mol = 2.35 g / molar mass

Molar mass = 2.35 g / 0.072 mol

Molar mass =  32.64 g / mol

Answer 2

The density of the gas and molar mass is 1.35 g/mol and 0.104 mol

Explanation:

The molar mass of a chemical compound is defined as the mass of a sample of that compound divided by the amount of substance in that sample, measured in moles.

A chemical compound is the chemical substance composed of many identical molecules composed of atoms more than one element held together by chemical bonds.

The gas molar volume is the volume of one mole of the gas at a given temperature and pressure

$PV = nRT$ to determine

$(1.10 atm) (2.55 L) = (n) (0.08206) (328 K)$

$n = 0.104 mol$

The molecular weight (molar mass) is the mass of one particle of that gas multiplied by Avogadro's number which is the number of constituent particles that contained in one mole

$0.104 mol * M g/mol = 3.45g$

$M = 3.45 g / 0.104 mol = 33.17 g/mol\\Density = Molar Mass x \frac{P}{RT} \\ = 33.17 g/mol * 1.10 atm / 0.0821 L mol / atm .K * 328 K\\= 1.35 g$

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