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2 years ago

I NEED HELP ASAP! PLEASE BE GENUINE

Chemistry

1 answer:

love history [14]2 years ago

6 0

1. The molar mass of the unknown gas obtained is 0.096 g/mol

2. The pressure of the oxygen gas in the tank is 1.524 atm

<h3>Graham's law of diffusion </h3>

This states that the rate of diffusion of a gas is inversely proportional to the square root of the molar mass i.e

R ∝ 1/ √M

R₁/R₂ = √(M₂/M₁)

<h3>1. How to determine the molar mass of the gas </h3>

Rate of unknown gas (R₁) = 11.1 mins
Rate of H₂ (R₂) = 2.42 mins
Molar mass of H₂ (M₂) = 2.02 g/mol

Molar mass of unknown gas (M₁) =?

R₁/R₂ = √(M₂/M₁)

11.1 / 2.42 = √(2.02 / M₁)

Square both side

(11.1 / 2.42)² = 2.02 / M₁

Cross multiply

(11.1 / 2.42)² × M₁ = 2.02

Divide both side by (11.1 / 2.42)²

M₁ = 2.02 / (11.1 / 2.42)²

M₁ = 0.096 g/mol

<h3>2. How to determine the pressure of O₂</h3>

From the question given above, the following data were obtained:

Volume (V) = 438 L
Mass of O₂ = 0.885 kg = 885 g
Molar mass of O₂ = 32 g/mol
Mole of of O₂ (n) = 885 / 32 = 27.65625 moles
Temperature (T) = 21 °C = 21 + 273 = 294 K
Gas constant (R) = 0.0821 atm.L/Kmol

Pressure (P) =?

The pressure of the gas can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

Divide both side by V

P = nRT / V

P = (27.65625 × 0.0821 × 294) / 438

P = 1.524 atm

Learn more about Graham's law of diffusion:

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Learn more about ideal gas equation:

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