Question

At 15°C and 900 mm pressure, 0.4 gram of a certain gas
occupied 3280 mL. If the pressure is changed to 1300 mm at constant temperature. What is the density of the gas?​

Answer 1

Answer:

Density of the gas = 0.2172 g/L

Explanation:

As per given information, at 15°C,900 mm pressure 0.4 gram of gas occupied 3280 ml

As per ideal gas equation

PV = nRT

Where n = mass / molar mass of gas

P = mass / molar mass of gas x RT/V

Mass = Density x Volume

Inserting the formula of mass;

P = density  / molar mass of gas x RT

We are given that temp = 15°C (15+273); pressure = 1300 nm; molar mass = 0.4 g; and R = 8.314

Putting the values in above formula to calculate density, we get

Density of the gas = 0.2172 g/L

Answer 2

Answer:

1.762 × 10⁻⁴ g / mL

Explanation:

We know :

Density = Mass / Volume

= > Density at 900 mm pressure = 0.5 / 3280 g / mL = 0.000122 g / mL

At constant temperature :

= > Density × Pressure

d₁ / P₁ = d₂ / P₂

= > d₂ = ( d₁ P₂ ) / P₁

We have values of :

d₁ = 0.00012 g / mL

P₁ = 900 mm

P₂ = 1300 mm

Putting values in d₂ :

d₂ = ( 0.000122 × 1300 ) / 900

= > d₂ = ( 0.000122 × 13 ) / 9

= > d₂ = 0.0001762 g / mL

= > d₂ = 1.762 × 10⁻⁴ g / mL

Hence we get required answer.