Question

calculate the pressure exerted by 8.5 g of NH3 contained in 0.5 l vessel at 300 K . For NH3​

Answer 1

Given :

Mass of ammonia = 8.5 g

Volume of container = 0.5 L

Temperature = 300 K

To Find :

Pressure exerted by ammonia gas.

Solution :

❖ First of all we have to find moles of ammonia.

It is defined as the ratio of mass to the molar mass.

Molar mass of NH₃ = 17 g/mol

➠ n = W / Mw

➠ n = 8.5 / 17

➠ n = 0.5

Ideal gas equation is given by

$\dag\:\underline{\boxed{\bf{\orange{PV=nRT}}}}$

• P denotes pressure
• V denotes volume
• n denotes number of moles
• R denotes gas constant
• T denotes temperature

By substituting the given values;

$\sf:\implies\:PV=nRT$

$\sf:\implies\:P\times0.5=0.5\times0.082\times300$

$\sf:\implies\:P=0.082\times300$

$:\implies\:\underline{\boxed{\bf{\gray{P=24.6\:atm}}}}$

Answer 2

Given

Mass of ammonia = 8.5 g

Mass of ammonia = 8.5 gVolume of container = 0.5 l

To Find

Pressure exerted by ammonia gas

Solution

• First of all we have to find moles of ammonia.

It is defined as the ratio of mass to the molar mass.

Molar mass of NH₃ = 17 g/mol

• n = W / Mw

• n = 8.5 / 17

• n = 0.5

PV = nRT

By substituting the given values;

PV = nRT

P × 0.5 = 0.5 × 0.082 × 300

P = 0.082 × 300

P = 2.46 atm