A sample of ammonia gas is completely decomposed to nitrogen and hydrogen gases. If the total pressure is 866 mmHg, calculate the partial pressure of nitrogen. 2NH3(g) --> N2(g) + 3H2(g)

Question

A sample of ammonia gas is completely decomposed to nitrogen and hydrogen gases. If the total pressure is 866 mmHg, calculate the partial pressure of nitrogen. 2NH_3(g) --> N_2(g) + 3H_2(g)

Please show steps.

Answer 1

Write a correctly balanced equation: 2NH₃(g) ==> 3H₂(g) + N₂(g)

Partial pressure of a gas = mole fraction of that gas x total pressure

Total moles of gas = 1 mole N₂ + 3 moles H₂ = 4 moles

Mole fraction N₂ = 1 mole/4 moles = 0.25

Partial pressure N₂ gas = 0.25 x 866 mm Hg = 217 mm Hg