Question

A scientist wishes to compress 50.0 ml of ammonia gas at normal atmospheric pressure to a volume of 1.0 ml. What pressure in atmospheres is necessary

Answer 1

Using Law: PV = nRT we can calculate P (pressure)

But this law becomes P₁V₁/T₁ = P₂V₂/T₂ for one compound under different conditions

T₁ = T₂ = const, so P₁V₁ = P₂V₂

P₁ = 1 atm (STP), so P₂ = P₁V₁/V₂ = 1*50.0/1.0 = 50 atm