At 1250 mmhg and 750c, the volume of a sample of ammonia gas is 6.8 l. what volume would the ammonia occupy at stp?

V₂ = 3 L

Explanation:

Given data:

Initial volume = 6.8 L

Initial pressure = 1250 mmHg (1250/760 =1.64 atm)

Initial temperature = 750°C (750 +273 = 1023 K)

Final temperature = 273 K

Final volume = ?

Final pressure = 1 atm

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 1.64 atm × 6.8 L × 273 K / 1023 K × 1 atm

V₂ = 3044.5 atm .L. K / 1023 K. atm

V₂ = 3 L

a chemical reaction happens

explanation:

sry but any answer choices