500. ml of gas is contained at stp. the volume changes to 560 ml at 20.°c
what is the pressure (in atm)?

P₂ = 0.96 atm

Explanation:

Given data:

Initial volume = 500 mL

Initial pressure = 1 atm

Initial temperature = 273 K

Final volume = 560 mL

Final temperature = 20°C (20+ 273 = 293K)

Final pressure = ?

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

According to general gas equation:

P₁V₁/T₁ = P₂V₂/T₂

P₂ = P₁V₁ T₂/ T₁ V₂  

P₂ = 1 atm × 500 mL × 293 K / 273 K × 560 mL  

P₂ = 146500 atm .mL. K /  152880 k.mL

P₂ = 0.96 atm

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .