A gas occupies 3.00 L at 1.50 atm and 25.0 °C. If the pressure is increased to 2.50 atm, and
the temperature is increased to 35.0°C, what
will be the final volume?

V₂ = 1.86 L

Explanation:

Given data:

Initial temperature = 25.0°C (25+273 = 298 k)

Initial volume = 3.00 L

Initial pressure = 1.50 atm

Final pressure = 2.50 atm

Final temperature = 35.0°C (35+273 = 308K)

Final volume = ?

Solution:

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

By putting values,

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 1.50 atm × 3.00 L × 308 K / 298 K × 2.50 atm

V₂ = 1386 atm .L. K / 745  K.atm

V₂ = 1.86 L

answer; i believe that the correct answer is (a) potassium(k)