A student is working with a 4.95 L sample of carbon dioxide at 22.8°C and 0.956 atm. The student compresses the gas to 1.75 L and increases the temperature of the gas to 65.3°C. What will the resulting pressure of the CO 2 gas be after the student made these changes?

The resulting pressure is 3.093 atm

calculation

The resulting pressure is calculated using the combined gas equation

That is P₁V₁/T₁ = P₂V₂/T₂ where,

P₁=0.956 atm

V₁=4.95 L

T₁=22.8 c in to kelvin = 22.8 + 273 = 295.8 k

P₂=? atm

V₂=1.75 L

T₂=65.3 c into kelvin = 65.3 + 273 = 338.3 K

make P₂ the subject of the formula by multiplying both side of the formula by T₂/V₂

P₂ = T₂P₁V₁ / V₂T₁

P₂ = [ (338.3 k x 0.956 atm x 4.95 L) / (1.75 L x 295.8 K) ] = 3.093 atm