Question

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?

Answer 1

 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