A1.54l gas bulb in a chemistry laboratory contains oxygen gas at 21 degrees c and 758 torr. the air conditioning in the laboratory breaks down ( 's morehouse) and the temperature rises to 31 degrees. calculate the final pressure of the gas given this increase in temperature

784 torr

Explanation:

Using  Pressure Law; at constant volume,

P∝ T at constant volume.

P= kT ; meaning

P1/T1 = P2/T2

P1= 758 torr

P2= ?

T1= 21 ° C or (273+21)K

   = 294°K

T2= 31 ° C or (273+31)K

    =  304°K

Substituting into equation (1),

We have:

758/294 = P2/304

P2 = 758 x 304/294

    =   783.78torr

    ≈ 784 torr

c, liquids evaporate, creating a gas