A ball has a volume of 5.27 liters and is at a temperature of 27.0C. A pressure gauge attached to the ball reads 0.25 atmosphere. The atmospheric pressure is 1.00 atmosphere. Calculate the absolute pressure inside he ball and the amount of air it contains

The absolute pressure inside the ball is

1.25

atmospheres.

The ball contains

0.267

mole of air.

Explanation:

The absolute pressure is the sum of the gauge pressure and the atmospheric pressure.

The ball has an absolute pressure of 1.25 atmospheres:

0.25 atm + 1.00 atm = 1.25 atm.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

the answer for sodium is 0.186

the answer for rubidium is 0.251