Larisa pumps up a soccer ball until it has a gauge pressure of 61 kilopascals. the volume of the ball is 5.2 liters. the air temperature is 32°c, and the outside air is at standard pressure. how many moles of air are in the ball?

a.
0.13 mol
b.
0.33 mol
c.
1.2 mol
d.
3.2 mol

B.  0.33 mol

We are given;

Gauge pressure, P = 61 kPa (but 1 atm = 101.325 kPa)

                               = 0.602 atm

Volume, V = 5.2 liters

Temperature, T = 32°C, but K = °C + 273.15

thus, T = 305.15 K

We are required to determine the number of moles of air.

We are going to use the concept of ideal gas equation.

       We know atmospheric pressure is 101.325 kPa or 1 atm

Total ball pressure = 1 atm + 0.602 atm

                               = 1.602 atm

That is;

PV = nRT

n = PV ÷ RT

therefore;

n = (1.602 atm× 5.2 L) ÷ (0.082057 × 305.15 K)

  = 0.3326 moles

  = 0.33 moles

Therefore, there are 0.33 moles of air in the ball.

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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