Avolleyball is full of pressurized air. the air temperature is 24.6 degrees c. the volleyballs absolute pressure is 140.75 kilopascals and it’s volume is 5.27 liters. how many miles of air are inside the volleyball

0.300 mol  

Step-by-step explanation:

We can use the Ideal Gas Law to solve this problem.

pV = nRT     Divide both sides by RT

n = (pV)/(RT)

Data:

p = 140.75 kPa

V = 5.27 L

R = 8.314 kPa·L·K⁻¹mol⁻¹

T = 24.6 °C

Calculations:

(a) Convert temperature to kelvins

T = (24.6 + 273.15) K = 297.75 K

(b) Calculate the number of moles

n = (140.75 × 5.27)/(8.314 × 297.75)

  = 0.300 mol

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b