Question

Leon uses a pressure gauge to measure the air pressure in one of his car tires. The gauge shows that the pressure is 220 kilopascals. The temperature is 297 K, and the outdoor air is at standard pressure. If the tire contains 4.8 moles of air, what is the volume of the tire? The volume of the car tire is __ liters.

Answer 1

53.8 L

Step-by-step explanation:

Ideal gas law

PV=nRT

must be for volume so we arrange to V=nRT/P

V= (4.8)(8.31)(297)/220

Answer 2

The volume of the car tire is 53.93 Liters.

Step-by-step explanation:

Pressure of the gas in car tire =
`P=220kPa=2.17 atm`

(1 kPa = 0.009869 atm)

Temperature of the gas in tire =T = 297 K

Moles of air in the tire = n = 4.8 moles

Volume of the gas in the tire= V

Using an ideal gas equation:

`PV=nRT`

`V=(nRT)/(P)=(4.8 mol* 0.0821 atm L/mol K* 297 K)/(2.17 atm)`

V = 53.93 L

The volume of the car tire is 53.93 Liters.