The recommended air pressure of a car tire is 32.0 psi (221 kPa). An average tire holds
around 1 mole of gas. What is the volume of the tire at 32°C?

The answer to your question is Volume = 11.47 L

Explanation:

Data

Pressure = 221 kPa

Temperature = 32°C

moles = 1

Volume = ?

R = 0.082 atm L / mol°K

Process

1.- Convert pressure to atm

Pressure = 221 kPa = 221000 Pa

                      1 atm 101325 Pa

                      x          221000 Pa

                      x = (221000 x 1) / 101325

                      x = 2.18 atm

2.- Convert temperature to °K

°K = 32 + 273

   = 305°

3.- Substitution

                PV = nRT

- Solve for V

                V = nRT / P

- Substitution

                V = (1)(0.082)(305) / 2.18

- Result

                V = 11.47 L

The volume of the tire is 11.5 L

Explanation:

Step 1: Data given

Pressure of the car tire = 221 kPa = 2.1811 atm

Number of moles gas = 1.0 mol

Temperature = 32.0 °C

Step 2: Calculate the volume

p*V = n*R*T

⇒ with p = the pressure = 2.1811 atm

⇒ with V = the volume of the tire = TO BE DETERMINED

⇒ with n= The number of moles gas = 1 mol

⇒ with R = the gas constant = 0.08206 L*atm/mol*K

⇒ with T = the temperature = 305 K

V = (n*R*T) / p

V = (1.0 * 0.08206 * 305 ) / 2.1811 atm

V = 11.5 L

The volume of the tire is 11.5 L

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