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

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

the answer is minerals.