Question

7.25 moles of air are pumped into a car tire. At 80°C, the pressure inside the tire is 506.625

kPa. What is the volume of the tire?

Answer 1

To find the volume of the car tire, you can use the ideal gas law equation: V = nRT/P where V is the volume, n is the number of moles of air, R is the ideal gas constant, T is the temperature in Kelvin, and P is the pressure. In this case, the volume of the car tire is 21.52 liters.

Step-by-step explanation:

To find the volume of the car tire, we can use the ideal gas law equation:

V = nRT/P

where V is the volume, n is the number of moles of air, R is the ideal gas constant, T is the temperature in Kelvin, and P is the pressure. In this case, we are given the number of moles of air (7.25 moles), the temperature (80°C), and the pressure (506.625 kPa). We can convert the temperature to Kelvin by adding 273.15: 80 + 273.15 = 353.15 K. The ideal gas constant R is 8.314 J/(mol·K).

Now we can plug in the values to calculate the volume:

V = (7.25 mol * 8.314 J/(mol·K) * 353.15 K) / (506.625 kPa * 1000 J/kJ) = 21.52 L

Therefore, the volume of the car tire is 21.52 liters.

Answer 2

For this question you need to use the ideal gas equation PV = nRT.

P is pressure, V is volume, n is number of moles, R is molar gas constant (8.31J/mol*K) and T is temperature.

The temperature must be in Kelvin for this equation, 80°C in kelvin is (80 + 273.15) = 353.15K

We also want to convert the kPa into Pa so we times by 1000 giving us 506625Pa

Since we’re looking for volume we rearrange to make V the subject giving us V = nRT/P.

Now you just plug in the values, V = 7.25 * 8.31 * 353 / 506625 which will give us 0.042m^3.

Hope this helps