# Chemistry Question?

A bicycle pump inflates a tire whose volume is 535 mL until its internal pressure is 6.18 bar at a temperature of 24.6 oC.

How many moles of air does the tire contain?

What volume of air (in L) at 1.01 bar and 24.6 oC did the pump transfer?

### 2 Answers

- electron1Lv 71 year agoFavorite Answer
What volume of air (in L) at 1.01 bar and 24.6 oC did the pump transfer?

Since the temperature is constant, we can use the following equation to solve this problem.

P1 * V1 = P2 * V2

6.18 * 535 = 1.01 * V2

V2 = 3,306.3 ÷ 1.01

The new volume is approximately 3,274 ml.

To determine the number of moles of air, use the following equation.

P * V = n * R * T

The unit of pressure is atmospheres. One bar of pressure is 1 * 10^5 Pa. This is standard pressure.

P = 6.18 * 10^5 Pa

The volume must be in liters.

V = 0.535

R = 22.4 ÷ 273

Let’s convert the temperature from˚C to ˚K.

T = 24.6 + 273 = 297.6˚K

Now we can determine the number of moles of oxygen.

P * V = n * R * T

6.18 * 10^5 * 0.535 = n * (22.4 ÷ 273) * 297.6

n * 6666.4 = 9.026199 * 10^7

n = 9.026199 * 10^7 ÷6666.4

The number of moles of oxygen is approximately 1.36 * 10^4. I hope this is helpful for you.

- Login to reply the answers

- hcbiochemLv 71 year ago
P1V1 = P2V2

535 mL (6.18 bar) = V2 (1.01 bar)

V2 = 3274 mL or better 3.27 L

- Login to reply the answers