Question

1. On a summer day, you take a road trip through Death Valley, California, in an antique car. You start out at a temperature of 21°C, but the temperature in Death Valley will reach a peak of 51°C. The tires on your car hold 15.6 L of nitrogen gas at a starting pressure of 249 kPa. The tires will burst when the internal pressure (Pb) reaches 269 kPa.

Answer 1

How many moles of nitrogen gas are in each tire?
• What will the tire pressure be at peak temperature in Death Valley?
• Will the tires burst in Death Valley? Explain.
• If you must let nitrogen

Answer 2

• If you must let nitrogen gas out of the tire before you go, to what pressure must you reduce the tires before you start your trip? (Assume no significant change in tire volume.)

Answer 3

PV=nRT -> You have Pi (initial), Vi, Ti and R so you should solve for n
n=(PV)/(RT)

Answer 4

...what? I'm honestly so confused

Answer 5

If you assume R and n to be constant (which you can) then you will use:
\[P _{1}V _{1}/T _{1_{}}=P _{2}V _{2}/T _{2}\]

Answer 6

Ok. Temp, pressure, volume and moles are related through the ideal gas law.
PV=nRT

Answer 7

In this problem you are given 2 different states of pressure, temp, and volume. 1st starting temp 21C and starting pressure 249 kPa.

Answer 8

oh and the volume of 15.6 L. You can use those 3 values in the ideal gas law to solve for n, the number of moles.

Answer 9

...so do I plug them in or something?

Answer 10

\[PV=nRT\]
\[n=PV/RT\]
\[n=\frac{ 249 kPa x 15.6 L }{ (21+273)K *R }\]

Answer 11

x is suppose to be (times) not a variable

Answer 12

You will have to look up the value of R that matches your units

Answer 13

I hope that helps!