Chemistry, please help!!

This one's data is different than the others, so actually read it and if you don't have a real answer, don't answer.

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 56°C. The tires on your car hold 13.2 L of nitrogen gas at a starting pressure of 240 kPa. The tires will burst when the internal pressure (Pb) reaches 262 kPa. Answer the following questions and show your work.
• 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 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.)