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 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 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 1

3. Propane gas (C3H8) burns completely in the presence of oxygen gas (O2) to yield carbon dioxide gas (CO2) and water vapor (H2O).
Write a balanced equation for this reaction.
Assuming that all volume measurements occur at the same temperature and pressure, how many liters of oxygen will be required to completely burn 0.700 L of propane gas?
Assuming that all volume measurements occur at the same temperature and pressure, how many liters of carbon dioxide gas will be produced in the reaction?
Assuming that all volume measurements occur at the same temperature and pressure, how many liters of water vapor will be produced in the reaction

Answer 2

I really need help with these two questions!

Answer 3

Use PV=nRT