3. The Russian Mir space station used a chemical oxygen generator system to make oxygen for the crew. The system ignited a tube of solid lithium perchlorate (LiClO4) to make oxygen and lithium chloride (LiCl):
LiClO4 (s)  2O2 (g) + LiCl (s)
If you have 500 g of LiClO4, then how many liters of oxygen will the system make at the station’s standard operating conditions, a pressure of 101.5 kPa and a temperature of 21°C? (Show the steps involved in your work.)
Answer:

Question

3.	The Russian Mir space station used a chemical oxygen generator system to make oxygen for the crew. The system ignited a tube of solid lithium perchlorate (LiClO4) to make oxygen and lithium chloride (LiCl):
LiClO4 (s)  2O2 (g) + LiCl (s)
If you have 500 g of LiClO4, then how many liters of oxygen will the system make at the station’s standard operating conditions, a pressure of 101.5 kPa and a temperature of 21°C? (Show the steps involved in your work.)
Answer:

wolfe8 · Answer

Can you find the number of moles O2 produced first?

anonymous · Answer

@wolfe8  i got the answer to that one can you help me with this one please?

1.	A mountain biker goes for a ride in the desert. The air temperature is 21°C at the start of the ride, but the temperature in the desert will reach a peak of 51°C. The tires on the bike 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 the peak temperature in the desert?
•	Will the tires burst at the peak temperature? Explain.
•	To what pressure should the tire pressure be reduced before starting the ride to avoid bursting of the tires in the desert heat? (Assume no significant change in tire volume.)
Answer:

wolfe8 · Answer

Use the formula PV=nRT where n is the number of moles.