Imagine that you have a 6.50L gas tank and a 2.00 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 125atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases.
This is a question in which you need to make use of the ideal gas law, pv = nrT (where p = pressure, v = volume, n = number of moles of gas, t = temperature, and r = the idealgas contant = some crazy number that I can't remember, but is the same for every gas). If no temperature is specified, assume is it room temperature.
As far as trying to figure out how many moles of each, I would suggest using a ratio of the number of moles you need of each gas for the reaction to take place. You just need to make sure that your reaction is a balanced equation. It appears the equation you have is already balanced, so you would need 2 moles of C2H2 for every 5 moles of O2.
It tells you what pressure you need to fill the O2 tank to, as well as the volume of that tank. Solve the pv=nrT equation for n to find out how many moles of O2 gas you have in the tank at that pressure. Then take this number and use you ratio from above to find out how many moles of the C2H2 gas you need to have in the second tank. You should treat the ratio as an equivalence factor, thus making your units of # moles O2 cancel out during your calculations, leaving your result to be # moles C2H2.
Use the other tank's volume and solve the pv=nrT equation for pressure. Barring any math errors, this should be your final answer.
Sorry about not giving you the answer, but I am a teaching assistant for chemistry labs at my university, so I cannot in good concience give you the answer. But if you follow the method above, you should be able to solve this qusetion, as well as any that are similar to it. Good luck!
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