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anonymous
 one year ago
How many moles of ethylene (C2H4) can react with 12.9 liters of oxygen gas at 1.2 atmospheres and 297 Kelvin?
C2H4(g) + 3O2(g) yields 2CO2(g) + 2H2O(g)
I have a test later today, please show me how to do this so I'll know what to do on the test. Thank you. :)
anonymous
 one year ago
How many moles of ethylene (C2H4) can react with 12.9 liters of oxygen gas at 1.2 atmospheres and 297 Kelvin? C2H4(g) + 3O2(g) yields 2CO2(g) + 2H2O(g) I have a test later today, please show me how to do this so I'll know what to do on the test. Thank you. :)

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sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0I'm pretty sure this is a PVNRT problem. Do you know the ideal gas law formula?

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0Okay, well the first thing you need to go is find out how many moles of Oxygen you have, using the ideal gas law formula

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0Can you show me how to do that?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I think so, one sec let me look

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I attempted it by plugging it into the formula before but I just don't think I got the right answer

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0You should know the formula if you have a test later :s but it's really easy to remember! It's PVNRT. Or PV = nRT where p = pressure (atm) v = volume (L) R = gas constant n = moles (mol) t = temperature (T)

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0So, use the values given in the problem to solve for n, which equals the number of moles of Oxygen gas. What value did you get?

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0Okay awesome. So there's 0.634 moles of Oxygen. Since you have a chemical equation and the moles of Oxygen, do you think you sort of know how to get to the moles of C2H4?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0That's where I get lost lol

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0That's okay. That's where most people get lost. So, at this point we have to use dimensional analysis. Just a fancy word of saying to get from one thing to another. My high school chem teacher used to call it trainandcaboose

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0You have to use the chemical equation to determine the ratio. So, for every 3 mol of Oxygen there's 1 mol of C2H4

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0dw:1440095235516:dw make sure to cross out your units

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Ok thank you, I'll try it :)

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0Okay! Practice makes perfect! Let me know if you have anymore questions

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Ok, sorry I'm really tired haha. How am I supposed to plug it in?

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0What do you mean? Can you clarify? Plug in what? Do you mean the ideal gas law formula or dimensional analysis?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0dimensional analysis

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0Oh okay, well that's a little different. The only way to really understand it is by doing practice problems, but I generally use this sort of thinking: dw:1440096529907:dw

sjg13e
 one year ago
Best ResponseYou've already chosen the best response.0heres a link that might help http://www.katmarsoftware.com/articles/railroadtrackunitconversion.htm

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Ohh I see, thank you so much
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