I'm having trouble working out this homework problem:
I have oxygen at 35 degrees Celcius, and the pressure shown on the mercury barometer is 760 mm Hg. How much of this do I need to burn 227 grams of ethanol?
I think what you do is convert the mm Hg into atm, then plug these values into PV = nRT?
I'm not totally sure, thanks!
I have oxygen at 35 degrees Celcius, and the pressure shown on the mercury barometer is 760 mm Hg. How much of this do I need to burn 227 grams of ethanol?
I think what you do is convert the mm Hg into atm, then plug these values into PV = nRT?
I'm not totally sure, thanks!
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yah, u do
PV=nRT
so
find the amount of ethanol in mols
then set the equation of the reaction to find the mol ratio
then put the amount of oxygen in mols in the formula derived from PV=nRT
as V=mols of oxygen that u just found times .08206 times (35+273)/(1atm)
to get the amount of oxygen in L
PV=nRT
so
find the amount of ethanol in mols
then set the equation of the reaction to find the mol ratio
then put the amount of oxygen in mols in the formula derived from PV=nRT
as V=mols of oxygen that u just found times .08206 times (35+273)/(1atm)
to get the amount of oxygen in L
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Yes?