Posted by jemy on Thursday, July 8, 2010 at 6:12pm.
I NEED ANSWER PLEAS
I would approach the problem this way.
You know equilibrium moles O2 = .7 which means 0.3 mole O2 was used. Then mole NO2 formed must be 2 x 0.3 = 0.6 and moles NO must be 1-0.6 = 0.4.
Total moles = moles NO + moles O2 + moles NO2.
mole fraction O2, for example = moles O2/total moles.
Then partial pressure O2 = mole fraction O2 x total pressure.
The NO and NO2 are done the same way.
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