At 298 K, Kc for N2O (g) <---- 2NO (g) is 5. 98 x 10 -3. How many moles of NO2 are in equilibrium with 0.25 mole N2O4 in a 475 mL flask?

I need the answer.I don't know what to do.:confused:

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Originally Posted by baby_me

At 298 K, Kc for N2O (g) <---- 2NO (g) is 5. 98 x 10 -3. How many moles of NO2 are in equilibrium with 0.25 mole N2O4 in a 475 mL flask?

i need the answer.I don't know what to do.:confused:

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First, you need a balanced equation:

Second, using that equation, you write down the definition of Kc

Are you sure your reaction is correct?



You have to reduce the NO to nitrous oxide, N2O. While that's definitely feasible, I'd be afraid it would decompose to nitrogen and oxygen first.