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:

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:

First, you need a balanced equation:

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

Are you sure your reaction is correct?

2NO \rightarrow N_2O\,\,\,??

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.

2NO \rightarrow N_2O + \frac 12 O_2