## Lena772 one year ago The reaction below was observed in a 4.0 L flask at 100oC. N2O4 (g) ↔ 2 NO2(g) Initially, 0.2 mol of N2O4 and 0.2 mol of NO2 were placed in the flask. If the kp = 11 atm , will the reaction proceed toward products or reactants? Toward reactants Toward products It's at equilibrium

1. Lena772

I tried towards reactants and that was wrong... Maybe it's equilibrium?

2. Lena772

@Photon336

3. Abhisar

You can calculate molar concentrations of each of them and then find $$\sf Q_c$$. Compare it with $$\sf K_c$$. If $$\sf Q_c>K_c$$ then reaction will be backwards or forward otherwise. You can find $$\sf K_c$$ by using the equation $$\sf K_p = K_c \times (RT)^{\Delta n}$$

4. Photon336

agree with abhisar, you can figure out Qc which is relatively easy $Qc = \frac{ [NO_{2}]^{2} }{ [N_{2}O_{4}] } = [0.05M]^{2}/[0.05] = 1$ However as abhisar said you would need to convert Kp and compare it to Kc then this would tell you what direction the reaction is going.

5. Lena772

Qc=1 Kc=0.359 1>0.359 so backwards. Wouldn't that mean more reactants are formed? :/ @Abhisar @Photon336

6. Photon336

So technically we know that Qc = 1 so 0.359 is the value of Kc right? Right away because Qc and Kc are not equal you know that the reaction has not reached equilibrium or should I say at equilibrium. so if Q>K that means that there are too many products, so the equilibrium will shift to form more reactants until the Q = K and equilibrium is established.

7. Lena772

Thank you! @Photon336

8. Photon336

No problem