Posted by **Anonymous** on Saturday, February 12, 2011 at 10:55pm.

When N2O5 (g) is heated it dissociates into N2O3 (g) and O2 (g) according to the following reaction: N2O5 (g) <--> N2O3 (g) + O2 (g) Kc=7.75 at a given temperature. The N2O3 (g) dissociates to give N2O (g) and O2 (g) according the following reaction: N2O3 (g) <--> N2O (g) + O2 (g) Kc= 4.00 at the same temperature. When 4.00 mol of N2O5 (g) is heated in a 1.00-L reaction vessel to this temperature, the concentration of O2 (g) at equilibrium is 4.50 mol/L.

a) Find the concentration of N2O5 in the equilibrium system.

b) Find the concentration of N2O in the equilibrium system.

c) Find the concentration of N2O3 in the equilibrium system.

- chemistry -
**DrBob222**, Sunday, February 13, 2011 at 6:17pm
Get a second opinion on this AND check my thinking..

N2O5 ==> N2O3 + O2

N2O3 ==> N2O + O2

Add the two equations to obtain

N2O5 ==> N2O + 2O2 and k for this reaction is k1*k2 = 7.75*4 = 31.0 = (N2O)(O2)/(N2O5).

The final O2 is 4.5 moles; some came from reaction 1 and some from reaction 2. How much came from each. If we call x the amount from 1, then 4.00/7.75 must have come from rxn 2 or

1+(4.00/7.75) = 4.5 and x = 2.97

The amount from rxn 2 then must be 2.97*(4.00/7.75) = 1.53 (total is still 4.50).

From rxn 2,

N2O3 ==> N2O + O2

If O2 from this rxn is 1.53, that means N2O must be 1/2 that or 0.765 (that is part (c)). From

4.00 = (N2O)(O2)/(N2O3), we solve for N2O3 (substitute 4.5 for O2 because the O2 in the final mixture can't tell where it came from and we know the total is 4.5). That gets part(b).

For part a, concn N2O5 at equilibrium, use K1K2 = 31.0 = (N2O3)(O2)/(N2O5)

You know N2O3 and O2.

Just to check things, if we substitute the values I obtained for N2O3 (0.861) and 4.5 for O2 and 0.500 for N2O5, K1 gives 7.75 which was K in the problem. Again, get a second opinion and check my thinking.

- chemistry -
**Nika**, Tuesday, February 15, 2011 at 2:08am
Hi, I'm doing the same assignment. I got to the part where you added the reactions and got the K3 = 31. Then, I got stuck

I don't understand why you're doing the 4.00/7.75 and then stating that 1 +(4.00/7.75) = 4.5? isn't that 1.52 instead of 4.5?

## Answer This Question

## Related Questions

- Chemistry - For the reaction NO2(g) + NO(g) = N2O3(g) If at particular ...
- Chemistry12 - For the reaction NO2 + NO = N2O3 If at a particular temperature, K...
- chemistry - At what temperature would you expect dinitrogen pentoxide to sublime...
- Chemistry - Dinitrogen pentoxide, N2O5, decomposes by a first-order reaction. ...
- chemistry - The decomposition of N2O5 proceeds according to the following ...
- chemistry - given this reaction N2O5 -> 2 N2O + 1/2 O2 all gases and given ...
- Chemistry - A reaction is first order and it takes 324 minutes for the reaction ...
- Chemistry - Your Open Question Show me another ยป Chemistry help needed... ...
- Chemistry - The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g...
- science - 2N2O5->4NO2+O2,d[N2O5]/dt=k1[N2O5],d[NO2]/dt=k2[N2O5]andd[O2]/dt=k3...

More Related Questions