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1. Calculate Kp for the reaction below at 298K

2𝐢𝑙2(𝑔)+10𝑁𝑂(𝑔)⟷5𝑁2(𝑔)+2𝐢𝑙2𝑂5(𝑔)𝐾𝑝=?

Given at 298K:
2𝐢𝑙2𝑂5(𝑔)⟷5𝑂2(𝑔)+2𝐢𝑙2(𝑔) 𝐾𝑝1=0.095
2𝑁𝑂(𝑔)βŸ·π‘2(𝑔)+𝑂2(𝑔) 𝐾𝑝2=476

2. Below is a list of reactions. Match the rearranged equations with how you would calculate the new reaction coefficient.

reaction 1: A <---> C K_1

reaction 2: A <---> E K_2

reaction 3: B <---> D K_3

-C <---> E
-2A <---> 2C
-A + B <---> C + D
-C <---> A

Choose:
K_1/K_3
K_1
Kc = K_2/K_1
K_3/K_1
K_2*K_1
Kc = K_1*K_3
Kc = 1/K_1
Kc = K_1^2
1/K_1^2
K_1/K_2

For part 1. If Kforward = Kf then Kreverse = Kr = 1/Kf and if you make

A + B = C and Kc = ? and you multiply by 2 then
2A + 2B = 2C, Then K'c = (Kc)^2 and
2C = 2A + 2B then K"c = (1/K'c) = (1/Kc)^2
When adding equations for delta H or delta G or delta S calculations you are correct. The reversed equation is the negative of the forward but for K it is 1/K.

I'm not sure I understand completely for part 2. As I understand it you have these three following equations.
reaction 1: A <---> C K_1
reaction 2: A <---> E K_2
reaction 3: B <---> D K_3
I don't know what "reaction coefficaiton" means but I think you want the K for the reaction E<===> C. I assume k1 is Kc but I don't know that.
To do that you use eqn 1 and 2 (You don't need eqn 3 since that has B and D and neither show up in what you want).
Reverse eqn 1 like this.
A ==> C Kc = k1 so reversed it is

C ---> A K'c = 1/k1. Now add in eqn 2 like this
A ---> E K = k2
----------------------------------
C + A ==> A + E. The A cancels and you're left with
C ==> E Then Kc = k2/k1 so I would pick the third answer from the top.
Hope all of this helps.

well, the second question is that there's these reactions 1-3 given. i need to solve for reaction coefficaiton of the rearranged equations: C <---> E. the answer options are K_1/K_3 you see.

Thank you, I got the Kp2^5, but i was confused with the Kp1 since i thought it meant that i had to make it -Kp1 not 1/kp1

1. To calculate Kp for the given reaction at 298K, we need to use the equilibrium constant expression and the values of the equilibrium constants for the related reactions. The equation for Kp is as follows:

Kp = (P_N2)^5 * (P_Cl2O5)^2 / (P_Cl2)^2 * (P_NO)^10 * (P_O2)^2

Given that:
Kp1 = 0.095 for 2Cl2O5(g) ⟷ 5O2(g) + 2Cl2(g)
Kp2 = 476 for 2NO(g) ⟷ N2(g) + O2(g)

We can rearrange the equation for the reaction of interest to match the stoichiometry of the related reactions:

2Cl2(g) + 10NO(g) ⟷ 5N2(g) + 2Cl2O5(g)

Thus, we can determine the value of Kp for the reaction of interest by substituting the known Kp values into the equation:

Kp = (476)^5 * (0.095)^2 / (1)^2 * (1)^10 * (1)^2

Calculating this expression will yield the value of Kp for the reaction.

2. To match the rearranged equations with how you would calculate the new reaction coefficient, we need to determine the proper mathematical relationship based on the rearranged equations:

- Reaction 1: A ←→ C K_1
- Reaction 2: A ←→ E K_2
- Reaction 3: B ←→ D K_3

The rearranged equations are:
- C ←→ E
- 2A ←→ 2C
- A + B ←→ C + D
- C ←→ A

The correct choice is:
Kc = K_1/K_3

Explanation:
To calculate the new reaction coefficient based on the rearranged equations, we compare the stoichiometric coefficients of the different species involved. In this case, the rearranged equations give us a relationship between the reactants and products in terms of their stoichiometric coefficients.

The proper mathematical relationship that matches the rearranged equations is Kc = K_1/K_3. This means that the equilibrium constant for the rearranged equation is equal to the ratio of the equilibrium constants for reaction 1 and reaction 3.

I have no clue what you want. For the first part I understand you want the Kp for this reaction. 2𝐢𝑙2(𝑔)+10𝑁𝑂(𝑔)⟷5𝑁2(𝑔)+2𝐢𝑙2𝑂5(𝑔) 𝐾𝑝=? which I will call eqn 1. You have these two eqns (eqn 2 and eqn 3) to help.

2𝐢𝑙2𝑂5(𝑔)⟷5𝑂2(𝑔)+2𝐢𝑙2(𝑔) 𝐾𝑝1=0.095
2𝑁𝑂(𝑔)βŸ·π‘2(𝑔)+𝑂2(𝑔) 𝐾𝑝2=476
Do this:
Reverse eqn 2 and add to 5 times eqn 3. I suggest you do this on paper and make SURE you get eqn1 since I did this in my head and may have made an error. If you do that, then kp1 reverse = 1/Kp1 = (1/0.095) and new Kp2 = (Kp2)^5 so Kp for the reaction you want (eqn 1) will be
(476)^5/(0.095)
Post your work if you get stuck.
The remainder of what you wrote is gibberish. What are A, B, C, D and to which reactions so K1, K2, K3 etc refer?