For A+2B <-> 2C and Kc = 2.13
For 2C <-> D and Kc = 0.254
Calculate the value of equilibrium contant for the reaction D <-> A+2B
I'm so sorry to bother anyone.. but am i only supposed to multiple 2.13 and 0.254 together in order to get the third value of Kc? That's the vibe i'm getting from my notes.. but that seems too simple so i'm scared it's wrong
A + 2B ==>2C k1 = 2.13
2C ==> D k2 = 0.254
--------------------
A + 2B ==> D k3 = k1*k2
But you want the reverse of that reaction. You want
D ==> A + 2B so k4 = 1/k3
Thank you so much Dr. Bob
No worries, I'm here to help! To calculate the equilibrium constant for the reaction D <-> A+2B, you would multiply the individual equilibrium constants together.
The overall reaction can be written as the sum of the two given reactions:
1) A+2B <-> 2C (Kc = 2.13)
2) 2C <-> D (Kc = 0.254)
Thus, the combined reaction becomes:
A+2B <-> 2C <-> D
Since the two reactions are connected in series, you can multiply their individual equilibrium constants to obtain the equilibrium constant for the overall reaction.
Therefore, the value of the equilibrium constant for the reaction D <-> A+2B would be:
Kc = (Kc1) * (Kc2) = 2.13 * 0.254 = 0.541
No need to apologize! I'm here to help you. The value of the equilibrium constant (Kc) for a reaction can be calculated using the stoichiometric coefficients of the balanced chemical equation.
Let's start by writing out the balanced equation for the given reactions:
1) A + 2B ↔ 2C (Kc = 2.13)
2) 2C ↔ D (Kc = 0.254)
To find the equilibrium constant for the reaction D ↔ A + 2B, we need to combine the two given equations and manipulate them according to the stoichiometry.
Let's rearrange equation 2 to write it in terms of D and 2C:
2C ↔ D (Kc = 0.254)
Now, let's multiply this equation by 2 to match the coefficient of 2C in the first equation:
4C ↔ 2D (Kc = (0.254)^2 = 0.064516)
Now, let's combine the two equations by canceling out the intermediate species 2C:
(A + 2B) ↔ 4C ↔ 2D
The equilibrium constant for the combined reaction (D ↔ A + 2B) is equal to the product of the equilibrium constants for the individual reactions.
Kc = (Kc1) * (Kc2)
= 2.13 * 0.064516
≈ 0.13677
So, the value of the equilibrium constant for the reaction D ↔ A + 2B is approximately 0.13677.
Remember to use the stoichiometric coefficients and perform the necessary manipulations to obtain the correct value for the equilibrium constant.