<h3>Kp = 1.483 . 10³</h3><h3>Further explanation</h3>
The equilibrium constant is the ratio of concentration or pressure between the results of the reaction / product and the reactant with each reaction coefficient raised
The equilibrium constant is based on the concentration (Kc) in a reaction
pA + qB -----> mC + nD
![\large {\boxed {\bold {Kc ~ = ~ \frac {[C] ^ m [D] ^ n} {[A] ^ p [B] ^ q}}}}](https://tex.z-dn.net/?f=%20%5Clarge%20%7B%5Cboxed%20%7B%5Cbold%20%7BKc%20~%20%3D%20~%20%5Cfrac%20%7B%5BC%5D%20%5E%20m%20%5BD%5D%20%5E%20n%7D%20%7B%5BA%5D%20%5E%20p%20%5BB%5D%20%5E%20q%7D%7D%7D%7D%20)
While the equilibrium constant is based on partial pressure
![\large {\boxed {\bold {Kp ~ = ~ \frac {[pC] ^ m [pD] ^ n} {[pA] ^ p [pB] ^ q}}}}](https://tex.z-dn.net/?f=%20%5Clarge%20%7B%5Cboxed%20%7B%5Cbold%20%7BKp%20~%20%3D%20~%20%5Cfrac%20%7B%5BpC%5D%20%5E%20m%20%5BpD%5D%20%5E%20n%7D%20%7B%5BpA%5D%20%5E%20p%20%5BpB%5D%20%5E%20q%7D%7D%7D%7D%20)
The value of Kp and Kc can be linked to the formula '

R = gas constant = 0.0821 L.atm / mol.K
=n = number of product coefficients-number of reactant coefficients
There are rules in determining the Kp value for the related reaction
- 1. If the reaction equation is reversed, the value of Kp is also reversed
- 2. if the reaction coefficient is divided by a factor n, then the new Kp value is the square root of n from the old Kp
- 3. if the reaction coefficient is multiplied by the factor n, then the new Kp value is the power of n from the old Kp
2COF₂ (g) ⇌CO₂(g) + CF₄ (g) Kp = 2.2 × 10⁶ at 298 K(reaction 1)

For the reaction 2, the reaction coefficient is divided by 2, so the new Kp value :

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