- Calculating equilibrium constant Kp using partial pressures
They are related to each other by the equation: Kp = Kc (RT)^ (Δn), where Kc and Kp are already explained, R is the universal gas constant, T is the temperature, and Δn is the difference between the total moles of gas for the products and the total moles of gas for the reactants
- Worked examples: Calculating equilibrium constants - Khan Academy
In this video, we'll calculate equilibrium constants using measurements of concentration and partial pressures at equilibrium First, we'll find Kc for an equilibrium system using equilibrium concentrations Then, we'll find Kp for a different system using equilibrium partial pressures
- Writing equilibrium constant and reaction quotient expressions
If we were to write a Kp expression here, we would include the partial pressure of our gas, which is carbon dioxide So this would be the partial pressure of carbon dioxide to the first power And once again, we would leave the two solids out of our equilibrium constant expression
- Calculating an equilibrium constant from initial and equilibrium . . .
So, we would write Kp is equal to, and for our products, we have PCl3, so this would be the partial pressure of PCl3 times the partial pressure of our other product, which is Cl2, so let's put in there the partial pressure of Cl2
- Using the reaction quotient to find equilibrium partial pressures . . .
The equilibrium constant Kp is equal to 0 26 at 1000 Kelvin Our goal is to find the equilibrium partial pressures of our two gasses, carbon monoxide and carbon dioxide
- The equilibrium constant K (article) | Khan Academy
At this point, you might be wondering why this equation looks so familiar and how Q is different from K c The main difference is that we can calculate Q for a reaction at any point whether the reaction is at equilibrium or not, but we can only calculate K c at equilibrium
- Standard change in free energy and the equilibrium constant
And this equation relates the equilibrium constant K to delta-G zero, the standard change in free energy So, delta-G zero becomes a guide to the ratio of the amount of products to reactants at equilibrium, because it's related to the equilibrium constant K in this equation
- Changes in free energy and the reaction quotient - Khan Academy
For this reaction at 25 degrees C the equilibrium constant, which would be KP, is equal to 6 1 times 10 to the fifth Our value for the reaction quotient was 0625
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