Relation between kp and kc

Relationship between Kp and Kc is Kp = Kc(RT)^Δn .

1. What is the relationship between KP and KC equal?
2. Are KC and KP proportional?
3. What if KP is greater than KC?
4. What does KC and KP depend on?
5. Why is KP not equal to KC?
6. When the value of KP is less than KC?
7. What does it mean if KP is less than 1?
8. Are KC and KP always equal?
9. Is KC always greater than KP?
10. When KP becomes equal to KC give an example?
11. Are KC and KP always equal?
12. Do the values of KP and KC depend on pressure?
13. Why KP and KC are pressure independent?
14. What happens to KP if pressure increases?
15. How are KC and KP related to each other in the following reaction justify?
16. What is the relationship between KP and pressure?

What is the relationship between KP and KC equal?

Kp only counts with gases molecule , while Kc only counts with aqueous solution+ gases. So here reactant and product both are gaseous that's why only reaction having equal numbers of reactants and products will have kp=kc ie.

Are KC and KP proportional?

Notice that in the Kc correlation, a large Kp in the denominator will yield a small Kc value (that is, Kc is inversely proportional to Kp).

What if KP is greater than KC?

Assertion: Kp is always greater than Kc. Reason: The effect of pressure is greater on the rate of reaction than the effect of concentration.

What does KC and KP depend on?

the relation between Kp and Kc depends on the change in the number of moles of gaseous reactants and products.

Why is KP not equal to KC?

Kp only counts with gases, while Kc only counts with aqueous solution + gases. I assumed that any reactions with only gases, or a mix of gases and solids, will have an equal Kp and Kc value, but that is clearly not the case.

When the value of KP is less than KC?

KP = KC(RT)△n; When △n = 2 − (2 + 1) = −1, i.e. negative.

What does it mean if KP is less than 1?

If the value of K is less than 1, the reactants in the reaction are favored.

Are KC and KP always equal?

Kp only counts with gases molecule , while Kc only counts with aqueous solution+ gases. So here reactant and product both are gaseous that's why only reaction having equal numbers of reactants and products will have kp=kc ie.

Is KC always greater than KP?

Kp is always greater than Kc .

When KP becomes equal to KC give an example?

e.g., H2(g)+I2(g)↽⇀2HI(g) Kp=KC.

Are KC and KP always equal?

Kp only counts with gases molecule , while Kc only counts with aqueous solution+ gases. So here reactant and product both are gaseous that's why only reaction having equal numbers of reactants and products will have kp=kc ie.

Do the values of KP and KC depend on pressure?

S : Kc, Kp and Kx are the equilibrium constants of a reaction in terms of concentration, pressure and mole fraction respectively. E : Kc and Kp do not depend on equilibrium pressure but Kx depends upon equilibrium pressure if Δn=0.

Why KP and KC are pressure independent?

The reason Kp is pressure-independent is not directly because it is defined as such. Rather, the reason Kp is pressure-independent is because it's assumed that the gases in the equilibrium expression behave ideally. That's the fundamental stipulation; the pressure-independence is a consequence of this.

What happens to KP if pressure increases?

Pressure does not affect the value of Kp, just as concentration does not affect the value of Kc. An increase in pressure causes equilibrium to shift in favor of the direction with the fewer moles so that the pressure decreases. The partial pressure ratio of reactant to products stays the same so Kp does not change.

How are KC and KP related to each other in the following reaction justify?

The given reaction is . Here one mole of nitrogen and one mole of oxygen gas reacts to produce two moles of NO. Here ∆n= number of mole of product-number of moles of reactant. So, the relationship between Kp and Kc is Kp=Kc.

What is the relationship between KP and pressure?

Equilibrium constant Kp is equal to the partial pressure of products divided by partial pressure of reactants and the partial pressure are raised with some power which is equal to the coefficient of the substance in balanced equation.