What is the equation for KP?
For the equation Kp = Kc(RT)^(delta N), shouldn’t there be two instances in which Kp = Kc? First, when delta N = 0 (mols of product gas = mols of reactant gas); second when temperature T is the exact reciprocal of constant R or when R*T = 1 (if R = 0.08206 L*atm*mol^(-1)*K^(-1), T = 1/0.08206 K)?
What is the relation between KP and KC in chemistry?
We know that the relationship between Kc and Kp is Kp=Kc (RT.
How do you know if KC is KP?
1 AnswerIn order for Kc and Kp to be equal, you need the volume to remain constant at equilibrium, that is, In this case, you have 2 moles of gas on the products’ side and 5 moles of gas on the reactants side → Kp≠Kc . Since you have 2 moles of gas on both sides of the equilibrium, you will indeed get Kp=Kc .
What is the unit of KP and KC?
They are factors / constants, they have no unit(s). ( well Kc only sometimes). Kp, defined as the equilibrium constant in terms of fugacities of the components of the reactive mixture (partial pressures in the case of ideal gases), is non-dimensional. They are factors / constants, they have no unit(s).
Does KP change with pressure?
Changing the pressure can’t make any difference to the Kp expression. The position of equilibrium doesn’t need to move to keep Kp constant. Equilibrium constants are changed if you change the temperature of the system. This is typical of what happens with any equilibrium where the forward reaction is exothermic.
Is KP equal to KC?
So if you want to get to Kp from Kc, the equation is this. So you have Kp equals Kc times RT to the delta n. Kp is the equilibrium constant and pressures.
Are KP and KC the same?
Kc is the equilibrium constant when it is found through the use of concentrations, while Kp is the equilibrium constant when it is found through the use of partial pressures.
When KP will be greater than KC?
Kp equals Kc when Δn = 0. This is true when the number of moles of gaseous products equals the number of moles of gaseous reactants in the balanced chemical equation. The value of Kp may also be less than Kc (for Δn < 0) or greater than Kc (for Δn > 0).
At what condition is KP KC in equilibrium?
Kp And Kc are the equilibrium constant of an ideal gaseous mixture. Kp is equilibrium constant used when equilibrium concentrations are expressed in atmospheric pressure and Kc is equilibrium constant used when equilibrium concentrations are expressed in molarity.
Does KP only include gases?
A homogeneous equilibrium is one in which everything in the equilibrium mixture is present in the same phase. In this case, to use Kp, everything must be a gas.
Does KP unit?
Equilibrium constants (K, Kc, Kp) should not have units for many reasons. 1. Activities should be used not concentrations as activities are more accurate for real solutions and real gasses. Activities do not have units.
What is unit of KC?
They are both equilibrium constants as far as I know. Kc is in terms of molarity and Kp is in terms of pressure. Also both of them are ratios of respective quantities [ ratio of molarity(s) in Kc and ratio of pressure(s) in Kp], so they should be dimensionless according to dimensional analysis.
Why are KP and KC dimensionless?
Kc and Kp are also dimensionless, as they are defined properly using activities of the reactants and products which are dimensionless too. For simple calculations for Kp, dividing by the standard pressure of 1 bar for each component in the ratio brought to any power will always yield a dimensionless result.