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What is KP and KC?

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. For many general chemical reactions aA + bB ⇋ cC + dD.

byjus.com - Relation Between Kp And Kc - Formula, Units, Derivation - BYJU'S
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Relation Between Kp And Kc

K p And K c

K p And K c are the equilibrium constant of an ideal gaseous mixture. K p is equilibrium constant used when equilibrium concentrations are expressed in atmospheric pressure and K c is equilibrium constant used when equilibrium concentrations are expressed in molarity.

For many general chemical reactions aA + bB ⇋ cC + dD

Where a mole of reactant A

b mole of reactant B

c mole of product C

d mole of product D

Consider an example

2A (g) +B (g) ⇋ 2C (g) All in the gas phase.

The K p is given by-

(egin{array}{l}K_{p}= frac{P_{C}^{2}}{P_{A}^{2}P_{B}}end{array} )

Ideal Gas Equation

Each of these ideal gas molecules behaves similarly. So for each of them,

PV = nRT

On rearranging we get-

(egin{array}{l}P=frac{n}{V}RTend{array} )

Substituting these in equation (1)

(egin{array}{l}Rightarrow K_{p}=frac{left [ C ight ]^{2}left ( RT ight )^{2}}{left [ A ight ]^{2}left ( RT ight )^{2}left [ B ight ]left ( RT ight )}end{array} ) (egin{array}{l}Rightarrow K_{p}=frac{left [ C ight ]^{2}}{left [ A ight ]^{2}left [ B ight ]} imes frac{left ( RT ight )^{2}}{left ( RT ight )^{2}left ( RT ight )}end{array} )

On cancelling like terms and substituting

(egin{array}{l}K_{c}=frac{left [ C ight ]^{2}}{left [ A ight ]^{2}left [ B ight ]}end{array} )

(egin{array}{l}Rightarrow K_{p}=frac{K_{c}}{RT}end{array} )

Or

(egin{array}{l}K_{p}=K_{c}left ( RT ight )^{-1}end{array} )

In general,

(egin{array}{l}K_{p}=K_{c}left ( RT ight )^{Delta n}end{array} )

Where, Δn represents the change in the number of moles of gas molecules. [That is Δn = product – reactant in moles only for gas molecules] When the change in the number of moles of gas molecules is zero, that is Δn = 0

⇒ K p =K c

In general, for any chemical reactions of gas molecules the relation between K p And K c is- (egin{array}{l}K_{p}=K_{c}left ( RT ight )^{Delta n}end{array} ) (egin{array}{l}K_{c}=K_{p}left ( RT ight )^{-Delta n}end{array} )

Physics Related Topics:

Frequently Asked Questions – FAQs What are the basic properties of gases? Gases have three fundamental properties. Gases are very easy to compress. They occupy more space than solids or liquids. They typically expand to fill the spaces around them. What is the ideal gas equation? PV = nRT What is pressure? Pressure is defined as the force per unit area. What is temperature? Temperature is the measure of heat. What is an ideal gas? An ideal gas is a hypothetical gas which is made of a group of randomly-propagating point particles that intermix only through elastic collisions. Stay tuned to BYJU’S for more such interesting articles. Also, register to “BYJU’S-The Learning App” for loads of interactive, engaging physics related videos and an unlimited academic assist.

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What happens when K is less than Q?

If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants.

chem.purdue.edu - Calculating the Reaction Quotient, Q

Calculating the Reaction Quotient, Q

The expression for the reaction quotient, Q, looks like that used to calculate an equilibrium constant but Q can be calculated for any set of conditions, not just for equilibrium. Q can be used to determine which direction a reaction will shift to reach equilibrium. If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

In order to determine Q we need to know:

the equation for the reaction, including the physical states,

the quantities of each species (molarities and/or pressures), all measured at the same moment in time.

Write the expression for the reaction quotient.

Find the molar concentrations or partial pressures of each species involved.

Subsitute values into the expression and solve.

2

2

2

2

SO 2 Cl 2 (g) SO 2 (g) + Cl 2 (g) K c = 0.078 at 100oC

Write the expression to find the reaction quotient, Q.

Since K c is given, the amounts must be expressed as moles per liter (molarity). The amounts are in moles so a conversion is required. 0.500 mole SO 2 Cl 2 /5.00 L = 0.100 M SO 2 Cl 2 0.035 mole SO 2 /5.00 L = 0.070 M SO 2 0.080 mole Cl 2 /5.00 L = 0.016 M Cl 2 is given, the amounts must be expressed as moles per liter (molarity). The amounts are in moles so a conversion is required. Substitute the values in to the expression and solve for Q. Compare the answer to the value for the equilibrium constant and predict the shift.

0.078 (K) > 0.011 (Q)

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