state and derive the relation between Kc and K p and carry out some calculations involving them and z list the factors which affect the state of equilibrium and state and apply Le-Chatelier principle.

The relationship between Kc and Kp is derived from the ideal gas law. Kc is the equilibrium constant in terms of concentration (mol/L) and Kp is the equilibrium constant in terms of pressure.

The ideal gas law is PV = nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature.

If we rearrange this to get P = n/V * RT, we can see that P is directly proportional to n/V, which is the concentration. Therefore, we can replace concentration in the expression for Kc with P/RT to get Kp.

So, Kp = Kc(RT)^Δn, where Δn is the change in moles of gas in the reaction (moles of gaseous products - moles of gaseous reactants).

For example, for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), Δn = 2 - (1+3) = -2. If Kc for this reaction at a certain temperature is 4.34 x 10^-3, R is 0.0821 L.atm/mol.K, and T is 300K, then Kp = Kc(RT)^Δn = 4.34 x 10^-3 * (0.0821 * 300)^-2 = 3.6 x 10^5.

The factors which affect the state of equilibrium are concentration, pressure, temperature, and the presence of a catalyst.

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

For example, if we increase the pressure of the system in the above reaction, according to Le Chatelier's principle, the system will try to decrease the pressure by shifting the equilibrium to the side with fewer moles of gas, which is the right side (production of NH3). Therefore, increasing the pressure increases the production of NH3.