If K_b and K_f for a reversible reactions are 0.8 x 10^–5 and 1.6 x 10^–4 respectively, the value of the equilibrium constant is __________

The equilibrium constant for a reaction at room temperature is K₁ and that at 700 K is K₂. If K₁ > K₂, then _____________

An equilibrium constant of 3.2\(\times\)10^–6 for a reaction means, the equilibrium is _____________

Equimolar concentrations of H₂ and I₂ are heated to equilibrium in a 1 litre flask. What percentage of initial concentration of H₂ has reacted at equilibrium if rate constant for both forward and reverse reactions are equal ____________

For the formation of Two moles of SO₃(g) from SO₂ and O₂, the equilibrium constant is K₁. The equilibrium constant for the dissociation of one mole of SO₃ into SO₂ and O₂ is __________

For reaction, \(2A+B\rightleftharpoons 2C,\ K=x\) . Equilibrium constant for \(C\rightleftharpoons A+1/2B\) will be ____________

In the equilibrium reaction CaCO₃(s)⇌ CaO(s) + CO₂(g) whose concentration remains constant at a given temperature?

What is the relation between K_P and K_C. Give one example for which K_P is equal to K_C.

State Le-Chatelier principle.

State law of mass action.

Derive a general expression for the equilibrium constant K_P and K_C for the reaction 
3H₂(g) + N₂(g) ⇌ 2NH₃(g).

What is the effect of added inert gas on the reaction at equilibrium at constant volume.

Deduce the Vant Hoff equation.

Write the relationship between equilibrium constant and enthalpy.

"Rate of Melting = Rate of freezing"
When is the above condition achieved? Explain with an example

The value of Kc for the reaction
N₂O₂(g) \(\rightleftharpoons \) 2NO₂(g)

One mole of PCl₅ is heated in one litre closed container. If 0.6 mole of chlorine is found at equilibrium, calculate the value of equilibrium constant.

Oxidation of nitrogen monoxide was studied at 200^o C with initial pressures of 1 atm NO and 1 atm of O₂. At equilibrium partial pressure of oxygen is found to be 0.52 atm calculate K_P value.

List out few examples of irreversible reactions (changes) taking place in our daily life activity.

Mention the applications of equilibrium constant

The atmospheric oxidation of NO
2NO(g) + O₂(g) ⇌ 2NO₂(g)
was studied with initial pressure of 1 atm of NO and 1 atm of O₂. At equilibrium, partial pressure of oxygen is 0.52 atm calculate K_p of the reaction.

28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH₃ was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

Derive the K_p and K_c for the following equilibrium reaction.
\({ H }_{ 2\left( g \right) }+{ I }_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

Explain the effect of concentration, pressure, temperature, catalyst and inert gas on equilibrium.