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 __________

At a given temperature and pressure, the equilibrium constant values for the equilibria
\({ 3A }_{ 2 }+{ B }_{ 2 }+2C\overset { { K }_{ 1 } }{ \rightleftharpoons } { 2A }_{ 3 }BC\) and
\({ A }_{ 3 }BC\overset { { K }_{ 2 } }{ \rightleftharpoons } 3/2\left[ { A }_{ 2 } \right] +\frac { 1 }{ 2 } { B }_{ 2 }+C\)
The relation between K₁ and K₂ is ___________

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

The formation of ammonia from N₂(g) and H₂(g) is a reversible reaction
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat
What is the effect of increase of temperature on this equilibrium reaction ______________

Solubility of carbon dioxide gas in cold water can be increased by ____________

Which one of the following is incorrect statement?

K₁ and K₂ are the equilibrium constants for the reactions respectively.
\({ N }_{ 2 }(g)+{ O }_{ 2 }(g)\overset { { K }_{ 1 } }{ \rightleftharpoons } 2NO(g)\)
\(2NO(g)+{ O }_{ 2 }(g)\overset { { K }_{ 2 } }{ \rightleftharpoons } { 2NO }_{ 2 }(g)\)
What is the equilibrium constant for the reaction NO₂(g) ⇌ ½N₂(g) + O₂(g)

In the equilibrium,
2A(g) ⇌ 2B(g) + C₂(g)
the equilibrium concentrations of A, B and C₂ at 400 K are 1\(\times\)10^–4 M, 2.0 \(\times\)10^–3 M, 1.5 \(\times\)10^–4 M respectively. The value of K_C for the equilibrium at 400 K is ________

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

\({K_c\over K_p}\) for the reaction,
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is ___________

For the reaction AB (g) ⇌ A(g) + B(g), at equilibrium, AB is 20% dissociated at a total pressure of P, The equilibrium constant K_P is related to the total pressure by the expression __________

In which of the following equilibrium, K_P and K_C are not equal ?

If x is the fraction of PCl₅ dissociated at equilibrium in the reaction
PCl₅ ⇌ PCl₃ + Cl₂
then starting with 0.5 mole of PCl₅, the total number of moles of reactants and products at equilibrium is ___________

The values of K_P1 and K_P2 for the reactions
X ⇌ Y + Z
A ⇌ 2B are in the ratio 9 : 1 if degree of dissociation and initial concentration of X and A be equal then total pressure at equilibrium P₁ and P₂ are in the ratio __________

In the reaction,
Fe (OH)₃ (s) ⇌ Fe³⁺(aq) + 3OH^–(aq),
if the concentration of OH^– ions is decreased by ¼ times, then the equilibrium concentration of Fe³⁺ will

Consider the reaction where K_P = 0.5 at a particular temperature
PCl₅(g) ⇌ PCl₃ (g) + Cl₂ (g)
if the three gases are mixed in a container so that the partial pressure of each gas is initially 1 atm, then which one of the following is true ____________

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 ____________

In a chemical equilibrium, the rate constant for the forward reaction is 2.5 \(\times\)10² and the equilibrium constant is 50. The rate constant for the reverse reaction is ____________

Which of the following is not a general characteristic of equilibrium involving physical process ___________

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 __________

Match the equilibria with the corresponding conditions,

Consider the following reversible reaction at equilibrium, A + B ⇌ C, If the concentration of the reactants A and B are doubled, then the equilibrium constant will ___________

[Co(H₂O)₆]²⁺ (aq) (pink) + 4Cl^– (aq) ⇌ [CoCl₄]^2– (aq) (blue) + 6 H₂O (l)
In the above reaction at equilibrium, the reaction mixture is blue in colour at room temperature. On cooling this mixture, it becomes pink in colour. On the basis of this information, which one of the following is true?

The equilibrium constants of the following reactions are:

The equilibrium constant (K) for the reaction ;
\({ 2NH }_{ 3 }+5/2{ O }_{ 2 }\overset { K }{ \rightleftharpoons } 2NO+{ 3H }_{ 2 }{ O },\) will be

A 20 litre container at 400 K contains CO₂ (g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of CO₂ attains its maximum value will be: Given that: SrCO₃ (S) ⇌ SrO (S) + CO₂(g)
KP = 1.6 atm

If there is no change in concentration, why is the equilibrium state considered dynamic?

For a given reaction at a particular temperature, the equilibrium constant has constant value. Is the value of Q also constant? Explain.

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

For a gaseous homogeneous reaction at equilibrium, number of moles of products are greater than the number of moles of reactants. Is K_C is larger or smaller than K_P.

When the numerical value of the reaction quotient (Q) is greater than the equilibrium constant (K), in which direction does the reaction proceed to reach equilibrium?

State Le-Chatelier principle.

Consider the following reactions,
H₂(g) + I₂(g) ⇌ 2 HI(g)
In each of the above reaction find out whether you have to increase (or) decrease the volume to increase the yield of the product.

State law of mass action.

Explain how will you predict the direction of a equilibrium reaction.

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

Write a balanced chemical equation for  equilibrium reaction for which the equilibrium constant is given by expression
\(K_c={[NH_3]^4[O_2]^5\over [NO]^4[H_2O]^6}\)

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

Derive the relation between K_P and K_C.

Deduce the Vant Hoff equation.

The value of K_c for the following reaction at 717 K is 48.

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

One mole of H₂ and one mole of I₂ are allowed to attain equilibrium in 1 lit container. If the equilibrium mixture contains 0.4 mole of HI. Calculate the equilibrium constant.

The equilibrium concentrations of NH₃, N₂ and H₂ are 1.8 x 10^-2 M, 1.2 x 10^-2 M and 3 x 10^-2 M respectively. Calculate the equilibrium constant for the formation of NH₃ from N₂ and H₂. [Hint: M= mol lit^-1]

For an equilibrium reaction K_p = 0.0260 at 25° C ΔH= 32.4 kJmol^-1, calculate Kp at 37° C

For the reaction,
A₂(g) + B₂(g) ⇌ 2AB(g) ; ΔH is –ve.
the following molecular scenes represent different reaction mixture (A – green, B – blue)

i) Calculate the equilibrium constant K_P and (K_C).
ii) For the reaction mixture represented by scene (x), (y) the reaction proceed in which directions?
iii) What is the effect of increase in pressure for the mixture at equilibrium.

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.

For the reaction
SrCO₃ (s) ⇌ SrO (s) + CO₂(g),
the value of equilibrium constant K_P = 2.2 x 10^–4 at 1002 K. Calculate K_C for the reaction.

To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with 0.3 mol of HI gas and allows the reaction to proceed at 500^o C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate K_C and K_{P for this reaction.}

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.

The equilibrium constant at 298 K for a reaction is 100.
A + B \(\rightleftharpoons \) C + D
If the initial concentration of all the four species is 1 M, the equilibrium concentration of D (in mol lit^-1) will be

Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) ⇌ [Fe(SCN)]²⁺(aq)
A solution is made with initial Fe³⁺, SCN^- concentration of 1 x 10^-3 M and 8 x 10^-4 M respectively. At equilibrium [Fe(SCN)]²⁺ concentration is 2 x 10^-4 M. Calculate the value 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.

The following water gas shift reaction is an important industrial process for the production of hydrogen gas.
CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)
At a given temperature K_p = 2.7. If 0.13 mol of CO, 0.56 mol of water, 0.78 mol of CO₂ and 0.28 mol of H₂ are introduced into a 2 L flask, and find out in which direction must the reaction proceed to reach equilibrium

1 mol of PCl₅, kept in a closed container of volume 1 dm³ and was allowed to attain equilibrium at 423 K. Calculate the equilibrium composition of reaction mixture. (The K_c value for PCl₅ dissociation at 423 K is 2)

The equilibrium constant for the following reaction is 0.15 at 298 K and 1 atm pressure.
N₂O₄(g) ⇌ 2NO₂(g);
\(\Delta \mathrm{H}_{\mathrm{f}}^{\circ}=57.32 \mathrm{KJmol}^{-1}\)
The reaction conditions are altered as follows.
a) The reaction temperature is altered to 100^o C keeping the pressure at 1 atm, Calculate the equilibrium constant.

1 mol of CH₄, 1 mole of CS₂ and 2 mol of H₂S are 2 mol of H₂ are mixed in a 500 ml flask. The equilibrium constant for the reaction K_C = 4 x 10^–2 mol² lit^–2. In which direction will the reaction proceed to reach equilibrium ?

At particular temperature K_C = 4 x 10^–2 for the reaction
H₂S(g) ⇌ H₂(g) + ½ S₂(g)
Calculate KC for each of the following reaction
i) 2H₂S (g) ⇌ 2H₂ (g) + S₂ (g)
ii) 3H₂S (g) ⇌ 3H₂ (g) + 3/2 S₂(g)

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.

The equilibrium for the dissociation of XY₂ is given as,
2XY₂ (g) ⇌ 2XY (g) + Y₂(g)
if the degree of dissociation x is so small compared to one. Show that 2 K_P = PX₃ where P is the total pressure and K_P is the dissociation equilibrium constant of XY₂.

A sealed container was filled with 1 mol of A₂ (g), 1 mol B₂ (g) at 800 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 1 for the reaction
A₂ (g) + B₂ (g) ⇌ 2AB (g)

The equilibrium constant K_P for the reaction
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is 8.19 x 10² at 298 K and 4.6 x 10^–1 at 498 K. Calculate ΔH^o for the reaction

The partial pressure of carbon dioxide in the reaction
CaCO₃ (s) ⇌ CaO (s) + CO₂(g) is 1.017 × 10^–3 atm at 500⁰C. Calculate K_p at 600⁰C for the reaction. ΔH for the reaction is 181 KJ mol^–1 and does not change in the given range of temperature.