Samacheer Kalvi solutions for Chemistry - Volume 1 and 2 [English] Class 11 TN Board chapter 8 - Physical and Chemical Equilibrium [Latest edition]

If K_b and K_f for a reversible reaction are 0.8 × 10^-5 and 1.6 × 10^-4 respectively, the value of the equilibrium constant is,

At a given temperature and pressure, the equilibrium constant values for the equilibria

\[\ce{3A2 + B2 + 2Cr <=>[K1] 2A3BC}\] and

\[\ce{A3BC <=> 3/2 A2 + 1/2 B2 + C}\]

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

\[\ce{N2(g) + 3H2(g) <=> 2NH3(g) + Heat}\]

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.

\[\ce{N2(g) + O2(g) <=>[K1] 2NO(g)}\]

\[\ce{NO(g) + O2(g) <=>[K2] 2NO2(g)}\]

What is the equilibrium constant for the reaction \[\ce{NO2(g) <=> 1/2 N2(g) + O2(g)}\]

In the equilibrium,

\[\ce{2A(g) <=> 2B(g) + C2(g)}\]

the equilibrium concentrations of A, B and C₂ at 400 K are 1 × 10^–4 M, 2.0 × 10^–3 M, 1.5 × 10^–4 M respectively. The value of K_C for the equilibrium at 400 K is

An equilibrium constant of 3.2 × 10^-6 for a reaction means, the equilibrium is

`"K"_"C"/"K"_"P"` for the reaction,

\[\ce{N2(g) + 3H2(g) <=> 2NH3(g)}\] is

For the reaction \[\ce{AB(g) <=> A(g) + B(g)}\], 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

\[\ce{PCl5 <=> PCl3 + Cl2}\]

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 of X and A be equal then total pressure at equilibrium P₁, and P₂ are in the ratio

In the reaction

\[\ce{Fe(OH)3(S) <=> Fe^{(3+)} (aq) + 3OH- (aq)}\]

if the concentration of OH^– ions is decreased by 1/4 times, then the equilibrium concentration of Fe³⁺ will

Consider the reaction where K_p = 0.5 at a particular temperature

\[\ce{PCl5(g) <=> PCl3 (g) + Cl2 (g)}\]

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 liter flask. What percentage of the initial concentration of H₂ has reacted at equilibrium if the rate constant for both forward and reverse reactions are equal

In a chemical equilibrium, the rate constant for the forward reaction is 2.5 × 10^-2, 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:

1. Liquid ⇌ Vapour
2. Solid ⇌ Liquid
3. Solid ⇌ Vapour
4. Solute(s) ⇌ Solute (Solution)

1. Melting point
2. Saturated solution
3. Boiling point
4. Sublimation point
5. Unsaturated solution

Consider the following reversible reaction at equilibrium,

\[\ce{A + B <=> C}\],

If the concentration of the reactants A and B are doubled, then the equilibrium constant will

\[\ce{[CO(H2O)6]^2+ (aq) (pink) + 4Cl- (aq) <=> [CoCl4]^2- (aq) (blue) + 6 H2O (l)}\]

In the above reaction at equilibrium, the reaction mixture is blue in colour at room temperature. On cooling this mixture, it becomes pink in color. On the basis of this information, which one of the following is true?

The equilibrium constants of the following reactions are:

\[\ce{N2 + 3H2 <=> 2NH3}\]; K₁

\[\ce{N2 + O2 <=> 2NO}\]; K₂

\[\ce{H2 + 1/2O2 <=> H2O}\]; K₃

The equilibrium constant (K) for the reaction;

\[\ce{2NH3 + 5/2 O2 <=> 2NO + 3H2O}\], will be

A 20 litre container at 400 K contains CO₂ (g) at pressure 0.4 atm and an excess (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 the pressure of CO₂ attains its maximum value will be:

Given that: \[\ce{SeCO3(S)≅ SrO + CO2 (g)}\] [K_p = 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 a constant value. Is the value of Q also constant? Explain.

What is the relation between K_p and K_c? Given one example for which K_p is equal to K_c.

For a gaseous homogeneous reaction at equilibrium, a number of moles of products is 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, in which direction does the reaction proceed to reach equilibrium?

For the reaction, \[\ce{A2(g) + B2(g) <=> 2AB(g); \Delta H}\] is -ve.

the following molecular scenes represent differenr reaction mixture. (A-green, B-blue)

Closed  ←
System	At equilibrium	(x)	(y)

1. Calculate the equilibrium constant K_p and (K_c).
2. For the reaction mixture represented by scene (x), (y) the reaction proceed in which directions?
3. What is the effect of an increase in pressure for the mixture at equilibrium?

State Le – Chateller principle.

Consider the following reaction,

\[\ce{H2(g) + l2(g) <=> 2HI(g)}\]

In the above reactions find out whether you have to increase (or) decrease the volume to increase the yield of the product.

Consider the following reaction,

\[\ce{CaCO3(s) <=> CaO(s) + CO2(g)}\]

In the above reactions find out whether you have to increase (or) decrease the volume to increase the yield of the product.

Consider the following reaction,

\[\ce{S(s) + F2(g) <=> SF6(g)}\]

In the above reactions 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 an equilibrium reaction.

Derive a general expression for the equilibrium constant Kp and Kc for the reaction, \[\ce{3H2(g) + N2(g) <=> 2NH3(g)}\].

Write the balanced chemical equation for an equilibrium reaction for which the equilibrium constant is given by expression.

`"K"_"C" = (["NH"_3]^4["O"_2]^5)/(["NO"]^4["H"_2"O"]^6)`

What is the effect of added Inert gas on the reaction at equilibrium?

Derive the relation between K_p and K_c.

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

\[\ce{SrCO3(s) <=> SrO(s) + CO2(g)}\]

the value of equilibrium constant K_p = 2.2 × 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°C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate K_c and K_p.

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 × 10^-2 for the reaction, \[\ce{H2S (g) <=> H2(g) +1/2 S2(g)}\]. Calculate the K_c for the following reaction.

\[\ce{2H2S (g) <=> 2H2 (g) + S2 (g)}\]

At particular temperature K_c = 4 × 10^-2 for the reaction, \[\ce{H2S (g) <=> H2(g) +1/2 S2(g)}\]. Calculate the K_c for the following reaction.

\[\ce{3H2S (g) <=> 3H2 (g) + 3/2 S2 (g)}\]

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,

\[\ce{2 XY2 (g) <=> 2 XY (g) + Y2 (g)}\]

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 0.3 mol H₂(g), 0.4 mol I₂(g) and 0.2 mol HI(g) at 800 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 870 for the reaction, \[\ce{A2 (g) + B2 (g) <=> 2 AB (g)}\].

Deduce the Vant Hoff equation.

The equilibrium constant K_p for the reaction \[\ce{N2 (g) + 3H2 (g) <=> 2NH3 (g)}\] is 8.19 × 10² at 298 K and 4.6 × 10^-1 at 498 K. Calculate ∆H° for the reaction.

The partial pressure of carbon dioxide in the reaction

\[\ce{CaCO3(s) <=> CaO(s) + CO2(g)}\] is 1.017 × 10^-3 atm at 500°C. Calculate K_p at 600°C for the reaction. H for the reaction is 181 KJ mol^-1 and does not change in the given range of temperature.