11th Chemistry Monthly Test - 3 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Monthly Test - 3 ( Physical and Chemical Equilibrium )-Aug 2020

Time : 2.00 Hours

Part - A

Generic 2 - Answer All Question

What is the K_c value for formation of HI at 700 K? Predict the extent of the reaction?

Write the Kc for the reaction CO₂(g) + H₂O(l) \(\leftrightharpoons \) H^+(aq)+ HCO₃^-(aq).

What are the different types of equilibrium? Explain with example?

Define reaction quotient.

Consider the following reactions,
a) H₂(g) + I₂(g) ⇌ 2 HI
b) CaCO₃ (s) ⇌ CaO (s) + CO₂(g)
c) S(s) + 3F₂ (g) ⇌ SF₆ (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.

A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium partial pressure of HI(g) is 0.04 atm. What is K, for the given equilibrium?
2HI(g)u21cc H₂(g) +I₂(g)

2CO(g) +O₂(g) u21cc 2CO₂ at 1000 K. What is the Kc for this reaction? Predict the extent of this reaction.

Derive the relation between K_P and K_C.

"At constant volume addition of inert gas has no effect on equilibrium" - Justify

Write the expressions of equilibrium constants in terms of partial pressure and active masses for
\(2{ BrCl }_{ \left( g \right) }\rightleftharpoons { Br }_{ 2\left( g \right) }+{ Cl }_{ 2\left( g \right) }\)

Predict which of the following reaction will have appreciable concentration of reactants and products?
(i) \({ Cl }_{ 2\left( g \right) }\rightleftharpoons 2Cl_{ \left( g \right) };{ k }_{ c }=5\times { 10 }^{ -39 }\)
(ii) \({ Cl }_{ 2\left( g \right) }+2{ NO }_{ \left( g \right) }\rightleftharpoons 2NOCl_{ \left( g \right) };{ k }_{ c }=3.7\times { 10 }^{ -8 }\)
(iii) \({ Cl }_{ 2\left( g \right) }+2{ NO }_{ 2\left( g \right) }\rightleftharpoons 2NO_{ 2 }Cl_{ \left( g \right) };{ k }_{ c }=1.8\)

For the reaction,\({ A }_{ \left( g \right) }+{ B }_{ \left( s \right) }\rightleftharpoons { C }_{ \left( g \right) }+{ D }_{ \left( g \right) }\) K_c = 50 mol lit^-1at 127°C. Calculate K_p'

Equilibrium constant K; for the reaction, N₂(g) + 3H₂(g)u21cc 2NH₃(g) at 500 K is 0.06l. At particular time, the analysis shows that the composition of the reaction mixture is 3.0 mol L^-1 of N²; 2.0 mol L^-1 of H₃; 0.50 mol L^-1 of NH³. Is the reaction at equilibrium?

When will be K_P < K_C? Give two example

Part - B

Generic 3 - Answer All Question

Give three examples for solid vapour equilibrium.

(a) In the reaction A + B u27f6C + D, what will happen to the equilibrium if concentration of A is increased?
(b) The equilibrium constant for a reaction is 2 x 10^-23 at 25°C and 2 x 10^-2 at 50°C. Is the reaction endothermic or exothermic?
(c) Mention at least three ways by which the concentration of SO³ can be increased in the following reaction in a state of equilibrium.
2SO₂(g) + O₂g) u21cc2SO₃(g)

What happens when the concentration of H₂ and I₂ are increased in the reaction \({ H }_{ 2 }+{ I }_{ 2 }\rightleftharpoons 2HI?\)

Consider the reaction, N₂(g) + 3H₂(g) u21cc 2NH₃(g). Explain the effect of pressure on this equilibrium 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.

How does oxygen exchanges between maternal and fetal blood in a pregnant woman?

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

The value of Kc for the reaction

At a certain temperature and total pressure of 10⁵Pa, iodine vapours contain 40% by volume of iodine atoms in the equilibrium I₂(g) u21cc 2I(g). Calculate K_p for the equilibrium

Explain the effect of temperature on the following equilibrium reaction.
N₂(g) + 3H₂Cg)u21cc 2NH₃(g)Δ H = - 92.2 kJ.

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

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.

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

Discuss the changes you observe in the reaction of I synthesis of ammonia with preference to effect of pressure.

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11th Chemistry Monthly Test - 3 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Monthly Test - 3 ( Physical and Chemical Equilibrium )-Aug 2020

Part - A

Generic 2 - Answer All Question

What is the Kc value for formation of HI at 700 K? Predict the extent of the reaction?

Write the Kc for the reaction CO2(g) + H2O(l) \(\leftrightharpoons \) H+(aq)+ HCO3-(aq).

What are the different types of equilibrium? Explain with example?

Define reaction quotient.

Consider the following reactions, a) H2(g) + I2(g) ⇌ 2 HI b) CaCO3 (s) ⇌ CaO (s) + CO2(g) c) S(s) + 3F2 (g) ⇌ SF6 (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.

A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium partial pressure of HI(g) is 0.04 atm. What is K, for the given equilibrium? 2HI(g)u21cc H2(g) +I2(g)

2CO(g) +O2(g) u21cc 2CO2 at 1000 K. What is the Kc for this reaction? Predict the extent of this reaction.

Derive the relation between KP and KC.

"At constant volume addition of inert gas has no effect on equilibrium" - Justify

Write the expressions of equilibrium constants in terms of partial pressure and active masses for \(2{ BrCl }_{ \left( g \right) }\rightleftharpoons { Br }_{ 2\left( g \right) }+{ Cl }_{ 2\left( g \right) }\)

For the reaction,\({ A }_{ \left( g \right) }+{ B }_{ \left( s \right) }\rightleftharpoons { C }_{ \left( g \right) }+{ D }_{ \left( g \right) }\) Kc = 50 mol lit-1at 127°C. Calculate Kp'

Equilibrium constant K; for the reaction, N2(g) + 3H2(g)u21cc 2NH3(g) at 500 K is 0.06l. At particular time, the analysis shows that the composition of the reaction mixture is 3.0 mol L-1 of N2; 2.0 mol L-1 of H3; 0.50 mol L-1 of NH3. Is the reaction at equilibrium?

When will be KP < KC? Give two example

Part - B

Generic 3 - Answer All Question

Give three examples for solid vapour equilibrium.

What happens when the concentration of H2 and I2 are increased in the reaction \({ H }_{ 2 }+{ I }_{ 2 }\rightleftharpoons 2HI?\)

Consider the reaction, N2(g) + 3H2(g) u21cc 2NH3(g). Explain the effect of pressure on this equilibrium reaction.

Oxidation of nitrogen monoxide was studied at 200o 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 KP value.

How does oxygen exchanges between maternal and fetal blood in a pregnant woman?

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

The value of Kc for the reaction

At a certain temperature and total pressure of 105 Pa, iodine vapours contain 40% by volume of iodine atoms in the equilibrium I2(g) u21cc 2I(g). Calculate Kp for the equilibrium

Explain the effect of temperature on the following equilibrium reaction. N2(g) + 3H2Cg)u21cc 2NH3(g)Δ H = - 92.2 kJ.

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

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 500o C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate KC and KP.

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

Discuss the changes you observe in the reaction of I synthesis of ammonia with preference to effect of pressure.

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What is the K_c value for formation of HI at 700 K? Predict the extent of the reaction?

Write the Kc for the reaction CO₂(g) + H₂O(l) \(\leftrightharpoons \) H^+(aq)+ HCO₃^-(aq).

Consider the following reactions,
a) H₂(g) + I₂(g) ⇌ 2 HI
b) CaCO₃ (s) ⇌ CaO (s) + CO₂(g)
c) S(s) + 3F₂ (g) ⇌ SF₆ (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.

A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium partial pressure of HI(g) is 0.04 atm. What is K, for the given equilibrium?
2HI(g)u21cc H₂(g) +I₂(g)

2CO(g) +O₂(g) u21cc 2CO₂ at 1000 K. What is the Kc for this reaction? Predict the extent of this reaction.

Derive the relation between K_P and K_C.

Write the expressions of equilibrium constants in terms of partial pressure and active masses for
\(2{ BrCl }_{ \left( g \right) }\rightleftharpoons { Br }_{ 2\left( g \right) }+{ Cl }_{ 2\left( g \right) }\)

For the reaction,\({ A }_{ \left( g \right) }+{ B }_{ \left( s \right) }\rightleftharpoons { C }_{ \left( g \right) }+{ D }_{ \left( g \right) }\) K_c = 50 mol lit^-1at 127°C. Calculate K_p'

Equilibrium constant K; for the reaction, N₂(g) + 3H₂(g)u21cc 2NH₃(g) at 500 K is 0.06l. At particular time, the analysis shows that the composition of the reaction mixture is 3.0 mol L^-1 of N²; 2.0 mol L^-1 of H₃; 0.50 mol L^-1 of NH³. Is the reaction at equilibrium?

When will be K_P < K_C? Give two example

What happens when the concentration of H₂ and I₂ are increased in the reaction \({ H }_{ 2 }+{ I }_{ 2 }\rightleftharpoons 2HI?\)

Consider the reaction, N₂(g) + 3H₂(g) u21cc 2NH₃(g). Explain the effect of pressure on this equilibrium 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.

At a certain temperature and total pressure of 10⁵Pa, iodine vapours contain 40% by volume of iodine atoms in the equilibrium I₂(g) u21cc 2I(g). Calculate K_p for the equilibrium

Explain the effect of temperature on the following equilibrium reaction.
N₂(g) + 3H₂Cg)u21cc 2NH₃(g)Δ H = - 92.2 kJ.

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

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.

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