11th Chemistry Monthly Test - 4 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Monthly Test - 4 ( Physical and Chemical Equilibrium )-Aug 2020

Time : 2.00 Hours

Part - A

Generic 5 - Answer All Question

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

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

(i) Describe the effect of
(a) addition of H₂,
(b) addition of CH₃0H
(c) removal of CO
(d) removal ofCH₃OH on the equilibrium of
the reaction, \({ 2H }_{ 2(g) }+{ CO }_{ (g) }\rightleftharpoons { CH }_{ 3 }{ OH }_{ (g) }\)
(ii) What happens to an equilibrium in a reversible reaction if a catalyst is added to it?

Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) u21cc [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 equilibrium constant for the following reaction is 0.15 at 298 K and 1 atm pressure.
N₂O₄(g) u21cc 2NO₂(g);
ΔHº = 57.32 KJmol^-1
The reaction conditions are altered as follows.
a) The reaction temperature is altered to 100o C keeping the pressure at 1 atm, Calculate the equilibrium constant.

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

The atmospheric oxidation of NO
2NO(g) + O₂(g) u21cc 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 equilibrium for the dissociation of XY₂ is given as,
2XY₂ (g)\(\leftrightharpoons\) 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 KP is the dissociation equilibrium constant of XY₂.

At certain temperature and under a pressure of 4 atm, PCl₅ is 10% dissociated. Calculate the pressure at which PCls will be 20% dissociated at temperature remaining constant.

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)

At particular temperature K_C = 4 × 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) + \(\frac{3}{2}\) S₂(g)

Explain: How does the extent of reaction depend on K_c?

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11th Chemistry Monthly Test - 4 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Monthly Test - 4 ( Physical and Chemical Equilibrium )-Aug 2020

Part - A

Generic 5 - Answer All Question

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

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

Consider the following reaction Fe3+(aq) + SCN–(aq) u21cc [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 equilibrium constant for the following reaction is 0.15 at 298 K and 1 atm pressure. N2O4(g) u21cc 2NO2(g); ΔHº = 57.32 KJmol-1 The reaction conditions are altered as follows. a) The reaction temperature is altered to 100o C keeping the pressure at 1 atm, Calculate the equilibrium constant.

The equilibrium constant KP for the reaction N2(g) + 3H2(g) \(\leftrightharpoons\) 2NH3(g) is 8.19 × 102 at 298 K and 4.6 × 10–1 at 498 K. Calculate ΔHo for the reaction

The atmospheric oxidation of NO 2NO(g) + O2(g) u21cc 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 Kp of the reaction.

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

At certain temperature and under a pressure of 4 atm, PCl5 is 10% dissociated. Calculate the pressure at which PCls will be 20% dissociated at temperature remaining constant.

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 Kc value for PCl5 dissociation at 423 K is 2)

At particular temperature KC = 4 × 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) + \(\frac{3}{2}\) S2(g)

Explain: How does the extent of reaction depend on Kc?

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

Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) u21cc [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 equilibrium constant KP for the reaction
N₂(g) + 3H₂(g) \(\leftrightharpoons\) 2NH₃(g) is 8.19 × 10² at 298 K and 4.6 × 10^–1 at 498 K. Calculate ΔH^o for the reaction

The atmospheric oxidation of NO
2NO(g) + O₂(g) u21cc 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 equilibrium for the dissociation of XY₂ is given as,
2XY₂ (g)\(\leftrightharpoons\) 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 KP is the dissociation equilibrium constant of XY₂.

At certain temperature and under a pressure of 4 atm, PCl₅ is 10% dissociated. Calculate the pressure at which PCls will be 20% dissociated at temperature remaining constant.

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)

At particular temperature K_C = 4 × 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) + \(\frac{3}{2}\) S₂(g)

Explain: How does the extent of reaction depend on K_c?