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Q: Extent of completion of 2Cl₂O ⇌ products depends on Kc; mostly Cl₂ when: (ETEA 2010)

A) Kc very large

B) Kc very small

C) Kc moderate

D) Kc = 1

Q: Mass-action forces proportional to active masses is statement of: (ETEA 2012)

A) Raoult’s law

B) Le-Chatelier principle

C) Conservation of energy

D) Law of mass action

Q: Why simple crystallization is NOT used for NaCl purification? (ETEA 2012)

A) Solubility constant with temp

B) Less soluble

C) increases with temp

D) Decreases with temperature

Q: If Kc is large, at equilibrium: (ETEA 2012)

A) Reactant concentration high

B) Product concentration low

C) Product concentration high

D) Reactant & product equal

Q: For endothermic reaction N₂ + O₂ ⇌ 2NO, increasing temperature: (ETEA 2012)

A) Shifts backward

B) No change

C) Shifts forward

D) All

Q: Haber process is best represented by: (ETEA 2013)

A) N₂ + 3H₂ → 2NH₃

B) NH₃ + 3OH⁻ → 2NH₂⁻

C) MgN₂ + H₂O →…

D) Li₃N + H₂O → …

Q: AB ⇌ A⁺ + B⁻, Ksp = 4×10⁻¹²; molar solubility is: (ETEA 2013)

A) 4×10⁻¹²

B) 2×10⁻⁶

C) 8×10⁻⁶

D) 2×10⁻⁴

Q: Guldberg & Waage stated: (ETEA 2014)

A) Acid-base equilibria

B) Periodic law

C) Law of mass action

D) Rule of multiplicity

Q: Purification of NaCl by HCl is based on: (ETEA 2014)

A) Volatility

B) Common-ion effect

C) Ionization

D) None

Q: For NH₄OH ⇌ NH₄⁺ + OH⁻, adding NH₄Cl shifts equilibrium: (ETEA 2015)

A) Right

B) Left

C) No change

D) Reached quickly

Q: For the gaseous equilibrium N₂(g) + 3H₂(g) ⇌ 2NH₃(g) at 25 °C, the relationship between Kp and Kc is: (ETEA 2016)

A) Kp = Kc

B) Kp > Kc

C) Kp < Kc

D) None

Q: Excess of Ag₂CrO₄ was dissolved in distilled water its solubility was found to be 1.3×10⁻⁴mol dm⁻³ what is the solubility product (ETEA 2017)

A) Ksp = [1.3×10⁻⁴]²[1.3×10⁻⁴]

B) Ksp = [2.6×10⁻⁴]²[1.3×10⁻⁴]

C) Ksp = [1.3×10⁻⁵][7.3×10⁻⁵]

D) Ksp = [1.3×10⁻⁴]²

Q: For PCl₅ ⇌ PCl₃ + Cl₂, Kp=0.85 at 500 K. Kc equals: (ETEA 2017)

A) 0.85/(0.082×500)

B) 0.82

C) 0.85×500

D) 0.85/0.82

Q: Solubility of AgCr₂O₇ at 25 °C = 2×10⁻⁵ M. Ksp = (ETEA 2018)

A) 3.2×10⁻¹⁰

B) 4.0×10⁻¹⁰

C) 8.0×10⁻²⁶

D) 8.0×10⁻¹⁰

Q: For CO + O₂ ⇌ CO₂: (ETEA 2018)

A) Kp > Kc

B) Kp < Kc

C) Kp = Kc

D) Kp ≥ Kc

Q: initially one mole each N₂ and O₂ were made to react as, N₂ +O₂⇌ 2NO if at equilibrium 0.25 moles of O2 is present the equilibrium concentration of NO will be: (ETEA 2018)

A) 0.50

B) 0.125

C) 1.50

D) 0.75

Q: Highest Kc among: (ETEA 2018)

A) H₂ + I₂ ⇌ 2HI

B) Esterification

C) Cl + Cl → Cl₂

D) C + 2H₂ → CH₄

Q: Heating CaCO₃ in open container; increasing pressure: (ETEA 2018)

A) Shifts right

B) Shifts left

C) No effect

D) System not at equilibrium

Q: If Kc is very small: (ETEA 2018)

A) Reactants large

B) Products appreciable

C) Both appreciable

D) Equilibrium impossible

Q: Adding NH₄Cl to (NH₄)₂CO₃ decreases: (ETEA 2018)

A) NH₄⁺ concentration

B) CO₃²⁻ concentration

C) No change in CO₃²⁻

D) No change at all