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BITSAT Equilibrium Constant — practice questions

Explore 50 free Equilibrium Constant questions in BITSAT Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Equilibrium Constant questions and exercises with answers

Showing questions 1–30 of 50.

Le Chatelier's principle says that if a system at equilibrium is disturbed, the system will shift in the direction that:Read the answer and worked solution →For the reaction aA + bB ⇌ cC + dD at equilibrium, the equilibrium constant Kc is:Read the answer and worked solution →For an exothermic reaction at equilibrium, increasing temperature will shift the equilibrium:Read the answer and worked solution →Le Chatelier's principle states that a system at equilibrium responds to a stress by:Read the answer and worked solution →For the reaction N2 + 3H2 ⇌ 2NH3, increasing pressure favours:Read the answer and worked solution →Relation between Kp and Kc for a gas reaction with Δn_gas = change in moles of gas:Read the answer and worked solution →For an endothermic reaction, increasing T shifts equilibrium:Read the answer and worked solution →For dissociation of weak acid HA in water: HA ⇌ H+ + A-. Equilibrium constant is called:Read the answer and worked solution →pH of a 0.01 M HCl solution:Read the answer and worked solution →pOH of a solution with pH = 8.5 (at 25°C):Read the answer and worked solution →Solubility product Ksp of AgCl is 1.6 × 10⁻¹⁰. Its solubility in pure water (mol/L):Read the answer and worked solution →For a buffer solution containing weak acid HA and its salt NaA, the pH is approximately:Read the answer and worked solution →At equilibrium for an exothermic reaction, increasing pressure (for gas reaction with Δn < 0):Read the answer and worked solution →At 500 K, Kc for N2 + 3H2 ⇌ 2NH3 is 60 (in mol⁻² L²). Kp at 500 K (R = 0.0821):Read the answer and worked solution →For weak acid HA with Ka = 10⁻⁵, [H+] in 0.1 M solution is approximately:Read the answer and worked solution →Buffer capacity is maximum when:Read the answer and worked solution →A weak base BOH has Kb = 1.8 × 10⁻⁵. pH of 0.1 M solution is approximately:Read the answer and worked solution →Solubility of CaF2 in water (Ksp = 4.0 × 10⁻¹¹):Read the answer and worked solution →For the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g), if initial pressure of PCl5 is P0 and degree of dissociation is α, total pressure at equilibrium:Read the answer and worked solution →For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), at equilibrium increasing pressure:Read the answer and worked solution →If K = 1 for a reaction, the standard free energy change ΔG°:Read the answer and worked solution →At 298 K, water has Kw = 10⁻¹⁴. Concentration of H+ in pure water:Read the answer and worked solution →At equilibrium, the ratio of forward to reverse reaction rates:Read the answer and worked solution →In a saturated solution of AgCl, [Ag+] = 1.26 × 10⁻⁵. If KNO3 is added (no common ion), solubility of AgCl:Read the answer and worked solution →For the reaction H2(g) + I2(g) ⇌ 2HI(g) with Kc = 50 at 800 K, if [H2] = [I2] = 0.01 M initially, equilibrium [HI]:Read the answer and worked solution →Degree of dissociation α of weak acid HA (Ka = 1.8 × 10⁻⁵) in 0.01 M solution:Read the answer and worked solution →Match each scientist to their contributionRead the answer and worked solution →Ionic or covalent?Read the answer and worked solution →Complete the driver of bond formationRead the answer and worked solution →Single, double and triple bondsRead the answer and worked solution →

Worked practice questions

Le Chatelier's principle says that if a system at equilibrium is disturbed, the system will shift in the direction that:

  1. Stops the reaction
  2. Reverses the reaction completely
  3. Amplifies the disturbance
  4. Opposes the change
Show answer and solution

Correct answer: D. Opposes the change

Le Chatelier's principle in plain English: a disturbed equilibrium pushes back. If you add more reactant, the forward reaction speeds up to consume some of it. If you raise temperature on an endothermic reaction, equilibrium shifts forward (absorbs heat). The system never amplifies the disturbance, never stops, and rarely runs to completion.

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For the reaction aA + bB ⇌ cC + dD at equilibrium, the equilibrium constant Kc is:

  1. [A][B][C][D]
  2. [A]ᵃ[B]ᵇ/[C]ᶜ[D]ᵈ
  3. Kp
  4. [C]ᶜ[D]ᵈ/[A]ᵃ[B]ᵇ
Show answer and solution

Correct answer: D. [C]ᶜ[D]ᵈ/[A]ᵃ[B]ᵇ

Kc = [C]ᶜ[D]ᵈ/[A]ᵃ[B]ᵇ where small letters are stoichiometric coefficients and the [] denotes molar concentrations at equilibrium.

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For an exothermic reaction at equilibrium, increasing temperature will shift the equilibrium:

  1. No effect
  2. Toward reactants
  3. Toward products
  4. Becomes irreversible
Show answer and solution

Correct answer: B. Toward reactants

By Le Chatelier's principle: for exothermic reactions, increasing T shifts equilibrium backward (towards reactants), as the system absorbs the added heat by reversing.

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More Chemistry topics

Chemical EquilibriumElectrochemistryCoordination CompoundsElectrochemical SeriesIdeal and Non-Ideal SolutionsIdeal SolutionsNon-Ideal SolutionsReactions in Aqueous Solution