CBSE Class 11 Chemical Equilibrium — practice questions
73 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice CBSE Class 11 Chemical Equilibrium in the app →According to VSEPR theory, the shape of a molecule is determined byThe hybridisation of carbon in methane (CH₄) isWhich molecule is non-polar despite having polar bonds?The bond order of the oxygen molecule O₂ (by molecular orbital theory) isA coordinate (dative) bond differs from a normal covalent bond in thatWhich species has sp hybridisation on the central atom?As bond order increases, bond lengthAn ionic bond forms byThe shape of NH₃ is pyramidal rather than planar becauseWhich has the highest dipole moment?Among the following, which is paramagnetic?Formal charge on an atom = Per NCERT §6.1, equilibrium in a physical or chemical process is best described as which kind?Per NCERT §6.1.5, equilibrium can only be attained under which condition?Per NCERT §6.3 eqn 6.4, for the reaction aA + bB ⇌ cC + dD, the equilibrium constant Kc is expressed as which?Per NCERT §6.3 eqn 6.8, if Kc is the equilibrium constant of a forward reaction, the equilibrium constant of tPer NCERT §6.3, if a balanced chemical equation is MULTIPLIED throughout by n, the new equilibrium constant eqPer NCERT §6.4.1 eqn 6.15, the relationship between Kp and Kc for a gaseous reaction is which?Per NCERT §6.4.1, for the reaction H₂(g) + I₂(g) ⇌ 2 HI(g), the relation between Kp and Kc is which?Per NCERT §6.4.1, for N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g), the relation between Kp and Kc is which?Per NCERT Problem 6.1, given [N₂] = 1.5×10⁻² M, [H₂] = 3.0×10⁻² M, [NH₃] = 1.2×10⁻² M at 500 K, what is Kc forPer NCERT §6.5, for the heterogeneous equilibrium CaCO₃(s) ⇌ CaO(s) + CO₂(g), the equilibrium constant Kp equaPer NCERT §6.5, why do pure solids and pure liquids NOT appear in the expression for the equilibrium constant?Per NCERT §6.4.1, the units of Kp for N₂O₄(g) ⇌ 2 NO₂(g) (when partial pressures are in bar) are which?Per NCERT §6.6.2, if the reaction quotient Q is LESS than the equilibrium constant K, the reaction proceeds inPer NCERT eqn 6.22, the relation between standard Gibbs energy change ΔG° and equilibrium constant K is which?Per NCERT §6.7, if ΔG° is negative for a reaction, the value of equilibrium constant K satisfies which?Per NCERT §6.6.1, if Kc > 10³, what does this magnitude indicate about the reaction at equilibrium?Per NCERT §6.8, Le Chatelier's principle states that a stress on a system at equilibrium causes the system to Per NCERT §6.8.2, for the equilibrium CO(g) + 3 H₂(g) ⇌ CH₄(g) + H₂O(g), an INCREASE in pressure (decrease in Per NCERT §6.8.3, adding an INERT gas (e.g. argon) at CONSTANT VOLUME to a gaseous equilibrium has what effectPer NCERT §6.8.4, for an EXOTHERMIC reaction, what is the effect of raising the temperature on the equilibriumPer NCERT §6.8.5, what is the effect of adding a CATALYST on the position of equilibrium and on K?Per NCERT §6.8.5 + Table 6.5, for N₂ + 3H₂ ⇌ 2NH₃ (ΔH < 0), the Haber process operates at moderately high tempPer NCERT Problem 6.10, given ΔG° = 13.8 kJ/mol at 298 K for glucose phosphorylation, the value of Kc is closePer NCERT Problem 6.5, given Kc = 3.75×10⁻⁶ at 1069 K for 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g), the value of Kp is cloPer NCERT §6.10.1, in the ARRHENIUS concept, an acid is defined as a substance which does which on dissolving Per NCERT §6.10.2, in the BRØNSTED-LOWRY concept, an acid is defined as which kind of species?Per NCERT §6.10.3, in the LEWIS concept (G.N. Lewis, 1923), a base is defined as which kind of species?Per NCERT §6.10.2, what is the conjugate base of the Brønsted acid HSO₄⁻?Per NCERT §6.10.2 + Problem 6.13, what is the conjugate acid of the Brønsted base NH₃?Per NCERT §6.10.2, the conjugate base of a STRONG acid is necessarily which kind of base?Per NCERT §6.11.1 eqn 6.28, the ionic product of water Kw = [H⁺][OH⁻] at 298 K has which value?Per NCERT §6.11.1, Kw varies with which physical variable, since it is itself an equilibrium constant?Per NCERT §6.11.2, the pH of a solution is defined as which expression?Per NCERT eqn 6.29, at 298 K, what is the value of pH + pOH for any aqueous solution?Per NCERT §6.11.2, the pH of a 10⁻² M HCl solution (strong acid, fully dissociated) is closest to which value?Per NCERT §6.11.2, the pH of a 10⁻⁴ M NaOH solution (strong base, fully dissociated) is closest to which valuePer NCERT §6.12.5 (common-ion effect), addition of CH₃COONa to a solution of CH₃COOH does what to the degree oPer NCERT §6.13 (Henderson-Hasselbalch, eqn 6.40-6.41), the pH of an acidic buffer is given by which expressioPer NCERT §6.13, when [salt] = [acid] in a buffer, the pH of the buffer equals which quantity?Per NCERT §6.13, a buffer made from acetic acid and sodium acetate (pKa ≈ 4.76) at equimolar concentrations giPer NCERT §6.13, a buffer made from ammonia and ammonium chloride (pKb ≈ 4.75; conjugate-acid pKa ≈ 9.25) at ePer NCERT §6.13, on DILUTING a buffer solution, what happens to the buffer pH (to first approximation)?Per NCERT §6.14, for a sparingly soluble salt MX(s) ⇌ M⁺(aq) + X⁻(aq) with molar solubility S, the SOLUBILITY Per NCERT §6.14, for a salt M₂X(s) ⇌ 2 M⁺(aq) + X²⁻(aq) of molar solubility S, the SOLUBILITY PRODUCT Ksp equaPer NCERT §6.14, for a salt A₂X₃(s) ⇌ 2 A³⁺(aq) + 3 X²⁻(aq) of molar solubility S, the SOLUBILITY PRODUCT Ksp Per NCERT §6.14, comparing the ionic product Qsp with Ksp, PRECIPITATION of the salt occurs under which conditPer NCERT §6.14, the SOLUBILITY of a sparingly soluble salt in the presence of a COMMON ION (e.g. AgCl in NaClPer NCERT §6.14 (definition), what is the molar SOLUBILITY S of barium sulphate at 298 K, given Ksp(BaSO₄) = 1For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$, the equilibrium constant is:Increasing pressure on the equilibrium $N_2 + 3H_2 \rightleftharpoons 2NH_3$ shifts it:The pH of a solution with $[H^+] = 10^{-3}$ M is:A buffer is made by mixing $0.1$ M acetic acid ($pK_a = 4.74$) with $0.1$ M sodium acetate. The pH is:For the reaction 2A + B ⇌ 3C + D, the equilibrium constant Kc is:In the synthesis of ammonia (N2 + 3H2 ⇌ 2NH3 + heat), increasing the TEMPERATURE will:In an exothermic reaction, as temperature INCREASES, the equilibrium constant Kc:According to the Bronsted-Lowry theory, an acid is:A solution with pH = 4 is:A BUFFER solution is best described as:A solution of NH4Cl (ammonium chloride) in water is:If the solubility of AgCl is s mol/L in pure water, then its Ksp is:Adding NaCl (sodium chloride) to a saturated AgCl solution will: