CBSE Class 11 (Science) Chemical Equilibrium — practice questions
67 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice CBSE Class 11 (Science) 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 = As per your syllabus, equilibrium in a physical or chemical process is best described as which kind?As per your syllabus, equilibrium can only be attained under which condition?As per your syllabus, eqn 6.4, for the reaction aA + bB ⇌ cC + dD, the equilibrium constant Kc is expressed asAs per your syllabus, eqn 6.8, if Kc is the equilibrium constant of a forward reaction, the equilibrium constaAs per your syllabus, if a balanced chemical equation is MULTIPLIED throughout by n, the new equilibrium constAs per your syllabus, eqn 6.15, the relationship between Kp and Kc for a gaseous reaction is which?As per your syllabus, for the reaction H₂(g) + I₂(g) ⇌ 2 HI(g), the relation between Kp and Kc is which?As per your syllabus, for N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g), the relation between Kp and Kc is which?As per your syllabus, 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 for As per your syllabus, for the heterogeneous equilibrium CaCO₃(s) ⇌ CaO(s) + CO₂(g), the equilibrium constant KAs per your syllabus, the units of Kp for N₂O₄(g) ⇌ 2 NO₂(g) (when partial pressures are in bar) are which?As per your syllabus, if the reaction quotient Q is LESS than the equilibrium constant K, the reaction proceedAs per your syllabus, eqn 6.22, the relation between standard Gibbs energy change ΔG° and equilibrium constantAs per your syllabus, if ΔG° is negative for a reaction, the value of equilibrium constant K satisfies which?As per your syllabus, if Kc > 10³, what does this magnitude indicate about the reaction at equilibrium?As per your syllabus, adding an INERT gas (e.g. argon) at CONSTANT VOLUME to a gaseous equilibrium has what efAs per your syllabus, for an EXOTHERMIC reaction, what is the effect of raising the temperature on the equilibAs per your syllabus, what is the effect of adding a CATALYST on the position of equilibrium and on K?As per your syllabus, given ΔG° = 13.8 kJ/mol at 298 K for glucose phosphorylation, the value of Kc is closestAs per your syllabus, given Kc = 3.75×10⁻⁶ at 1069 K for 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g), the value of Kp is closAs per your syllabus, in the ARRHENIUS concept, an acid is defined as a substance which does which on dissolviAs per your syllabus, in the BRØNSTED-LOWRY concept, an acid is defined as which kind of species?As per your syllabus, in the LEWIS concept (G.N. Lewis, 1923), a base is defined as which kind of species?As per your syllabus, what is the conjugate base of the Brønsted acid HSO₄⁻?As per your syllabus, + Problem 6.13, what is the conjugate acid of the Brønsted base NH₃?As per your syllabus, the conjugate base of a STRONG acid is necessarily which kind of base?As per your syllabus, eqn 6.28, the ionic product of water Kw = [H⁺][OH⁻] at 298 K has which value?As per your syllabus, Kw varies with which physical variable, since it is itself an equilibrium constant?As per your syllabus, the pH of a solution is defined as which expression?As per your syllabus, eqn 6.29, at 298 K, what is the value of pH + pOH for any aqueous solution?As per your syllabus, the pH of a 10⁻² M HCl solution (strong acid, fully dissociated) is closest to which valAs per your syllabus, the pH of a 10⁻⁴ M NaOH solution (strong base, fully dissociated) is closest to which vaAs per your syllabus, addition of CH₃COONa to a solution of CH₃COOH does what to the degree of ionisation of aAs per your syllabus, the pH of an acidic buffer is given by which expression?As per your syllabus, when [salt] = [acid] in a buffer, the pH of the buffer equals which quantity?As per your syllabus, a buffer made from acetic acid and sodium acetate (pKa ≈ 4.76) at equimolar concentratioAs per your syllabus, on DILUTING a buffer solution, what happens to the buffer pH (to first approximation)?As per your syllabus, for a sparingly soluble salt MX(s) ⇌ M⁺(aq) + X⁻(aq) with molar solubility S, the SOLUBIAs per your syllabus, for a salt M₂X(s) ⇌ 2 M⁺(aq) + X²⁻(aq) of molar solubility S, the SOLUBILITY PRODUCT KspAs per your syllabus, for a salt A₂X₃(s) ⇌ 2 A³⁺(aq) + 3 X²⁻(aq) of molar solubility S, the SOLUBILITY PRODUCTAs per your syllabus, comparing the ionic product Qsp with Ksp, PRECIPITATION of the salt occurs under which cAs per your syllabus, what is the molar SOLUBILITY S of barium sulphate at 298 K, given Ksp(BaSO₄) = 1.1 × 10⁻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:At dynamic equilibrium:Equilibrium can be established in:For N₂ + 3H₂ ⇌ 2NH₃, Kc equals:Adding heat to an exothermic equilibrium shifts it:Kw at 25°C equals:A buffer solution: