CBSE Class 11 (Science) Equilibrium — practice questions
120 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice CBSE Class 11 (Science) Equilibrium in the app →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:For the gas-phase reaction $2\mathrm{SO_2(g)} + \mathrm{O_2(g)} \rightleftharpoons 2\mathrm{SO_3(g)}$, the valAt equilibrium, the rates of the forward and reverse reactions are:In a saturated sugar solution, the rate of dissolution equals the rate of:An equilibrium in which reactants and products are in different phases is:For a heterogeneous equilibrium to exist, there must also be present some:The equilibrium constant for the reverse reaction is the:The quantity used to predict the direction a reaction will take is the:Q differs from K because the concentrations used in Q are:Q is useful because comparing it with K predicts the reaction's:Which principle predicts the effect of changing conditions on equilibrium?Adding more of a reactant shifts the reaction in the direction that:According to Arrhenius, acids dissociate in water to give:According to Arrhenius, bases produce in water:A hydrogen ion is essentially a bare:The bare hydrogen ion binds to a water molecule at its:A Bronsted-Lowry acid is a substance capable of donating:Thomas M. Lowry was a chemist from:The pH scale is:The pH of a solution is defined as the negative logarithm to base:A solution with a hydrogen ion concentration of 10 to the minus 7 M has a pH of:A NaOH solution with a hydronium concentration of 10 to the minus 10 M has a pH of:Suppressing ionisation by adding an ion already present is the:Acetic acid together with sodium acetate acts as a:Ice and water stay in equilibrium in an insulated flask at atmospheric pressure at which temperature?Ice and water coexist at 1 atm at which temperature?A liquid with higher vapour pressure at a set temperature isWater and its vapour are in equilibrium at 100 degrees C at what pressure?How does the boiling point of water change at high altitude?Solid iodine in a closed vessel fills it with what colour of vapour?Adding radioactive sugar to a saturated sugar solution shows that equilibrium isA solution in which no more solute dissolves at a given temperature is calledThe fizzing of carbon dioxide on opening a soda bottle is governed by which law?Ice and water at 1 atm can stay in equilibrium at how many temperatures?For aA + bB to cC + dD, the expression for Kc isIf Kc for H2 + I2 to 2HI is 57.0 at 700 K, Kc for 2HI to H2 + I2 isIf all coefficients in a balanced equation are halved, the new Kc equalsWhich relation connects Kp and Kc for a gaseous equilibrium?For N2(g) + 3H2(g) to 2NH3(g), the value of dn used in Kp = Kc(RT)^dn isFor which equilibrium is Kp equal to Kc?For 2NOCl(g) to 2NO(g) + Cl2(g), what is dn?What are the units of Kc for N2(g) + 3H2(g) to 2NH3(g)?For CaCO3(s) to CaO(s) + CO2(g), the equilibrium constant Kp equalsThe value of Kc for a reaction at a fixed temperature depends onA very large Kc, say above 1000, suggests that at equilibriumIf the reaction quotient Qc is greater than Kc, the reaction willFor H2 + I2 to 2HI (Kc = 57.0), a mix has [H2] 0.10 M, [I2] 0.20 M, [HI] 0.40 M. Qc isWhen Qc is less than Kc, the net reaction moves towardWhich equation links the standard Gibbs energy change with K?A reaction has dG0 = +13.8 kJ/mol at 298 K. Its Kc is aboutLe Chatelier's principle says that a change in conditions at equilibrium makes the systemIn the Haber process, removing ammonia as it forms shifts the equilibriumFe3+ and SCN- form a deep red complex. Adding Hg2+ to this mix willRaising pressure on N2 + 3H2 to 2NH3 at fixed temperature shifts it towardChanging pressure has no effect on the equilibrium position ofAdding an inert gas to an equilibrium mixture at constant volume willRaising the temperature of an exothermic equilibrium causes its K toCooling an NO2 and N2O4 mixture in a freezing mixture makes its brown colourA catalyst added to a reaction at equilibrium willCompared with its conjugate base, a conjugate acid hasIn NH3 + H2O to NH4+ + OH-, the conjugate acid of NH3 isWhen water donates a proton to ammonia, its conjugate base formed isWhat is the conjugate acid of the amide ion NH2-?If a Bronsted acid is very strong, its conjugate base isIn the Lewis concept, a base is a species thatBF3 has no proton yet acts as an acid by reacting with NH3. It is aA bare proton in water bonds to a water molecule and exists asAn acid-base equilibrium lies on the side that formsA very weak acid has a conjugate base that isIn pure water at 298 K, the hydronium ion concentration isA NaOH solution has [OH-] = 10^-4 M at 25 C. Its pH isIf the pH of a solution falls by one unit, its H+ concentration