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7.EQUILIBRIUM (1.)What is the pH of 10−2 M H2SO4? (a.) 1.600 (b.) 2 (c.) 10−2 (d.) 1.6990 (2.)For the reaction, H2 (g) + I2(g) ⟶ 2HI(g), the equilibrium constant Kp changes with (a.) Total pressure (b.) Catalyst (c.) The amount H2 and I2 (d.) Temperature (3.)For the reaction, C(s) + CO2 (g) ⇌ 2CO(g), the principle pressure of CO2 and CO are 2.0 and 4.0 atm respectively at equilibrium. The Kp for the reaction is (a.) 2.0 (b.) 4.0 (c.) 8.0 (d.) 1.6 (4.)Which of the following is not a buffer solution? (a.) 100 mL 0.1 M CH3COOH + 50 mL 0.1 M CH3COONa (b.) 100 mL 0.1 M CH3COOH + 50 mL 0.1 M NaOH (c.) 50 mL 0.1 M CH3COOH + 100 mL 0.1 M NaOH (d.) 100 mL 0.1 M NH4OH + 50 mL 0.1 M HCl (5.)In the thermal decomposition of potassium chlorate given as 2KClO3 → 2KCl + 3O2, law of mass action (a.) Can be applied (b.) Cannot be applied (c.) Can be applied at low temperature (d.) Can be applied at high temperature and pressure (6.)50 mL of 0.1 M HCl and 50 mL of 0.2 M NaOH are mixed. The pH of the resulting solution is (a.) 1.30 (b.) 4.2 (c.) 12.70 (d.) 11.70 (7.)The pH of a buffer solution of 0.1 M NH4OH [pKb = 5.0] and 0.01 M NH4Cl is (a.) 1 (b.) 4 (c.) 10 (d.) 13 (8.)The aqueous solutions of HCOONa, C6H5NH3Cl and KCN are respectively (a.) Acidic, acidic, basic (b.) Acidic, basic, neutral (c.) Basic, neutral, neutral (d.) Basic, acidic, basic (9.)The solubility product of Ag2CrO4is 32 × 10−12 . What is the concentration of CrO4 − ions in that solution? (a.) 2 × 10−4M (b.) 16 × 10−4M (c.) 8 × 10−4M (d.) 8 × 10−8M (10.)The strongest conjugate base is (a.) NO3 − (b.) Cl − (c.) SO4 2− (d.) CH3COO− (11.)0.365 g of HCl gas was passed through 100 cm3 of 0.2 M NaOH solution. The pH of the resulting solution would be (a.) 1 (b.) 5 (c.) 8 (d.) 13 (12.)Solubility product of Mg(OH)2 at ordinary temperature is 1.96 × 10−11. pH of a saturated solution of Mg(OH)2 will be (a.) 10.53 (b.) 8.47 (c.) 6.94 (d.) 3.47 (13.)Which one of the following substances has the highest proton affinity? (a.) H2O (b.) H2S (c.) NH3 (d.) CH3COOH (14.)For the following reaction in gaseous phase CO(g) + 1 2 O2(g) ⟶ CO2(g)Kp⁄Kc is (a.) (RT) 1⁄2 (b.) (RT) −1⁄2 (c.) (RT) (d.) (RT) −1
(15.)To a 10 mL of 10−3 N H2SO4 solution water has been added to make the total volume of 1 L. Its pOH would be (a.) 9 (b.) 3 (c.) 12 (d.) 4 (16.)pH of solution can be expressed as (a.) −loge [H +] (b.) − log10[H +] (c.) loge [H +] (d.) log10[H +] (17.)In the reaction, H2 (g) + Cl2(g) ⇌ 2HCl(g) (a.) Kp ≠ Kc (b.) Kp = Kc (c.) Kp > Kc (d.) Kp < Kc (18.)The indicator used in titration of oxalic acid with caustic soda solution is (a.) Methyl orange (b.) Methyl red (c.) Fluorescein (d.) Phenolphthalein (19.)Which of the following salt does not get hydrolysed in water? (a.) KClO4 (b.) NH4Cl (c.) CH3COONa (d.) None of these (20.)0.5 M ammonium benzoate is hydrolysed to 0.25 percent. Hence, its hydrolysis constant is (a.) 2.5 × 10−5 (b.) 1.25 × 10−5 (c.) 3.125 × 10−6 (d.) 6.25 × 10−6 (21.)The equilibrium constant Kp for the reaction, H2 (g) + I2(g) ⇌ 2HI(g) is (a.) More than one (b.) Less than one (c.) Equal to Kc (d.) Zero (22.)Theory of ionisation was given by (a.) Rutherford (b.) Graham (c.) Faraday (d.) Arrhenius (23.)The rate constant for forward reaction and backward reaction of hydrolysis of ester are 1.1 × 10−2 and 1.5 × 10−3 per minute respectively. Equilibrium constant for the reaction is CH3COOC2H5 + H2O ⇌ CH3COOH + C2H5OH (a.) 33.7 (b.) 7.33 (c.) 5.33 (d.) 33.3 (24.)The equilibrium which remains unaffected by change in pressure of the reactants is (a.) N2 (g) + O2 (g) ⇌ 2NO(g) (b.) 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) (c.) 2O3 (g) ⇌ 3O2 (g) (d.) 2NO2 ⇌ N2O4(g) (25.)Calculate the pH of a solution in which hydrogen ion concentration is 0.005 g-equi/L? (a.) 2.3 (b.) 2.8 (c.) 2.9 (d.) 2.6 (26.)The strongest Lewis base in the following is (a.) CH3 − (b.) F − (c.) NH2 − (d.) OH − (27.)Pure ammonia is placed in a vessel at temperature where its dissociation constant (α) is appreciable. At equilibrium, (a.) Kp does not change significantly with pressure (b.) α does not change with pressure (c.) Concentration of NH3 does not change with pressure (d.) Concentration of H2 is less than that of N2 (28.)A certain buffer solution contains equal concentration of X −and HX. The Ka for HXis 10−8 . The pH of the buffer is (a.) 3 (b.) 8 (c.) 11 (d.) 14 (29.)In the manufacture of ammonia by Haber’s process, N2 (g) + 3H2 ⇌ 2NH3 (g) + 92.3 kJ Which of the following condition is unfavourable? (a.) Increasing the temperature (b.) Increasing the pressure (c.) Reducing the temperature (d.) Removing ammonia as it is formed (30.)What is the effect of having the pressure by doubling the volume on the following system at 500°C? H2 (g) + I2(g) ⇌ 2HI(g) (a.) Shift to product side (b.) Shift to reactant side (c.) Liquifactionof HI (d.) No effect
(31.)Which of the following is not a physical equilibrium? (a.) Ice ⇌ Water (b.) I2(s) ⇌ I2(g) (c.) S(l) ⇌ S(g) (d.) 3O2 ⇌ 2O3 (32.)A mixture of 0.3 mole of H2 and 0.3 mole of I2 is allowed to react in a 10 L evacuated flask at 500°C. The reaction is H2 + I2 ⇌ 2HI, the K is found to be 64. The amount of unreacted I2 at equilibrium is (a.) 0.03 mol (b.) 0.06 mol (c.) 0.09 mol (d.) 3.6 mol (33.)Conjugate base of HSO4 − is (a.) SO4 2− (b.) H2SO4 (c.) H3SO4 + (d.) None of these (34.)Which one is strongest electrolyte in the following? (a.) NaCl (b.) CH3COOH (c.) NH4OH (d.) C6H12O6 (35.)Which of the following is a Lewis base? (a.) NaOH (b.) NH3 (c.) BCl3 (d.) All of these (36.)In qualitative analysis, in order to detect second group basic redical, H2S gas is passed in the presence of dilute HCl to (a.) Increase the dissociation of H2S (b.) Decrease the dissociation of salt solution (c.) Decrease the dissociation of H2S (d.) Increase the dissociation of salt solution (37.)The pH of a solution is 4. The hydrogen ion concentration of the solution in mol/L is (a.) 9.5 (b.) 10−4 (c.) 104 (d.) 10−2 (38.)The pH value of an acid is 5 and its concentration is 1 M. What is the value of Ka for the acid? (a.) 10−7 (b.) 10−5 (c.) 10−10 (d.) 10−8 (39.)A reaction is, A + B → C + D. Initially we start with equal concentrations of Aand B. At equilibrium, we find the moles of C are two times of A. What is the equilibrium constant of the reaction? (a.) 2 (b.) 4 (c.) 1 2 (d.) 1 4 (40.)On adding 0.1 M solution each of [Ag +],[Ba 2+],[Ca 2+]in a Na2SO4 solution, species first precipitated is [Ksp BaSO4 = 10−11 ,Ksp CaSO4 = 10−6 ,Ksp AgSO4 = 10−5 ] (a.) Ag2SO4 (b.) BaSO4 (c.) CaSO4 (d.) All of these (41.)Amines behave as (a.) Lewis acid (b.) Lewis base (c.) Aprotic acid (d.) Neutral compound (42.)Hydrogen ion concentration in mol/L in a solution of pH=5.4 will be (a.) 3.98 × 10−6 (b.) 3.68 × 10−6 (c.) 3.88 × 106 (d.) 3.98 × 108 (43.)When hydrogen molecules decomposed into it’s atoms which conditions gives maximum yield of H atom? (a.) High temperature and low pressure (b.) Low temperature and high pressure (c.) High temperature and high pressure (d.) Low temperature and low pressure (44.)Which one of the following is least likely to act as a Lewis base? (a.) I + (b.) I (c.) SCl2 (d.) PCl3 (45.)The pH of the solution 5 mL M 5 HCl + 10 mL of M 10 NaOH is (a.) 5 (b.) 3 (c.) 7 (d.) 8 (46.)The strongest Bronsted base is (a.) ClO3 −
(b.) ClO2 − (c.) ClO4 − (d.) ClO − (47.)If pressure increases then its effect on given equilibrium 2NO(g) ⇌ N2 (g) + O2(g) is shift in (a.) Forward direction (b.) Backward direction (c.) No effect (d.) None of these (48.)The solubility product of a sparingly soluble salt AB at room temperature is 1.21 × 10−6 . Its molar solubility is (a.) 1.21 × 10−6 (b.) 1.21 × 10−3 (c.) 1.1 × 10−4 (d.) 1.1 × 10−3 (49.)Given pH of a solution A is 3 and it is mixed with another solution B having pH 2. After mixing are resultant pH of the solution will be (a.) 3.2 (b.) 1.9 (c.) 3.4 (d.) 3.5 (50.)Of the following which change will shift the reaction towards the product? I2 (g) ⇌ 2I(g), ∆H°r (298 K) = +150 kJ (a.) Increase in temperature (b.) Increase in total pressure (c.) Increase in concentration of I (d.) Decrease in concentration of I2 (51.)At a certain temperature, the dissociation constants of formic acid and acetic acid are 1.8 × 10−4 and 1.8 × 10−5 respectively. The concentration of acetic acid solution in which the hydrogen ion has the same concentration as in 0.001 M formic acid solution is equal to (a.) 0.01 M (b.) 0.001 M (c.) 0.1 M (d.) 0.0001 M (52.)The formation of SO3 takes place according to the following reaction, 2SO2 + O2 ⇌ 2SO3, ∆H = −45.2 kcal. The formation of SO3 is favoured by (a.) Increase of volume (b.) Increase in pressure (c.) Increase in temperature (d.) Removal of oxygen (53.)In which one of the following gaseous equilibria, Kp is less than Kc? (a.) N2O4 ⇌ 2NO2 (b.) 2SO2 + O2 ⇌ 2SO3 (c.) 2HI ⇌ H2 + I2 (d.) N2 + O2 ⇌ 2NO (54.)In the reaction, H2 + I2 ⇌ 2HI In a 2 I flask 0.4 moles of each H2 and I2 are taken. At equilibrium 0.5 moles of HI are formed. What will be the value of equilibrium constant Kc? (a.) 20.2 (b.) 25.4 (c.) 0.284 (d.) 11.1 (55.)The solubility of AgI in NaI solution is less than that in pure water because (a.) The temperature of the solution decreases (b.) Solubility product of AgI is less than that of NaI (c.) Of common ion effect (d.) AgI forms complex with NaI (56.)The equilibrium constant (Kp) for the reaction, PCl5 (g) → PCl3 (g) + Cl2(g) is 16. If the volume of the container is reduced to one half its original volume, the value of Kp for the reaction at the same temperature will be (a.) 8 (b.) 16 (c.) 32 (d.) 64 (57.)For the reaction, H2 + I2 ⇌ 2HI, the equilibrium concentration of H2,I2 and HI are 8.0, 3.0 and 28.0 mol/L respectively. The equilibrium constant is (a.) 28.34 (b.) 32.66 (c.) 34.78 (d.) 38.88 (58.)The solubility product of BaSO4is 1.5 × 10−9 . The precipitation in a 0.01 M Ba 2+ solution will start, on adding H2SO4of concentration (a.) 10−9 M (b.) 10−8 M (c.) 10−7 M (d.) 10−6 M (59.)For the reaction, CO(g) + Cl2 (g) ⇌ COCl2 (g),the Kp⁄Kc is equal to (a.) 1⁄RT (b.) RT (c.) √RT (d.) 1.0 (60.)NaOH(aq),HCl(aq)andNaCl(aq) concentration of each is 10−3 M. Their pH will be respectively