Tuesday, 27 September 2016

Chapter 8 CHEMICAL EQUILIBRIUM MCQs

Chemistry 1st year Chapter 8 CHEMICAL EQUILIBRIUM 

Q.1 A reaction is reversible because
8
(a) reactants are reactive (b) products are reactive
(c) products are stable (d) reactants are stable
Q.2 A large value of Kc means that at equilibrium
(a)  less reactants and more products
(b) more reactants and less product
(c)  same amount
(d) none
Q.3 Extent to H2 + I2  2HI can be increased by
(a) increasing pressure (b) increasing product
(c) increasing temp (d) adding a catalyst
Q.4 Strength of an acid can be determined by
(a) PKa (b) PKp
(c) POH (d) PKw
Q.5 In an exothermic reversible reaction increase in temp shifts the equilibrium to
(a) reactant side (b) product side
(c) remains unchanged (d) none
Q.6 Units of Kw are
(a) mole dm–3 (b) mole2 dm–3
(c) mole2 dm–6 (d) mole2 dm–3
Q.7 A basic Buffer solution can be prepared by mixing
(a)  weak acid and its salt with strong base
(b) strong acid and its salt with weak base
(c)  weak base and its salt with strong acid
(d) strong base and its salt with weak acid
Q.8 Buffer action can be explained by
(a) common ion effect (b) law of mass action
(c) Le–Chatlier’s principle (d) all above
CHEMICAL EQUILIBRIUM
Q.9 Ionization of weak acid is expressed in term of following constant
(a) Kw (b) Kn
(c) Ka (d) Kb
Q.10 Solubility of Ca(OH)2 is exothermic. If solubility will increase
(a) at high temp (b) at low temp
(c) temp independent (d) none
Q.11 For which system does the equilibrium constant, Kc has units of concentration
(a) N2 + 3H2 2NH3 (b) H2 + I2 2 HI
(c) 2NO2 N2O4 (d) 2HF H2 + F2
Q.12 Which statement about the following equilibrium is correct
2SO2(g) + O2(g) 2SO3(g)  H = – 188.3 kJ mol–1
(a)  the value of Kp falls with a rise in temp
(b) the value of Kp falls with increasing pressure
(c)  adding V2O5 catalyst increase the equilibrium yield of sulphur trioxide
(d) the value of Kp is equal to Kc
Q.13 The PH of 10–3 mole dm–3 of an aqueous solution of H2SO4 is
(a) 3.0 (b) 2.7
(c) 2.0 (d) 1.5
Q.14 The solubility product of AgCl is 2.0 x 10–10 mole2 dm–6. The max concentration of Ag+ ions in the solution is
(a) 2.0 x 10–10 mol dm–3 (b) 1.41 x 10–5 mol dm–3
(c) 1.0 x 10–10 mol dm–3 (d) 4.0 x 10–20 mol dm–3
Q.15 An excess of aqueous silver nitrate to added to aqueous barium chloride and precipitate is removed by filtration what are the main ions in the filtrate
(a) Ag+ and NO only (b) Ag+ and Ba2+ and NO3
(c) Ba2+ and NO only (d) Ba+2 and NO and Cl–
Q.16 For N2 + 3H2 2NH3
(a) Kc = Kp (b) Kp = Kc RT
(c) Kp = Kc (RT)–2 (d) Kp = Kc (RT)–1
Q.17 H2 + I2 2HI
In the above equilibrium system, if the conc. of reactants of 25oC is increased, the value of Kc will
(a) increase (b) decrease
(c)  remains constant
(d) depends upon nature of reactants
Q.18 In a chemical reaction, equilibrium is said to have established when
(a)  opposing reactions stops
(b) concentrations of reactants and products are equal
(c)  rate constants of opposing reactions are equal
Q.19 The relation between Kc and Kp is
(a) Kc = Kp (RT) n (b) Kp = Kc (RT) n
(c) Kp = Kc (RT) n (d) Kp = Kc
Q.20 The precipitation occurs if the ionic concentration is
(a) less than Ksp (b) more than Ksp
(c) equal to Ksp (d) is present at any moment
Q.21 The PH of oranges is
(a) 3.5 (b) 3.1
(c) 4.6 (d) 4.2
Q.22 Which one of following solution have zero PH
(a) 1M HCl (b) 0.5 MH2SO4
(c) 0.1 M HNO3 (d) 1M CH3COOH
Q.23 The solubility product expression for BaF2 can be written as
(a) [Ba2+] [F–] (b) [Ba2+] [2F]
(c) [Ba2+] [F–]2 (d) [Ba+] [F–]2
Q.24 To prepare a buffer with PH close to 9.0, you could use a mixture of
(a)  NH4OH and NH4Cl
(b) CH3COOH and CH3COONa
(c)  HNO2 + NaNO2
(d) NaHCO3 + H2CO3
Q.25 For which reaction the numerical value of Kc and Kp are same
(a) N2 + 3H2 2NH3 (b) 2SO2 + O2 2SO3
(c) H2 + Cl2 2HCl (d) N2O4 2NO2
Q.26 For which system does the equilibrium constant Kc have units (mole dm–3)–1
(a) H2 + I2 2HI (b) N2 + 3H2 2NH3
(c)  2NO2 N2O4
(d) CH3COOH + C2H5OH CH3COOC2H5 + H2O
CHEMICAL EQUILIBRIUM
Q.27 What can affect the magnitude of equilibrium constant Kp of a reversible gaseous reaction
(a) temperature (b) pressure
(c) catalyst (d) none of above
Q.28 Which gas can change the PH towards acidic
(a) argon (b) carbon dioxide
(c) nitrogen (d) oxygen
Q.29 The solution having zero PH will be
(a) basic (b) high basic
(c) neutral (d) highly acidic
Q.30 A solution have H+ ions concentration 1 x 10–7 its PH will be
(a) acid (b) basic
(c) neutral (d) zero
Q.31 Which one of the following has highest PH
(a) 0.1 M HCl (b) 1.0 M HCl
(c) gastric juice (d) lemons
Q.32 Which PH is considered as basic
(a) 1 (b) 7
(c) 2 (d) 11
Q.33 The sum of PH and POH is
(a) 2 (b) 7
(c) 14 (d) 13.5
Q.34 A buffer solution can be prepared by mixing
(a)  a strong acid and weak base
(b) a weak acid and weak base
(c)  a strong acid and its salt
(d) a weak base and its salt with strong acid
Q.35 Law of mass action was presented by
(a) Henderson (b) Lewis
(c) Guldberg and Waage (d) Arrehenius
Q.36 The unit of Kc for reaction
N2 + O2 2NO
(a) mol dm–3 (b) mol–1 dm3
(c) mol–2 dm6 (d) no units
Q.37 PH of pure water is
(a) 3.2 (b) 4.2
(c) 7.0 (d) 0
Q.38 Which of following change will favour the formation of more SO3 at equilibrium
2SO2 + O2 2SO3 + heat
(a)  by adding SO3 at equilibrium
(b) by increasing temp
(c)  by decreasing temp
(d) by decreasing pressure
Q.39 When pressure is applied to the given equilibrium ice water which of the following will happen
(a)  more ice will be formed
(b) more water will be formed
(c)  equilibrium will not be disturbed
(d) water will formed
Q.40 Which of following change will favour the formation of more HI in the given reaction H2 + I2 2HI
(a)  increasing pressure
(b) decreasing pressure

(c)  by adding more HI
(d) by adding more H2 and I2 

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