Ncert -class 11- Chemistry-Unit 6 -Equilibrium Welcome to your Ncert -class 11- Chemistry-Unit 6 -Equilibrium 1. The aqueous solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride? Sugar releases more ions in water and increases conductance Both sugar and NaCl ionises partially in water thereby increasing the conductance NaCl ionises completely in water and increase in concentration of salt increases conductance. Both sugar and NaCl ionises completely in water thereby increasing the conductance None 2. 𝑂3 is prepared by subjecting 𝑂2 to silent electric discharge. The favourable conditions for the formation of ozone according to Le-chatlier's principle are high temperature, low pressure low temperature, high pressure high temperature, high pressure low temperature, low pressure None 3. The dynamic nature of chemical equilibrium can be demonstrated in the synthesis of ammonia by Haber.s process. Choose the appropriate option given below by using hydrogen isotope by maintaining high temperature and low pressure by using sulphur isotope by using deuterium isotope None 4. The initial rate of hydrolysis of methyl acetate (1.0M) by a weak acid (HA,1.0M) is 1/100th of that of a strong acid of(HX,1.0M) at 25ºC. The Ka of HA is $$1×10^{-4}$$ $$1×10^{-3}$$ $$1×10^{-5}$$ $$1×10^{-6}$$ None 5. The amino acid alanine has two isomers, 𝛼 alanine and 𝛽 alanine when equal masses of these two compound are dissolved in equal mass of a solvent, the solution of 𝛼 alanine freeze at relatively l; lower temperature, which forms 𝛼 alanine and 𝛽 alanine has the larger equilibrium constant for ionization? same for both 𝛽 alanine unpredictable α alanine None 6. What will be the ionisation constant of formic acid if its 0.01 M solution is 14.5% ionised? $$2.1×10^{-4}$$ 14.5 0.145 $$1.45×10^{-4}$$ None 7. For dissolution of solids in liquids, at a given temperature, the constant is mass of the solvent pressure mass of the solute solubility None 8. The reaction :$$MgCO_{3}(s)\rightleftharpoons MgO(s)+CO_{2}(g)$$ is in progress. if number of mole of MgO in the vessel is doubled at an instance? the moles of 𝐶𝑂2 present at equilibrium is havled the partial pressure of 𝐶𝑂2 in the vessel remains unchanged the reaction quotient , Q is doubled the reaction quotient , Q is havled None 9. For liquid ⇌ vapour equilibrium, at a given temperature, the constant is mass of a solvent solubility vapour pressure mass of a gas None 10. Pure NaCl is prepared by saturating a cold saturated solution of common salt in water with HCl gas. The principle used is Fractional distillation Common ion effect Displacement law Le Chatelier principle None 11. Solid ammonium carbamate dissociates as:$$NH_{2}COONH_{4(s)}\rightleftharpoons 2NH_{3(g)}+CO_{2(g)}$$In a closed vessel, solid ammonium carbamate is in equilibrium with its dissociation products. At equilibrium, ammonia is added such that the partial pressure of NH3 at new equilibrium equals the original total pressure. The ratio of total pressure at new equilibrium to that of original total pressure is: 1:1 3:4 27 : 31 31:27 None 12. Which of the following statement(s) is/are incorrect? When water is added to 𝐾𝐶𝑁, a reaction occurs because the 𝐶𝑁− ion is a strong proton acceptor. No reaction occurs when KCl is dissolved in water because neither 𝐾+ nor \(Cl^{-} \) can remove or accept proton from water. When water is added to sodium acetate, an acidic solution is produced because of the formation of free acetic acid from the action of water on CH3 COO- None 13. When NH4Cl is added to NH4OH solution, the dissociation of ammonium hydroxide is reduced. It is due to: Hydrolysis Common ion effect Oxidation Reduction None 14. If we place solid iodine in a closed vessel, after sometime the vessel gets filled up with violet vapour. When equilibrium is attained, the intensity of colour will be decreases increases constant no colour at all None 15. If 𝐾1 and 𝐾2 are the equilibrium constants for a reversible reaction at T1 K and T2K temperature, respectively (T 1<T 2 ) and the reaction takes place with neither heat evolution nor absorption, then K 1 <K 2 at high temperature K1>K2 at high temperature K 1 =K 2 only at high temperature 𝐾 1 = 𝐾 2 at any temperature None 16. Which of the following statements is correct? Equilibrium constant for a reaction with negative ΔH value decreases as the temperature increases The intensity of red colour increases when oxalic acid is added to a solution containing iron (III). nitrate and potassium thiocyanate. In equilibrium mixture of ice and water kept in perfectly insulated flask mass of ice and water does not change with time. On addition of catalyst the equilibrium constant value is not affected. None 17. For dissolution of gases in liquids, the concentration of a gas in liquid is. lower to the pressure of the gas as compared to the liquid proportional to the vapour pressure of the gas equal to the pressure of the gas in relation to the liquid proportional to the pressure of the gas over the liquid. None 18. In a system: A(s)⇒2B(g)+3C(g) if the concentration of C at equilibrium is increased by a factor of 2, it will cause the equilibrium concentration of B to decrease by two times the original value 8 times its original value 2√2 times its original value one half of its original value None 19. Which of the following processes will increase $$[OH^{−}] in NH_{4}OH$$ solution? Addition of water. Addition of 𝐻 𝐶 𝑙solution. Addition of solid 𝑁𝐻4𝑂𝐻 Addition of 𝑁 𝐻 4 𝐶 𝑙 solution None 20. the rates of transfer of molecules from ice into water and of reverse transfer from water into ice are equal at atmospheric pressure and 273 K. Both the processes occur simultaneously and at the same rate so that the amount of ice and water remains constant. This process is called dynamic equilibrium ionic equilibrium Liquid-Vapour Equilibrium Liquid-Gas Equilibrium None Time's up Please Share This Share this content Opens in a new window Opens in a new window Opens in a new window Opens in a new window Opens in a new window Opens in a new window Opens in a new window Opens in a new window Opens in a new window Opens in a new window Leave a Reply Cancel replyCommentEnter your name or username to commentEnter your email address to commentEnter your website URL (optional) Save my name, email, and website in this browser for the next time I comment.
