ECAT Chemistry Chapter 8 Chemical Equilibrium Online Test With Answers

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ECAT Chemistry Chapter 8 Chemical Equilibrium Online Test

Sr. # Questions Answers Choice
1 At certain temperature, 50% of HI is dissociated into H2and I2the equilibrium constant is 1.0 3.0 0.5 0.25
2 Total pressure Amount of A<sub>2</sub>and B<sub>2</sub> Temperature Catalyst
3 In an exothermic reaction, a 10° rise in temperature will Decrease the value of equilibrium constant Double the value of K<sub>c</sub> Not produce any change in K<sub>c</sub> Produce some increase in K<sub>c</sub>
4 In which of the following cases, the reaction goes farthest to completion K = 10<sup>3</sup> K = 10<sup>-2</sup> K = 10 K = 10<sup>0</sup>
5 0.02 0.2 50 25
6 The state of equilibrium refers to State of rest Dynamic state Stationary state State of inertness
7 Two moles of HI was heated in a sealed tube at 440°C till the equilibrium was reached. HI was found to be 22% decomposed. The equilibrium constant for dissociation is 0.282 0.0796 0.0199 1.99
8 The avtive mass of 64 g of HI in a two litre flask would be 2 1 5 0.25
9 Which of the following factors will favour the reverse reaction in a chemical equilibrium? Increase in concentration of one of the reactants Increase in concentration of one of the products Removal of one of the products regularly None of these
10 Favour the formation of N<sub>2</sub>O<sub>4</sub> Favour the decomposition of N<sub>2</sub>O<sub>4</sub> Not alter the equilibrium Stop the reaction
11 According to Le-Chatelier's principal, adding heat to a solid and liquid in equilibrium will cause the Amount of solid to decrease Amount of liquid to decrease Temperature to rise Temperature to fall
12 Equal volumes of N<sub>2</sub>and H<sub>2</sub>are reacting Equal masses of N<sub>2</sub>and H<sub>2</sub>are reacting The reaction has stopped The same amount of ammonia is formed as is decomposed into N<sub>2</sub>and H<sub>2</sub>
13 [A] = [B] [A] &lt; [B] [B] = [C] [A] &gt; [B]
14 Complete conversion of A to B has taken place Conversion of A to B is only 50% complete Only 10% conversion of A to B has taken place The rate of transformation of A to B is just equal to rate of transformation of B to A in the system
15 The equilibrium constant in a reversible chemical reaction at a given temperature Depends on the initial concentration of the reactants Depends on the concentration of one of the products at equilibrium Does not depend on the initial concentration of rectants It is characteristic of the reaction
16 In a reversible chemical reaction having two reactants in equilibrium, if the concentration of the reactants are doubled then the equilibrium constant will Also be doubled Be halved Becomes one fourth Remains the same
17 0.60 1.67 0.66 2.6
18 Forward reaction is favoured Backward reaction is favoured No effect None of the above
19 The solubility product of Ca(OH)2is 6.5 x 10-6. The concentration of OH-ions is 1.175 x 10<sup>-2</sup> 2.35 x 10<sup>-2</sup> 3.25 x 10<sup>-3</sup> 3.25 x 10<sup>-4</sup>
20 The solubility of PbF2is 2.6 x 10-3mole dm-3 then its solubility product is 2.6 x 10<sup>-3</sup> 6.76 x 10<sup>-6</sup> 5.2 x 10<sup>-6</sup> 7.0 x 10<sup>-8</sup>
21 Kspvalue for PbSO4= 1.8 x 10-8mole2dm-6. The maximum concentration of Pb++ions is 1.34 x 10<sup>-4</sup>mole dm<sup>-3</sup> 1.8 x 10<sup>-4</sup> 3.6 x 10<sup>-16</sup>mole dm<sup>-3</sup> 1.0 x 10<sup>-8</sup>mole dm<sup>-3</sup>
22 The solubility product of AgCl is 2.0 x 10-10mole 2dm-6. The maximum concentration of Ag+ions in the solution is 2.0 x 10<sup>-10</sup>mole dm<sup>-3</sup> 1.41 x 10<sup>-5</sup>mole dm<sup>-3</sup> 1.0 x 10<sup>-10</sup> 4.0 x 10<sup>-20</sup>mole dm<sup>-3</sup>
23 Product of concentration of ions raised to the power equal to the co-efficient of ions in balanced equation for saturated solution of a salt is called Ionic product Equilibrium constant K<sub>c</sub> K<sub>w</sub> Solubility product (K<sub>sp</sub>)
24 Buffers having pH less than 7 are made Mixture of weak acid + salt of it with strong base Mixture of weak acid + salt of it with weak base Mixture of weak base + salt of it with strong acid Mixture of weak base + salt of it with weak base
25 The relation between Kc and Kp is
26 pH of the human blood which is essentially maintained constant due to carbonates, biocarbonates, phosphates etc., is 7.00 7.25 7.35 7.47
27 A buffer solution of 0.1 molar HCOOH and 0.1 molar HCCONa has pH = 3.78 To is 0.01 molar HCl is added, then pH of the buffer solution becomes 2.78 4.78 3.78 3.70
28 If pH of buffer of 1 mole dm-3of HCOOH + 0.1 mole dm-3HCOONa having pKa = 3.78 is 1.78 2.78 3.78 4.78
29 pH of 0.1 molar HCl solution is 1 zero 13 14
30 A buffer of a 0.09 molar acetic acid and 0.11 molar sodium acetate has pH = 4.83. If 0.01 mole NaOH in 1 dm3of the buffer solution is added, then pH of the buffer becomes 4.74 4.92 5.0 4.0
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