{"id":618799,"date":"2023-03-03T11:00:49","date_gmt":"2023-03-03T11:00:49","guid":{"rendered":"https:\/\/www.indcareer.com\/schools\/?p=618799"},"modified":"2024-05-02T07:03:41","modified_gmt":"2024-05-02T07:03:41","slug":"ncert-exemplar-class-11-chemistry-chapter-7-equilibrium","status":"publish","type":"post","link":"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/","title":{"rendered":"NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium"},"content":{"rendered":"\n<p>NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium. NCERT Exemplar Solutions for Class 11 Chemistry Chapter 7 Equilibrium prepare students for their Class 11 exams thoroughly. <\/p>\n\n\n\n<p>Chemistry problems and solutions for the Class 11 pdf are provided here which are similar to the questions being asked in the previous year&#8217;s board. <\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\"><strong>NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium<\/strong><\/h2>\n\n\n\n<p>Class 11: Chemistry Chapter 7 solutions. Complete Class 11 Chemistry Chapter 7 Notes.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-multiple-choice-questions-type-i\"><strong>Multiple Choice Questions (Type-I)<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li>We know that the relationship between K<sub>c<\/sub> and K<sub>p<\/sub> is<br>K<sub>p<\/sub> = K<sub>c<\/sub> (RT)<sup>\u0394 n<br><\/sup>What would be the value of \u0394n for the reaction<br>NH<sub>4<\/sub>Cl (s) \u21d4 NH<sub>3<\/sub> (g) + HCl (g)\n<ul class=\"wp-block-list\">\n<li>(i) 1<\/li>\n\n\n\n<li>(ii) 0.5<\/li>\n\n\n\n<li>(iii) 1.5<\/li>\n\n\n\n<li>(iv) 2<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>For the reaction H<sub>2<\/sub>(g) + I<sub>2<\/sub>(g) \u21d4 2HI (g), the standard free energy is \u0394G<sup>\u2296<\/sup> &gt; 0. The equilibrium constant (K ) would be __________.\n<ul class=\"wp-block-list\">\n<li>(i) K = 0<\/li>\n\n\n\n<li>(ii) K &gt; 1<\/li>\n\n\n\n<li>(iii) K = 1<\/li>\n\n\n\n<li>(iv) K &lt; 1<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Which of the following is not a general characteristic of equilibria involving physical processes?\n<ul class=\"wp-block-list\">\n<li>(i) Equilibrium is possible only in a closed system at a given temperature.<\/li>\n\n\n\n<li>(ii) All measurable properties of the system remain constant.<\/li>\n\n\n\n<li>(iii) All the physical processes stop at equilibrium.<\/li>\n\n\n\n<li>(iv) The opposing processes occur at the same rate and there is dynamic but stable condition.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>PCl<sub>5<\/sub>, PCl<sub>3<\/sub> and Cl<sub>2<\/sub> are at equilibrium at 500K in a closed container and their concentrations are 0.8 \u00d7 10<sup>\u20133<\/sup> mol L<sup>\u20131<\/sup>, 1.2 \u00d7 10<sup>\u20133<\/sup> mol L<sup>\u20131<\/sup> and 1.2 \u00d7 10<sup>\u20133<\/sup> mol L<sup>\u20131<\/sup> respectively. The value of K<sub>c<\/sub> for the reaction PCl<sub>5<\/sub> (g) \u21d4 PCl<sub>3<\/sub> (g) + Cl<sub>2<\/sub> (g) will be\n<ul class=\"wp-block-list\">\n<li>(i) 1.8 \u00d7 10<sup>3<\/sup> mol L<sup>\u20131<\/sup><\/li>\n\n\n\n<li>(ii) 1.8 \u00d7 10<sup>\u20133<\/sup><\/li>\n\n\n\n<li>(iii) 1.8 \u00d7 10<sup>\u20133<\/sup> L mol<sup>\u20131<\/sup><\/li>\n\n\n\n<li>(iv) 0.55 \u00d7 10<sup>4<\/sup><\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Which of the following statements is incorrect?\n<ul class=\"wp-block-list\">\n<li>(i) In equilibrium mixture of ice and water kept in perfectly insulated flask mass of ice and water does not change with time.<\/li>\n\n\n\n<li>(ii) The intensity of red colour increases when oxalic acid is added to a solution containing iron (III) nitrate and potassium thiocyanate.<\/li>\n\n\n\n<li>(iii) On addition of catalyst the equilibrium constant value is not affected.<\/li>\n\n\n\n<li>(iv) Equilibrium constant for a reaction with negative \u0394H value decreases as the temperature increases.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture it becomes pink. On the basis of this information mark the correct answer.<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15831667815_903b19d6df_o.jpg\" alt=\"\">\n<ul class=\"wp-block-list\">\n<li>(i) \u0394H &gt; 0 for the reaction<\/li>\n\n\n\n<li>(ii) \u0394H &lt; 0 for the reaction<\/li>\n\n\n\n<li>(iii) \u0394H = 0 for the reaction<\/li>\n\n\n\n<li>(iv) The sign of \u0394H cannot be predicted on the basis of this information.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>The pH of neutral water at 25\u00b0C is 7.0. As the temperature increases, ionisation of water increases, however, the concentration of H<sup>+<\/sup> ions and OH<sup>\u2013<\/sup> ions are equal. What will be the pH of pure water at 60\u00b0C?\n<ul class=\"wp-block-list\">\n<li>(i) Equal to 7.0<\/li>\n\n\n\n<li>(ii) Greater than 7.0<\/li>\n\n\n\n<li>(iii) Less than 7.0<\/li>\n\n\n\n<li>(iv) Equal to zero<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>The ionisation constant of an acid, K<sub>a<\/sub>, is the measure of strength of an acid. The K<sub>a<\/sub> values of acetic acid, hypochlorous acid and formic acid are 1.74 \u00d7 10<sup>\u20135<\/sup>, 3.0 \u00d7 10<sup>\u20138<\/sup> and 1.8 \u00d7 10<sup>\u20134<\/sup> respectively. Which of the following orders of pH of 0.1 mol dm<sup>\u20133<\/sup> solutions of these acids is correct?\n<ul class=\"wp-block-list\">\n<li>(i) acetic acid &gt; hypochlorous acid &gt; formic acid<\/li>\n\n\n\n<li>(ii) hypochlorous acid &gt; acetic acid &gt; formic acid<\/li>\n\n\n\n<li>(iii) formic acid &gt; hypochlorous acid &gt; acetic acid<\/li>\n\n\n\n<li>(iv) formic acid &gt; acetic acid &gt; hypochlorous acid<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>K<sub>a1<\/sub>, K<sub>a2<\/sub> and K<sub>a3<\/sub> are the respective ionisation constants for the following reactions.<br>H<sub>2<\/sub>S \u21d4 H<sup>+<\/sup> + HS<sup>\u2013<\/sup><br>HS<sup>\u2013<\/sup> \u21d4 H<sup>+<\/sup> + S<sup>2\u2013<\/sup><br>H<sub>2<\/sub>S \u21d4 2H<sup>+<\/sup> + S<sup>2\u2013<br><\/sup>The correct relationship between K<sub>a1<\/sub>, K<sub>a2<\/sub> and K<sub>a3<\/sub> is\n<ul class=\"wp-block-list\">\n<li>(i) K<sub>a3<\/sub> = K<sub>a1<\/sub> * K<sub>a2<\/sub><\/li>\n\n\n\n<li>(ii) K<sub>a3<\/sub> = K<sub>a1<\/sub> + K<sub>a2<\/sub><\/li>\n\n\n\n<li>(iii) K<sub>a3<\/sub> = K<sub>a1<\/sub> \u2013 K<sub>a2<\/sub><\/li>\n\n\n\n<li>(iv) K<sub>a3<\/sub> = K<sub>a1<\/sub> \/ K<sub>a2<\/sub><\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Acidity of BF<sub>3<\/sub> can be explained on the basis of which of the following concepts?\n<ul class=\"wp-block-list\">\n<li>(i) Arrhenius concept<\/li>\n\n\n\n<li>(ii) Bronsted Lowry concept<\/li>\n\n\n\n<li>(iii) Lewis concept<\/li>\n\n\n\n<li>(iv) Bronsted Lowry as well as Lewis concept.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Which of the following will produce a buffer solution when mixed in equal volumes ?\n<ul class=\"wp-block-list\">\n<li>(i) 0.1 mol dm<sup>\u20133<\/sup> NH<sub>4<\/sub>OH and 0.1 mol dm<sup>\u20133<\/sup> HCl<\/li>\n\n\n\n<li>(ii) 0.05 mol dm<sup>\u20133<\/sup> NH<sub>4<\/sub>OH and 0.1 mol dm<sup>\u20133<\/sup> HCl<\/li>\n\n\n\n<li>(iii) 0.1 mol dm<sup>\u20133<\/sup> NH<sub>4<\/sub>OH and 0.05 mol dm<sup>\u20133<\/sup> HCl<\/li>\n\n\n\n<li>(iv) 0.1 mol dm<sup>\u20133<\/sup> CH<sub>4<\/sub>COONa and 0.1 mol dm<sup>\u20133<\/sup> NaOH<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>In which of the following solvents is silver chloride most soluble?\n<ul class=\"wp-block-list\">\n<li>(i) 0.1 mol dm<sup>\u20133<\/sup> AgNO<sub>3<\/sub> solution<\/li>\n\n\n\n<li>(ii) 0.1 mol dm<sup>\u20133<\/sup> HCl solution<\/li>\n\n\n\n<li>(iii) H<sub>2<\/sub>O<\/li>\n\n\n\n<li>(iv) Aqueous ammonia<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>What will be the value of pH of 0.01 mol dm<sup>\u20133<\/sup> CH<sub>3<\/sub>COOH (K<sub>a<\/sub> = 1.74 \u00d7 10<sup>\u20135<\/sup>)?\n<ul class=\"wp-block-list\">\n<li>(i) 3.4<\/li>\n\n\n\n<li>(ii) 3.6<\/li>\n\n\n\n<li>(iii) 3.9<\/li>\n\n\n\n<li>(iv) 3.0<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>K<sub>a<\/sub> for CH<sub>3<\/sub>COOH is 1.8 \u00d7 10<sup>\u20135<\/sup> and K<sub>b<\/sub> for NH<sub>4<\/sub>OH is 1.8 \u00d7 10<sub>-5<\/sub> . The pH of ammonium acetate will be\n<ul class=\"wp-block-list\">\n<li>(i) 7.005<\/li>\n\n\n\n<li>(ii) 4.75<\/li>\n\n\n\n<li>(iii) 7.0<\/li>\n\n\n\n<li>(iv) Between 6 and 7<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Which of the following options will be correct for the stage of half completion of the reaction A \u21d4 B.\n<ul class=\"wp-block-list\">\n<li>(i) \u0394G\u2296 = 0<\/li>\n\n\n\n<li>(ii) \u0394G\u2296 &gt; 0<\/li>\n\n\n\n<li>(iii) \u0394G\u2296 &lt; 0<\/li>\n\n\n\n<li>(iv) \u0394G\u2296 = \u2013RT ln2<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier\u2019s principle. Consider the reaction.<br>N<sub>2<\/sub>(g) + 3H<sub>2<\/sub>(g) \u21d4 2NH<sub>3<\/sub>(g)<br>Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?\n<ul class=\"wp-block-list\">\n<li>(i) K will remain same<\/li>\n\n\n\n<li>(ii) K will decrease<\/li>\n\n\n\n<li>(iii) K will increase<\/li>\n\n\n\n<li>(iv) K will increase initially and decrease when pressure is very high<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>What will be the correct order of vapour pressure of water, acetone and ether at 30\u00b0C. Given that among these compounds, water has maximum boiling point and ether has minimum boiling point?\n<ul class=\"wp-block-list\">\n<li>(i) Water &lt; ether &lt; acetone<\/li>\n\n\n\n<li>(ii) Water &lt; acetone &lt; ether<\/li>\n\n\n\n<li>(iii) Ether &lt; acetone &lt; water<\/li>\n\n\n\n<li>(iv) Acetone &lt; ether &lt; water<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>At 500 K, equilibrium constant, K<sub>c<\/sub>, for the following reaction is 5.<br>1 \/ 2 H<sub>2<\/sub> (g) + 1 \/ 2 I<sub>2<\/sub> (g) \u21d4 HI (g)<br>What would be the equilibrium constant K<sub>c<\/sub> for the reaction<br>2HI (g) \u21d4 H<sub>2<\/sub> (g) + I<sub>2<\/sub> (g)\n<ul class=\"wp-block-list\">\n<li>(i) 0.04<\/li>\n\n\n\n<li>(ii) 0.4<\/li>\n\n\n\n<li>(iii) 25<\/li>\n\n\n\n<li>(iv) 2.5<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>In which of the following reactions, the equilibrium remains unaffected on addition of small amount of argon at constant volume?\n<ul class=\"wp-block-list\">\n<li>(i) H<sub>2<\/sub> (g) + I<sub>2<\/sub> (g) \u21d4 2HI (g)<\/li>\n\n\n\n<li>(ii) PCl<sub>5<\/sub> (g) \u21d4 PCl<sub>3<\/sub> (g) + Cl<sub>2<\/sub>(g)<\/li>\n\n\n\n<li>(iii) N<sub>2<\/sub>(g) + 3H<sub>2<\/sub> (g) \u21d4 2NH<sub>3<\/sub> (g)<\/li>\n\n\n\n<li>(iv) The equilibrium will remain unaffected in all the three cases.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-multiple-choice-questions-type-ii\"><strong>Multiple Choice Questions (Type-II)<\/strong><\/h3>\n\n\n\n<p><strong>In the following questions two or more options may be correct.<\/strong><\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>For the reaction N<sub>2<\/sub> O<sub>4<\/sub> (g) \u21d4 2NO<sub>2<\/sub> (g), the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is correct?\n<ul class=\"wp-block-list\">\n<li>(i) The reaction is endothermic<\/li>\n\n\n\n<li>(ii) The reaction is exothermic<\/li>\n\n\n\n<li>(iii) If NO<sub>2<\/sub> (g) and N<sub>2<\/sub> O<sub>4<\/sub> (g) are mixed at 400 K at partial pressures 20 bar and 2 bar respectively, more N<sub>2<\/sub> O<sub>4<\/sub> (g) will be formed.<\/li>\n\n\n\n<li>(iv) The entropy of the system increases.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>At a particular temperature and atmospheric pressure, the solid and liquid phases of a pure substance can exist in equilibrium. Which of the following term defines this temperature?\n<ul class=\"wp-block-list\">\n<li>(i) Normal melting point<\/li>\n\n\n\n<li>(ii) Equilibrium temperature<\/li>\n\n\n\n<li>(iii) Boiling point<\/li>\n\n\n\n<li>(iv) Freezing point<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-short-answer-type-questions\"><strong>Short Answer Type Questions<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li>The ionisation of hydrochloric in water is given below:<br>HCl(aq) + H<sub>2<\/sub>O (l ) \u21d4 H<sub>3<\/sub>O<sup>+<\/sup> (aq) + Cl<sup>\u2013<\/sup> (aq)<br>Label two conjugate acid-base pairs in this ionisation.<\/li>\n\n\n\n<li>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?<\/li>\n\n\n\n<li>BF<sub>3<\/sub> does not have proton but still acts as an acid and reacts with NH<sub>3<\/sub>. Why is it so? What type of bond is formed between the two?<\/li>\n\n\n\n<li>Ionisation constant of a weak base MOH, is given by the expression<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15645863709_5356aaf279_o.jpg\" alt=\"\"><br>Values of ionisation constant of some weak bases at a particular temperature are given below:<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15646251088_6f664a03b8_o.jpg\" alt=\"\"><br>Arrange the bases in decreasing order of the extent of their ionisation at equilibrium. Which of the above base is the strongest?<\/li>\n\n\n\n<li>Conjugate acid of a weak base is always stronger. What will be the decreasing order of basic strength of the following conjugate bases?<br>OH<sup>\u2013<\/sup>,RO<sup>\u2013<\/sup>, CH<sub>3<\/sub>COO<sup>\u2013<\/sup>, Cl<sup>\u2013<\/sup><\/li>\n\n\n\n<li>Arrange the following in increasing order of pH.<br>KNO<sub>3<\/sub> (aq), CH<sub>3<\/sub>COONa (aq), NH<sub>4<\/sub>Cl (aq), C<sub>6<\/sub>H<sub>5<\/sub>COONH<sub>4<\/sub>(aq)<\/li>\n\n\n\n<li>The value of K<sub>c<\/sub> for the reaction 2HI (g) \u21d4 H<sub>2<\/sub> (g) + I<sub>2<\/sub> (g) is 1 \u00d7 10<sup>-4<br><\/sup>At a given time, the composition of reaction mixture is<br>[HI] = 2 \u00d7 10<sup>-5<\/sup> mol, [H<sub>2<\/sub>] = 1 \u00d7 10<sup>-5<\/sup> mol and [I<sub>2<\/sub>] = 1 \u00d7 10<sup>-5<\/sup> mol<br>In which direction will the reaction proceed?<\/li>\n\n\n\n<li>On the basis of the equation pH = \u2013 log [H<sup>+<\/sup>], the pH of 10<sup>-8<\/sup> mol dm<sup>-3<\/sup> solution of HCl should be 8. However, it is observed to be less than 7.0. Explain the reason.<\/li>\n\n\n\n<li>pH of a solution of a strong acid is 5.0. What will be the pH of the solution obtained after diluting the given solution a 100 times?<\/li>\n\n\n\n<li>A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution (Q<sub>sp<\/sub>) becomes greater than its solubility product. If the solubility of BaSO<sub>4<\/sub> in water is 8 \u00d7 10<sup>-4<\/sup> mol dm<sup>-3<\/sup>. Calculate its solubility in 0.01 mol dm<sup>-3<\/sup> of H<sub>2<\/sub>SO<sub>4<\/sub>.<\/li>\n\n\n\n<li>pH of 0.08 mol dm<sup>\u20133<\/sup> HOCl solution is 2.85. Calculate its ionisation constant.<\/li>\n\n\n\n<li>Calculate the pH of a solution formed by mixing equal volumes of two solutions A and B of a strong acid having pH = 6 and pH = 4 respectively.<\/li>\n\n\n\n<li>The solubility product of Al (OH)<sub>3<\/sub> is 2.7 \u00d7 10<sup>\u201311<\/sup>. Calculate its solubility in gL<sup>\u20131<\/sup> and also find out pH of this solution. (Atomic mass of Al = 27 u).<\/li>\n\n\n\n<li>Calculate the volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution. (K<sub>sp<\/sub> of PbCl<sub>2<\/sub> = 3.2 \u00d7 10<sup>\u20138<\/sup> , atomic mass of Pb = 207 u).<\/li>\n\n\n\n<li>A reaction between ammonia and boron trifluoride is given below:<br>: NH<sub>3<\/sub> + BF<sub>3<\/sub> \u2192 H<sub>3<\/sub>N : BF<sub>3<br><\/sub>Identify the acid and base in this reaction. Which theory explains it? What is the hybridisation of B and N in the reactants?<\/li>\n\n\n\n<li>Following data is given for the reaction: CaCO<sub>3<\/sub>(s) \u2192 CaO (s) + CO<sub>2<\/sub>(g)<br>\u0394<sub>f<\/sub> H<sup>\u2296<\/sup> [CaO(s)] = \u2013 635.1 kJ mol<sup>\u20131<\/sup><br>\u0394<sub>f<\/sub> H<sup>\u2296<\/sup> [CO<sub>2<\/sub>(g)] = \u2013 393.5 kJ mol<sup>\u20131<\/sup><br>\u0394<sub>f<\/sub> H<sup>\u2296<\/sup> [CaCO<sub>3<\/sub>(s)] = \u2013 1206.9 kJ mol<sup>\u20131<br><\/sup>Predict the effect of temperature on the equilibrium constant of the above reaction.<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-matching-type-questions\"><strong>Matching Type Questions<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Match the following equilibria with the corresponding condition<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15646251038_0e42b05e65_o.jpg\" alt=\"\"><\/li>\n\n\n\n<li><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15829794621_1fd55e8dea_o.jpg\" alt=\"\"><br>Some reactions are written below in Column I and their equilibrium constants in terms of K<sub>c<\/sub> are written in Column II. Match the following reactions with the corresponding equilibrium constant<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15211708854_1dcf168ee9_o.jpg\" alt=\"\"><\/li>\n\n\n\n<li>Match standard free energy of the reaction with the corresponding equilibrium constant<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15211708904_3b10bcf9e1_o.jpg\" alt=\"\"><\/li>\n\n\n\n<li>Match the following species with the corresponding conjugate acid<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15646838970_39f1f92ea3_o.jpg\" alt=\"\"><\/li>\n\n\n\n<li>Match the following graphical variation with their description<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15645863509_5899033f70.jpg\" alt=\"\"><\/li>\n\n\n\n<li>Match Column (I) with Column (II).<br><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/15645863459_121fdf6ec1_o.jpg\" alt=\"\"><\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-assertion-and-reason-type-questions\"><strong>Assertion and Reason Type Questions<\/strong><\/h3>\n\n\n\n<p><strong>In the following questions a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct option out of the choices given below each question.<\/strong><\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Assertion (A) : Increasing order of acidity of hydrogen halides is HF < HCl < HBr < HI<br>Reason (R) : While comparing acids formed by the elements belonging to the same group of periodic table, H\u2013A bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond.\n\n<ul class=\"wp-block-list\">\n\n<li>(i) Both A and R are true and R is the correct explanation of A.<\/li>\n\n\n<li>(ii) Both A and R are true but R is not the correct explanation of A.<\/li>\n\n\n<li>(iii) A is true but R is false.<\/li>\n\n\n<li>(iv) Both A and R are false.<\/li>\n\n<\/ul>\n\n<\/li>\n\n\n\n<li>Assertion (A) : A solution containing a mixture of acetic acid and sodium acetate maintains a constant value of pH on addition of small amounts of acid or alkali.<br>Reason (R) : A solution containing a mixture of acetic acid and sodium acetate acts as a buffer solution around pH 4.75.\n<ul class=\"wp-block-list\">\n<li>(i) Both A and R are true and R is correct explanation of A.<\/li>\n\n\n\n<li>(ii) Both A and R are true but R is not the correct explanation of A.<\/li>\n\n\n\n<li>(iii) A is true but R is false.<\/li>\n\n\n\n<li>(iv) Both A and R are false.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Assertion (A): The ionisation of hydrogen sulphide in water is low in the presence of hydrochloric acid.<br>Reason (R) : Hydrogen sulphide is a weak acid.\n<ul class=\"wp-block-list\">\n<li>(i) Both A and R are true and R is correct explanation of A.<\/li>\n\n\n\n<li>(ii) Both A and R are true but R is not correct explanation of A.<\/li>\n\n\n\n<li>(iii) A is true but R is false<\/li>\n\n\n\n<li>(iv) Both A and R are false<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Assertion (A): For any chemical reaction at a particular temperature, the equilibrium constant is fixed and is a characteristic property.<br>Reason (R) : Equilibrium constant is independent of temperature.\n<ul class=\"wp-block-list\">\n<li>(i) Both A and R are true and R is correct explanation of A.<\/li>\n\n\n\n<li>(ii) Both A and R are true but R is not correct explanation of A.<\/li>\n\n\n\n<li>(iii) A is true but R is false.<\/li>\n\n\n\n<li>(iv) Both A and R are false.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Assertion (A) : Aqueous solution of ammonium carbonate is basic.<br>Reason (R) : Acidic\/basic nature of a salt solution of a salt of weak acid and weak base depends on K<sub>a<\/sub> and K<sub>b<\/sub> value of the acid and the base forming it.\n<ul class=\"wp-block-list\">\n<li>(i) Both A and R are true and R is correct explanation of A.<\/li>\n\n\n\n<li>(ii) Both A and R are true but R is not correct explanation of A.<\/li>\n\n\n\n<li>(iii) A is true but R is false.<\/li>\n\n\n\n<li>(iv) Both A and R are false.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Assertion (A): An aqueous solution of ammonium acetate can act as a buffer.<br>Reason (R) : Acetic acid is a weak acid and NH<sub>4<\/sub>OH is a weak base.\n<ul class=\"wp-block-list\">\n<li>(i) Both A and R are true and R is correct explanation of A.<\/li>\n\n\n\n<li>(ii) Both A and R are true but R is not correct explanation of A.<\/li>\n\n\n\n<li>(iii) A is false but R is true.<\/li>\n\n\n\n<li>(iv) Both A and R are false.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Assertion (A): In the dissociation of PCl<sub>5<\/sub> at constant pressure and temperature addition of helium at equilibrium increases the dissociation of PCl<sub>5<\/sub>.<br>Reason (R) : Helium removes Cl<sub>2<\/sub> from the field of action.\n<ul class=\"wp-block-list\">\n<li>(i) Both A and R are true and R is correct explanation of A.<\/li>\n\n\n\n<li>(ii) Both A and R are true but R is not correct explanation of A.<\/li>\n\n\n\n<li>(iii) A is true but R is false.<\/li>\n\n\n\n<li>(iv) Both A and R are false.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<p><strong>Long Answer Type Questions<\/strong><\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>How can you predict the following stages of a reaction by comparing the value of K<sub>c<\/sub> and Q<sub>c<\/sub> ?\n<ul class=\"wp-block-list\">\n<li>(i) Net reaction proceeds in the forward direction.<\/li>\n\n\n\n<li>(ii) Net reaction proceeds in the backward direction.<\/li>\n\n\n\n<li>(iii) No net reaction occurs.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>On the basis of Le Chatelier principle explain how temperature and pressure can be adjusted to increase the yield of ammonia in the following reaction.<br>N<sub>2<\/sub>(g) + 3H<sub>2<\/sub>(g) \u21d4 2NH<sub>3<\/sub>(g) \u0394 H = \u2013 92.38 kJ mol<sup>\u20131<br><\/sup>What will be the effect of addition of argon to the above reaction mixture at constant volume?<\/li>\n\n\n\n<li>A sparingly soluble salt having general formula A <sup>p+<\/sup><sub>x<\/sub> B<sup>q-<\/sup><sub>y<\/sub>and molar solubility S is in equilibrium with its saturated solution. Derive a relationship between the solubility and solubility product for such salt.<\/li>\n\n\n\n<li>Write a relation between \u0394G and Q and define the meaning of each term and answer the following :\n<ul class=\"wp-block-list\">\n<li>(a) Why a reaction proceeds forward when Q &lt; K and no net reaction occurs when Q = K.<\/li>\n\n\n\n<li>(b) Explain the effect of increase in pressure in terms of reaction quotient Q. for the reaction : CO (g) + 3H<sub>2<\/sub>(g) \u21d4 CH<sub>4<\/sub>(g) + H<sub>2<\/sub>O (g)<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-answers-to-multiple-choice-questions\"><strong>Answers to Multiple Choice Questions<\/strong><\/h3>\n\n\n\n<h2 class=\"wp-block-heading\">Answers to Multiple Choice Questions<\/h2>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49048158307_9c0bb499bc_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047947431_f0f762f8d1_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047448163_81c6652155_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047450418_80eab91618_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047470918_8606e6a186_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047477753_0dc400ac5d_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047983566_b4d7cb7307_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047483368_947a2956cf_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047489688_ff7e3596df_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047995766_61efc67482_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047495928_7247e41e7a_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49048218747_6bd1202244_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49048008481_504c4173de_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49048224297_1b18b45dab_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49047511983_fec98eaa72_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<figure class=\"wp-block-image\"><img decoding=\"async\" src=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2024\/05\/49048018326_cc026ed087_o.png\" alt=\"\"\/><\/figure>\n\n\n\n<div class=\"wp-block-buttons is-layout-flex wp-block-buttons-is-layout-flex\">\n<div class=\"wp-block-button\"><a class=\"wp-block-button__link has-background wp-element-button\" href=\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-problems-solutions\/\" style=\"background-color:#f06d6d\" target=\"_blank\" rel=\"noreferrer noopener\">NCERT Exemplar Solutions<\/a><\/div>\n\n\n\n<div class=\"wp-block-button\"><a class=\"wp-block-button__link has-background wp-element-button\" href=\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-Chemistry-solutions\/\" style=\"background-color:#f06d6d\" target=\"_blank\" rel=\"noreferrer noopener\">NCERT Class 11 Exemplar Solutions<\/a><\/div>\n<\/div>\n","protected":false},"excerpt":{"rendered":"<p>NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium. NCERT Exemplar Solutions for Class 11 Chemistry Chapter 7 Equilibrium prepare students for their Class 11 exams thoroughly. Chemistry problems and solutions for the Class 11 pdf are provided here which are similar to the questions being asked in the previous year&#8217;s board. NCERT Exemplar Class 11 [&hellip;]<\/p>\n","protected":false},"author":302,"featured_media":618801,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"newspack_featured_image_position":"","newspack_post_subtitle":"","newspack_article_summary_title":"Overview:","newspack_article_summary":"","newspack_hide_updated_date":false,"newspack_show_updated_date":false,"footnotes":""},"categories":[1411,919],"tags":[],"boards":[],"class_list":["post-618799","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-book-solutions","category-class-11","entry"],"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v27.0 (Yoast SEO v27.1.1) - https:\/\/yoast.com\/product\/yoast-seo-premium-wordpress\/ -->\n<title>NCERT Exemplar for Class 11, Chemistry Chapter 7 - IndCareer Schools<\/title>\n<meta name=\"description\" content=\"NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium | Browse all Class 11 Chemistry Chapters NCERT Exemplar books - IndCareer Schools\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium\" \/>\n<meta property=\"og:description\" content=\"NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium. NCERT Exemplar Solutions for Class 11 Chemistry Chapter 7 Equilibrium prepare students for their\" \/>\n<meta property=\"og:url\" content=\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/\" \/>\n<meta property=\"og:site_name\" content=\"IndCareer Schools\" \/>\n<meta property=\"article:publisher\" content=\"https:\/\/www.facebook.com\/indcareer\" \/>\n<meta property=\"article:published_time\" content=\"2023-03-03T11:00:49+00:00\" \/>\n<meta property=\"article:modified_time\" content=\"2024-05-02T07:03:41+00:00\" \/>\n<meta property=\"og:image\" content=\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/indcareer-schools-2-18-2-scaled.jpg\" \/>\n\t<meta property=\"og:image:width\" content=\"1600\" \/>\n\t<meta property=\"og:image:height\" content=\"901\" \/>\n\t<meta property=\"og:image:type\" content=\"image\/jpeg\" \/>\n<meta name=\"author\" content=\"Pooja\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:creator\" content=\"@indcareer\" \/>\n<meta name=\"twitter:site\" content=\"@indcareer\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"Pooja\" \/>\n\t<meta name=\"twitter:label2\" content=\"Est. reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"18 minutes\" \/>\n<script type=\"application\/ld+json\" class=\"yoast-schema-graph\">{\"@context\":\"https:\/\/schema.org\",\"@graph\":[{\"@type\":\"Article\",\"@id\":\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/#article\",\"isPartOf\":{\"@id\":\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/\"},\"author\":{\"name\":\"Pooja\",\"@id\":\"https:\/\/www.indcareer.com\/schools\/#\/schema\/person\/d6945cf059726f162259ba738092301e\"},\"headline\":\"NCERT Exemplar Class 11 Chemistry Chapter 7: Equilibrium\",\"datePublished\":\"2023-03-03T11:00:49+00:00\",\"dateModified\":\"2024-05-02T07:03:41+00:00\",\"mainEntityOfPage\":{\"@id\":\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/\"},\"wordCount\":2497,\"publisher\":{\"@id\":\"https:\/\/www.indcareer.com\/schools\/#organization\"},\"image\":{\"@id\":\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/#primaryimage\"},\"thumbnailUrl\":\"https:\/\/www.indcareer.com\/schools\/wp-content\/uploads\/2023\/03\/indcareer-schools-2-18-2-scaled.jpg\",\"articleSection\":[\"Book Solutions\",\"class 11\"],\"inLanguage\":\"en-US\"},{\"@type\":\"WebPage\",\"@id\":\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/\",\"url\":\"https:\/\/www.indcareer.com\/schools\/ncert-exemplar-class-11-chemistry-chapter-7-equilibrium\/\",\"name\":\"NCERT Exemplar for Class 11, Chemistry Chapter 7 - 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