{"id":162950,"date":"2026-02-11T16:01:57","date_gmt":"2026-02-11T16:01:57","guid":{"rendered":"https:\/\/news.gyankatta.org\/?p=162950"},"modified":"2026-02-11T16:02:34","modified_gmt":"2026-02-11T16:02:34","slug":"class-11-chemistry-redox-reactions","status":"publish","type":"post","link":"https:\/\/news.gyankatta.org\/?p=162950","title":{"rendered":"Class 11 Chemistry: Redox Reactions"},"content":{"rendered":"\n
<\/code><\/pre>\n\n\n\n
<\/h2>\n\n\n\n
\n\n\n\n
Question 1:<\/h3>\n\n\n\n
Which of the following statement(s) is\/are not true about the following decomposition reaction?<\/p>\n\n\n\n
2KClO3<\/sub> \u2192 2KCl + 3O2<\/sub><\/p>\n\n\n\n
    \n
  • (i) Potassium is undergoing oxidation<\/li>\n\n\n\n
  • (ii) Chlorine is undergoing oxidation<\/li>\n\n\n\n
  • (iii) Oxygen is reduced<\/li>\n\n\n\n
  • (iv) None of the species are undergoing oxidation or reduction<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n
    Question 2:<\/h3>\n\n\n\n
    Identify disproportionation reaction<\/p>\n\n\n\n
      \n
    • (i) CH4<\/sub> + 2O2<\/sub> \u2192 CO2<\/sub> + 2H2<\/sub>O<\/li>\n\n\n\n
    • (ii) CH4<\/sub> + 4Cl2<\/sub> \u2192 CCl4<\/sub> + 4HCl<\/li>\n\n\n\n
    • (iii) 2F2<\/sub> + 2OH–<\/sup> \u2192 2F–<\/sup> + OF2<\/sub> + H2<\/sub>O<\/li>\n\n\n\n
    • (iv) 2NO2<\/sub> + 2OH–<\/sup> \u2192 NO2<\/sub>–<\/sup> + NO3<\/sub>–<\/sup> + H2<\/sub>O<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n
      Question 3:<\/h3>\n\n\n\n
      Which of the following arrangements represents an increasing oxidation number of the central atom?<\/p>\n\n\n\n
        \n
      • (i) CrO2<\/sub>–<\/sup>, ClO3<\/sub>–<\/sup>, CrO4<\/sub>2-<\/sup>, MnO4<\/sub>–<\/sup><\/li>\n\n\n\n
      • (ii) ClO3<\/sub>–<\/sup>, CrO4<\/sub>2-<\/sup>, MnO4<\/sub>–<\/sup>, CrO2<\/sub>–<\/sup><\/li>\n\n\n\n
      • (iii) CrO2<\/sub>–<\/sup>, ClO3<\/sub>–<\/sup>, MnO4<\/sub>–<\/sup>, CrO4<\/sub>2-<\/sup><\/li>\n\n\n\n
      • (iv) CrO4<\/sub>2-<\/sup>, MnO4<\/sub>–<\/sup>, CrO2<\/sub>–<\/sup>, ClO3<\/sub>–<\/sup><\/li>\n<\/ul>\n\n\n\n
        \n\n\n\n
        Question 4:<\/h3>\n\n\n\n
        The oxidation number of an element in a compound is evaluated on the basis of certain rules. Which of the following rules is not correct in this respect?<\/p>\n\n\n\n
          \n
        • (i) The oxidation number of hydrogen is always +1.<\/li>\n\n\n\n
        • (ii) The algebraic sum of all the oxidation numbers in a compound is zero.<\/li>\n\n\n\n
        • (iii) An element in the free or uncombined state bears oxidation number zero.<\/li>\n\n\n\n
        • (iv) In all its compounds, the oxidation number of fluorine is -1.<\/li>\n<\/ul>\n\n\n\n
          \n\n\n\n
          Question 5:<\/h3>\n\n\n\n
          Using the standard electrode potential, find out the pair between which redox reaction is not feasible.<\/p>\n\n\n\n
          E\u00b0 values: Fe3+<\/sup>\/Fe2+<\/sup> = +0.77 V; I2<\/sub>\/I–<\/sup> = +0.54 V; Cu2+<\/sup>\/Cu = +0.34 V; Ag+<\/sup>\/Ag = +0.80 V<\/p>\n\n\n\n
            \n
          • (i) Fe3+<\/sup> and I–<\/sup><\/li>\n\n\n\n
          • (ii) Ag+<\/sup> and Cu<\/li>\n\n\n\n
          • (iii) Fe3+<\/sup> and Cu<\/li>\n\n\n\n
          • (iv) Ag and Fe3+<\/sup><\/li>\n<\/ul>\n\n\n\n
            \n\n\n\n
            Question 6:<\/h3>\n\n\n\n
            The more positive the value of E\u00b0, the greater the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.<\/p>\n\n\n\n
            E\u00b0 values: Fe3+<\/sup>\/Fe2+<\/sup> = +0.77 V; I2<\/sub>(s)\/I–<\/sup> = +0.54 V; Cu2+<\/sup>\/Cu = +0.34 V; Ag+<\/sup>\/Ag = +0.80 V<\/p>\n\n\n\n
              \n
            • (i) Fe3+<\/sup><\/li>\n\n\n\n
            • (ii) I2<\/sub>(s)<\/li>\n\n\n\n
            • (iii) Cu2+<\/sup><\/li>\n\n\n\n
            • (iv) Ag+<\/sup><\/li>\n<\/ul>\n\n\n\n
              \n\n\n\n
              Question 7:<\/h3>\n\n\n\n
              What is an oxidation reaction?<\/p>\n\n\n\n
              \n\n\n\n
              Question 8:<\/h3>\n\n\n\n
              What is the reduction reaction?<\/p>\n\n\n\n
              \n\n\n\n
              Question 9:<\/h3>\n\n\n\n
              What are the most essential conditions that must be satisfied in a redox reaction?<\/p>\n\n\n\n
              \n\n\n\n
              Question 10:<\/h3>\n\n\n\n
              What happens to the oxidation number of an element in oxidation?<\/p>\n\n\n\n
              \n\n\n\n
              Question 11:<\/h3>\n\n\n\n
              Name the different types of redox reactions.<\/p>\n\n\n\n
              \n\n\n\n
              Question 12:<\/h3>\n\n\n\n
              All decomposition reactions are not redox reactions. Give justification.<\/p>\n\n\n\n
              \n\n\n\n
              Question 14:<\/h3>\n\n\n\n
              What is the role of a salt bridge in an electrochemical cell?<\/p>\n\n\n\n
              \n\n\n\n
              Question 15:<\/h3>\n\n\n\n
              Define a redox couple.<\/p>\n\n\n\n
              \n\n\n\n
              Question 16:<\/h3>\n\n\n\n
              Explain why:<\/p>\n\n\n\n
              3Fe3<\/sub>O4<\/sub>(s) + 8Al(s) \u2192 9Fe(s) + 4Al2<\/sub>O3<\/sub>(s)<\/p>\n\n\n\n
              is an oxidation reaction?<\/p>\n\n\n\n
              \n\n\n\n
              Question 17:<\/h3>\n\n\n\n
              The reaction<\/p>\n\n\n\n
              Cl2<\/sub>(g) + 2OH\u2013<\/sup>(aq) \u2192 ClO\u2013<\/sup>(aq) + Cl\u2013<\/sup>(aq) + H2<\/sub>O(l)<\/p>\n\n\n\n
              represents the process of bleaching. Identify and name the species that bleaches the substances due to their oxidising action.<\/p>\n\n\n\n
              \n\n\n\n
              Question 18:<\/h3>\n\n\n\n
              Fluorine reacts with ice and results in the change:<\/p>\n\n\n\n
              H2<\/sub>O(s) + F2<\/sub>(g) \u2192 HF(g) + HOF(g)<\/p>\n\n\n\n
              Justify that this reaction is a redox reaction.<\/p>\n\n\n\n
              \n\n\n\n
              Question 19:<\/h3>\n\n\n\n
              MnO4<\/sub>2-<\/sup> undergoes a disproportionation reaction in an acidic medium but MnO4<\/sub>\u2013<\/sup> does not. Give a reason.<\/p>\n\n\n\n
              \n\n\n\n
              Question 20:<\/h3>\n\n\n\n
              Write the formula for the following compounds:<\/p>\n\n\n\n
                \n
              • (a) Mercury(II) chloride<\/li>\n\n\n\n
              • (b) Nickel(II) sulphate<\/li>\n\n\n\n
              • (c) Tin(IV) oxide<\/li>\n\n\n\n
              • (d) Thallium(I) sulphate<\/li>\n\n\n\n
              • (e) Iron(III) sulphate<\/li>\n\n\n\n
              • (f) Chromium(III) oxide<\/li>\n<\/ul>\n\n\n\n
                \n\n\n\n
                Question 21:<\/h3>\n\n\n\n
                PbO and PbO2<\/sub> react with HCl according to the following chemical equations:<\/p>\n\n\n\n
                2PbO + 4HCl \u2192 2PbCl2<\/sub> + 2H2<\/sub>O<\/p>\n\n\n\n
                PbO2<\/sub> + 4HCl \u2192 PbCl2<\/sub> + Cl2<\/sub> + 2H2<\/sub>O<\/p>\n\n\n\n
                Why do these compounds differ in their reactivity?<\/p>\n\n\n\n
                \n\n\n\n
                Question 22:<\/h3>\n\n\n\n
                Nitric acid is an oxidising agent and reacts with PbO, but it does not react with PbO2<\/sub>. Explain why.<\/p>\n\n\n\n
                \n\n\n\n
                Question 23:<\/h3>\n\n\n\n
                The compound AgF2<\/sub> is an unstable compound. However, if formed, the compound acts as a very strong oxidising agent. Why?<\/p>\n\n\n\n
                \n\n\n\n
                Question 24:<\/h3>\n\n\n\n
                Calculate the oxidation number of phosphorus in the following species.<\/p>\n\n\n\n
                  \n
                • (a) HPO3<\/sub>2-<\/sup><\/li>\n\n\n\n
                • (b) PO4<\/sub>3-<\/sup><\/li>\n<\/ul>\n\n\n\n
                  \n\n\n\n
                  Question 25:<\/h3>\n\n\n\n
                  What sorts of information can you draw from the following reaction?<\/p>\n\n\n\n
                  (CN)2<\/sub>(g) + 2OH\u2013<\/sup>(aq) \u2192 CN\u2013<\/sup>(aq) + CNO\u2013<\/sup>(aq) + H2<\/sub>O(l)<\/p>\n\n\n\n
                  \n\n\n\n
                  Question 26:<\/h3>\n\n\n\n
                  Identify the redox reactions out of the following reactions and identify the oxidising and reducing agents in them.<\/p>\n\n\n\n
                    \n
                  • (i) 3HCl(aq) + HNO3<\/sub>(aq) \u2192 Cl2<\/sub>(g) + NOCl(g) + 2H2<\/sub>O(l)<\/li>\n\n\n\n
                  • (ii) HgCl2<\/sub>(aq) + 2KI(aq) \u2192 HgI2<\/sub>(s) + 2KCl(aq)<\/li>\n\n\n\n
                  • (iii) Fe2<\/sub>O3<\/sub>(s) + 3CO(g) \u2192 2Fe(s) + 3CO2<\/sub>(g)<\/li>\n\n\n\n
                  • (iv) PCl3<\/sub>(l) + 3H2<\/sub>O(l) \u2192 3HCl(aq) + H3<\/sub>PO4<\/sub>(aq)<\/li>\n\n\n\n
                  • (v) 4NH3<\/sub> + 3O2<\/sub>(g) \u2192 2N2<\/sub>(g) + 6H2<\/sub>O(g)<\/li>\n<\/ul>\n\n\n\n
                    \n\n\n\n
                    Question 27:<\/h3>\n\n\n\n
                    Refer to the periodic table given in your book and now answer the following questions:<\/p>\n\n\n\n
                      \n
                    • (a) Select the possible non-metals that can show a disproportionation reaction.<\/li>\n\n\n\n
                    • (b) Select three metals that can show a disproportionation reaction.<\/li>\n<\/ul>\n\n\n\n
                      \n\n\n\n
                      Question 28:<\/h3>\n\n\n\n
                      Explain redox reactions on the basis of electron transfer. Give suitable examples.<\/p>\n\n\n\n
                      \n\n\n\n
                      Question 29:<\/h3>\n\n\n\n
                      Arrange the given metals in the order in which they displace each other from the solution of their salts.<\/p>\n\n\n\n
                        \n
                      • (i) Al<\/li>\n\n\n\n
                      • (ii) Fe<\/li>\n\n\n\n
                      • (iii) Cu<\/li>\n\n\n\n
                      • (iv) Zn<\/li>\n\n\n\n
                      • (v) Mg<\/li>\n<\/ul>\n\n\n\n
                        \n\n\n\n
                        Question 30:<\/h3>\n\n\n\n
                        Why does fluorine not show a disproportionation reaction?<\/p>\n\n\n\n
                        \n\n\n\n
                        Question 31:<\/h3>\n\n\n\n
                        Which method can be used to find out the strength of the reductant\/oxidant in a solution? Explain with an example.<\/p>\n","protected":false},"excerpt":{"rendered":"
                        Question 1: Which of the following statement(s) is\/are not true about the following decomposition reaction? 2KClO3 \u2192 2KCl + 3O2 Question 2: Identify disproportionation reaction Question 3: Which of the following arrangements represents an increasing oxidation number of the central…<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"fifu_image_url":"","fifu_image_alt":"","footnotes":""},"categories":[1],"tags":[],"class_list":["post-162950","post","type-post","status-publish","format-standard","hentry","category-uncategorized"],"yoast_head":"\nClass 11 Chemistry: Redox Reactions - Gyankatta<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/news.gyankatta.org\/?p=162950\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Class 11 Chemistry: Redox Reactions - Gyankatta\" \/>\n<meta property=\"og:description\" content=\"Question 1: Which of the following statement(s) is\/are not true about the following decomposition reaction? 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