Question 28. Molecules of most electronegative elements such as O2, O3, halogens. The oxidation number of carbon is zero in Answer: Oxidation involves increase in O.N while reduction involves decrease in O.N. Answer: It is the difference in Standard Reduction Potential (SRP) of cathode and SRP of anode. This fallacy is overcome if we calculate the O.N. This system was introduced for the first time by German chemist, Alfred Stock and is known as Stock notation. But the amount of O2 which is actually available is 20.0 g which is less than the amount which is needed. Answer: (a) Hg(II)Cl2, (b) Ni(II)SO4, (c)Sn(IV)O2 (d) T12(I)SO4, (e) Fe2(III)(S04)3, (f) Cr2(III)O3. Why? Write Jour informations about the reaction: Two questions should be asked to determine if a reaction is a redox reaction: What is the maximum wight of nitric oxide that can be obtained starting only with 10.0 g of ammonia and 20.0 g of oxygen? Since the oxidation potential of Ag is much higher than that of H2O, therefore, (a) H3P02(aq) + 4AgNO3(aq) + 2H2O(l) ————->H3PO4(aq) + 4Ag(s) + 4HNO3(aq) Therefore, F2 is both reduced as well as oxidised. What is a disproportionation reaction ? 2MnO4–(aq) + 5S02(g) + 2H20(l) + H+(aq) ————> 2Mn2+(aq) + 5HSO4–(aq) NCERT Solutions for Chemistry – Class 11, Chapter 8: Redox Reactions “Redox Reactions” is the eighth chapter in the NCERT class 11 chemistry textbook. Choose all the statements which contain correct definitions of reduction How will you identify cathode and anode in electrochemical cell ? Question 1. Answer: Question 22. (a) 6CO2(g) + 12H2O(l) ————-> C6H12O6(s) + 6H2O(l) + 6O2(g) The O.N. (a) Hg2(Br03)2 (b) Br – Cl (c) KBrO4 (d) Br2 The oxidation number of atoms in their elemental state is taken as zero. For example, (i) An aqueous solution of AgNO3 with silver electrodes. (a) 3. Their relative oxidising power is, however, measured in terms of their electrode potentials. Question 23. Answer: Reactions (a) and (b) indicate that H3P02 (hypophosphorous acid) is a reducing agent and thus reduces both AgNO3 and CuS04 to Ag and Cu respectively. 160 g of 02 produce NO = 120 g Therefore, CuO is reduced to Cu but H 2 is oxidised to H 2 0. (b) The possible reaction between Ag+(aq) and Cu(s) is Cu(s) + 2Ag+  (aq)—> Cu2+(aq) + 2Ag(s) In this eighth unit of class 11 chemistry, we will learn about redox reactions, oxidation numbers, types of redox reactions (disproportionation), balancing redox reactions, and standard electrode potentials. Answer:  N2H4is reducing agent i.e., reductant whereas Cl03–is oxidising agent i.e., oxidant. Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions. SO2(g) + 2H2O(l) ————> SO42-(aq) + 4H+(aq) + 2 e–  …(i) Justify-giving reactions that among halogens, fluorine is the best oxidant and among hydrohalic compounds, hydroiodic add is the best reductant. Titration H2O2(aq) +2Fe2+(aq) +2H+(aq) ——-> 2Fe3+(aq) + 2H2O(l) In case of coordinate bond, it gives +2 value of oxidation number to less electronegative atom and -2 values to more electronegative atom when coordinate bond is directed formless electronegative atom to more electronegative atom . (b), Question 1. ENERGY CHANGES IN REACTIONS; Gases and Gas Laws; QUANTITATIVE ASPECTS OF CHEMICAL CHANGE; Magnetic field on a current carrying conductor; Coulomb’s law; EXPLOITING THE LITHOSPHERE OR EARTH’S CRUST; REDOX REACTIONS; GRADE 12 PHYSICAL SCIENCES. Answer: EMF of a cell is the difference in the electrode potentials of the two electrodes in a cell when no current flows through the cell. Answer: (a) The increasing order is. Similarly at the anode, either SO42-(aq) ions or H2O molecules are oxidised. (b) Cr is negative electrode, Pt in Mn04_ acts as positive electrode. Answer: In a galvanic cell due to redox reaction released energy gets converted into the electrical energy. Answer: Question 18. In compounds containing oxygen, the oxidation number of oxygen is – 2 except in peroxides (-1) such as Na, In all compounds. Chemical reaction in which oxidation as well as reduction is carried out simultaneously in the same container, is known as direct redox reaction In such reactions, energy is generally liberated in the form of heat energy. 6. Class 11 Chapter 08 Redox Reaction PDF Notes Assignment for JEE/NEET Free Study Material .Learn to find Oxidation Number, Types of Redox Reactions. Multiply Eq. 2 (+1) + x + 4 (-2) = 0 x – 6 = 0 x — +6 Thus, the reducing character of hydrohalic acids decreases in the order: HI > HBr > HCl > HF. In such reactions, energy is generally liberated in the form of electrical energy. Further, O.N. as redox reactions •Def: Redox reactions describe all chemical reactions in which there is a net change in atomic charge •It is a class of reactions that include: –formation of a compound from its elements –all combustion reactions –reactions that generate electricity –reactions … 2HBr + H2S04 —–> Br2+ S02 + 2H2O; 2HI + H2S04 ——> I2 + S02 + 2H2O (a) MnO4–(aq) +I–(aq) ———>Mn02(s) + I2 (s) (in basic medium) I2, however, being weaker oxidising agent oxidises S of S2O32-  ion to a lower oxidation of +2.5 in S4O62- ion. In other words, the oxidation number of reductant increases in a redox reaction. CBSE 12 Class Compartment Result 2020 (Out) – Check at cbseresults.nic.in, CBSE Class 10 Result 2020 (Out) – Check CBSE 10th Result at cbseresults.nic.in, cbse.nic.in, IARCS Olympiads: Indian Association for Research in Computing Science, Breaking: CBSE Exam to be conducted only for Main Subjects, CBSE Class 11 Chemistry Notes : Colloidal State. (c) Fe3+(aq) and Cu(s) (d)Ag(s) and Fe3+(aq) evaluation should be made separately as, The oxidation states of elements exhibiting variable oxidation states are specified by Roman numerals such as I, II, III, IV, etc., within parenthesis after the symbol or name of the element. Calculate the oxidation number of sulphur in H2SO4 and Na2SO4. The structure of H2SO5 is Question 17. Question 3. Play this game to review Chemistry. If we use a piece of platinum coated with finely divided black containing hydrogen gas absorbed in it. Question 1. (b) HCl is a weak reducing agent and can reduce H2S04to SO2and hence HCl is not oxidised to Cl2. 0. (ii) It maintains the electrical neutrality. 4. Although oxidation potential of H2O molecules is higher than that of Cl– ions, nevertheless, oxidation of Cl–(aq) ions occurs in preference to H2O since due to overvoltage much lower potential than -1.36 V is needed for the oxidation of H2O molecules. Thus, this is a redox reaction. The clause you wrote was relating (ii), we have, 1/1 points | Previous Answers NCSUGenChem102LabV1 11.IL.01. Fluorine reacts with ice and results in the change: Chemistry Redox Reaction part 1 (Introduction) CBSE class 11 XI. Question 2. (i) by 3 and add it to Eq. (b) O3(g) + H2O2 (l) ———–> H2O(l) + O2(g) + O2(g) Their electrode potentials are: (b)Balance the following equation by oxidation number method: Question 9. Class 11 Chemistry Chapter 8 Redox Reactions primarily deals in understanding the classical idea of Redox Reactions, that involves the oxidation and reduction reactions and other topics such as electrode processes, oxidation number, and electron transfer reactions. Give one example. Ans. The excess chlorine is removed by treating with sulphur dioxide. Redox reactions are balanced by … What is the oxidation state of Ni in Ni (CO)4? Since this is the last lab and the TAs will be busy studying for their own exams, your lab grades will be submitted soon after the last assignment is due. Chapter 11. From the equation, Redox reactions are those reactions in which oxidation and reduction takes place simultaneously; Classical view of redox reactions. For what purpose it is used? (a) + 2 (b) +4 (c) +1 (d) +3 Therefore, it can only decrease its O.N. Predict the products of electrolysis in each of the following: (a) Which substances are oxidised and reduced in this cell? These clauses must always be located adjacent to the thing they relate to. All elements in the elementary state have oxidation number zero, e.g., He, Cl. What is meant by cell potential? By chemical bonding, C2 is attached to three H-atoms (less electronegative than carbon) and one CH2OH group (more electronegative than carbon), therefore, Various Types of Redox Reactions In this lesson we investigate various redox reactions. Step II Split the redox reaction into its oxidation-half and reduction half-reaction. (iii) individual reaction at each electrode. Class 11 Chemistry Redox Reactions: Rules to assign and calculate oxidation number: Rules to assign and calculate oxidation number . .•. Therefore, 02 is the limiting reagent and hence calculations must be based upon the amount of 02 taken and not on the amount of NH3 taken. Similarly, at the anode, either Ag metal of the anode or H2O molecules may be oxidised. Here O.N. This chapter is regarded by many as one of the most important chapters in the CBSE class 11 chemistry syllabus, owing to the fact that the entire field of electrochemistry deals with redox reactions. of O is zero. (c) Cl2O7(g) + H2O2(aq) ———-> ClO2–(aq) + O2(g) + H+ Question 7. The oxidation number is defined as the charge in which an atom appears to have when all other atoms are removed from it as ions. The correct order is Mg, Al, Zn, Fe, Cu . Platinum black catalyses the reaction and equilibrium is attained faster. (a) -1, -1 (b) -2, -2 (c)  -1, -2 (d) +2, -2 (a) Mercury (II) chloride, (b) Nickel (II) sulphate, (c) Tin (IV) oxide, (d) Thallium Here you can get Class 11 Important Questions Chemistry based on NCERT Text book for Class XI.Chemistry Class 11 Important Questions are very helpful to score high marks in board exams. Br2, however, oxidises F to I2 but not F–  to F2 , and Cl–   to Cl2. (b)Fe2+ +Cr2O72-+ H+ ——–> Fe3+ + Cr3++ H2O, Question 5. Cr2O72–(aq) + 14H+(aq) + 6e– ————> 2Cr3+(aq) + 7H20(l) …(ii) 2Cu2+(aq) + 4I–(aq) >Cu2I2(s) + I2(aq); Cu2+(aq) + 2Br–> No reaction. The principle used in balancing redox reaction is that number of electrons lost is same as number of electrons gained. Ag+(aq) +e–———-> Ag(s); E° = +0.80 V …(i) When excess of Na is used, sodium oxide is formed in which the oxidation state of O is -2. Thus, when an aqueous solution 0f AgN03 is electrolysed, Ag from Ag anode dissolves while Ag+(aq) ions present in the solution get reduced and get deposited on the cathode. In HNO2 oxidation number of nitrogen is +3, it can decrease or increase with range of-3 to +5, hence it can act as both oxidising and reducing agent. (a) Arrange the following in order of increasing O.N of iodine: Answer:  H2O is a neutral molecule O.N of H2O = 0 Answer: Let the oxidation number of S in H2SO4 be x. M4O2 + 4HCI ————-> M4Cl2 + Cl2 + 2H20 Chlorine is used to purify drinking water. Step IV Equalize the total increase or decrease in oxidation number, 8H+ + 4 Mg + 2HNO3 + 8NO3– → 4 Mg (NO3)2 + N2O + 5H2O, 4 Mg + 10 HNO3 → 4 Mg (NO3)2 + N2O + 5H2O, All CBSE Notes for Class 11 Chemistry Maths Notes Physics Notes Biology Notes. Question 16. It is because of this reason that thiosulphate reacts differently with Br2 and I2. Answer: At cathode there is gain of electrons. Question 6. Cr3+/Cr = -0.74 V. Arrange these metals in increasing order of their reducing power. (a) O3 (b) KMnO4 (c) H2O2 (d) K2Cr2O7 (b) Fe2O3(s) +3CO(g) —-> 2Fe(s) + 3CO2(g) Question 3. All these reactions are always accompanied by energy change in the form of heat, light or electricity. Chapter 8 Redox Reactions Download NCERT Solutions for Class 11 Chemistry (Link of Pdf file is given below at the end of the Questions List) In this pdf file you can see answers of following Questions NCERT Solutions Exercises Questions . What is salt bridge? Question 8. of S in H2SO5. By conventional method, the O.N. Answer:  (i) In S02 , O.N. F2(g) + 2I–(aq) ———-> 2F–(aq) + I2(s); Cl2 (g) + 2Br–(aq) ————> 2Cl–(aq) + Br2 (Z) CBSE Class 11 Chemistry Worksheet - Redox Reactions (1) CBSE,CCE and NCERT students can refer to the attached file. What is meant by reducing agent? To get fastest exam alerts and government job alerts in India, join our Telegram channel. (a) Fe3+(aq) and I-(aq) (b) Ag+   (aq) and Cu(s) Write the oxidation number of each atom its symbol. Because of the presence of seven electrons in the valence shell, I shows an oxidation state of -1 (in compounds of I with more electropositive elements such as H, Na, K, Ca, etc.) In other words, the oxidation number of oxidant decreases in a redox reaction. (a) Select the possible non-metals that can show disproportionation reaction. (b) N2H4(l) + ClO–(aq) ——–> NO(g) + CV(aq) = +1) group, therefore, O.N. (a) or by using  H20218 or O318in reaction (b). KH, CaH2 etc. In principle, S can have a minimum O.N. What is meant by electrochemical series? Similarly, at the anode, either Cl–(aq) ions or H2O molecules are oxidised. Oxidation is defined as the addition of oxygen/electronegative element to a substance or rememoval of hydrogen/ electropositive element from a susbtance. Question 19. Thus, it is a redox reaction and more specifically, it is a disproportionation reaction. (iv) In HNO3, O.N. Question 10. Question 10. The oxidation number of the carboxylic carbon atom in CH3COOH is Ag(s) ———–> Ag+(aq) + e–; E° = -0.80 V …(iii) Important questions, guess papers, most expected questions and best questions from 11th Chemistry chapter 08 Redox Reactions have CBSE chapter wise important questions with solution for free download in PDF format. Why? Write the O.N of all the atoms for the following well known oxidants? Hydrocarbons . If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. Further, it may be noted that whenever any half reaction equation is multiplied by any integer, its electrode potential is not multiplied by that integer. H20(S) + F2 (g) ——-> HF(g) + HOF(g) Justify that the following reactions are redox reactions: Thus, this is a redox reaction. This reaction is also known as autoredox reaction. Answer: (a) Ag+  is reduced, C6H6O2 is oxidised.Ag+  is oxidising agent whereas C6H6O2 is reducing agent. 2K2Mn04 + Cl2 ———–> 2KCl + 2KMnO4 Here, O is removed from CuO, therefore, it is reduced to Cu while O is added to H2 to form H20, therefore, it is oxidised. Reductant or reducing agent is a chemical.substance which can give one or more electrons and causes reduction of some other species. At anode there is loss of electrons. We use the reaction between copper and silver nitrate to show a displacement reaction. In this Grade 11 Physical Sciences show we take a look at Redox Reactions I. (b) Cs. Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions. Answer: HCl gets oxidised. Answer:  Electrochemical series is the series of elements in which elements are arranged in decreasing order of their reduction potential. (b) When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent smelling gas HCl, but if the mixture contains bromide then we get red vapour of bromine. H2O(l) + 2e– ——–> H2(g) + 2OH–; E° = -0.83 V of N in N03–whether one calculates by conventional method or by chemical bonding method. This may be illustrated as, Every chemical equation must be balanced according to law of conservation of mass. Answer:Â. Thus, cyanogen is simultaneously reduced to cyanide ion and oxidised to cyanate ion. Question 8. (i) and gained in Eq. The above redox reaction can be split into the following two half reactions. Therefore, BCl3 is reduced while LiAlH4 is oxidised. Redox reactions grade 11 2. As fluorine is the most electronegative element, it always has an oxidation number of – 1 in all of its compounds. Suggest a list of substances where carbon can exhibit oxidation states from -4 to +4 and nitrogen from -3 to +5. 2Ag + 2H2 S04 ———-> Ag2 S04 + 2H20 + S02 Oxidant or oxidising agent is a chemical substance which can accept one or more electrons and causes oxidation of some other species. (c) Because it decomposes to give nascent oxygen. (CN)2(g) + 2OH–(aq) —–> CN–(aq) + CNO–(aq) + H2O(l) It can only decrease its O.N. What is the source of electrical energy in a galvanic cell? Redox Reactions Class 11 Chapter 8 Chemistry Important Questions. Topics in this lesson. (b) List three measures used to prevent rusting of iron. Oxidation is addition of oxygen / electronegative element to a substance or removal of hydrogen / electropositive element from a substance (d) Ne. of O is -1. Calculate the sum of the oxidation numbers of all the atoms. 11th Chemistry chapter 08 Redox Reactions have many topics. Answer: Question 9. Answer: Topics and Subtopics in NCERT Solutions for Class 11 Chemistry Chapter 8 Redox Reactions: NCERT Solutions Class 11 ChemistryChemistry Lab ManualChemistry Sample Papers. But the oxidation number cannot be fractional. (iv) An aqueous solution of CuCl2 with platinum electrodes.  Similarly, I have added an ‘s’ in the definitions in Slides 2, 4, 9, and 11. Chapter 13. Further show: Count for the fallacy. (b) H3P02(aq) + 2CuS04(aq) + 2H2O(l) ————->H3P04(aq) + 2Cu(s) + H2S04(aq) Which of these will actually get discharged would depend upon their electrode potentials which are given below: Question 3. Calculate the sum of the oxidation numbers of all the atoms. (iii) KClO4 ; K(+l); Cl(+7); 0(-2), Question 6. 11/25/14, 12:43 PM Lab 11 InLab - Redox Reactions Page 1 of 10 Current Score : 50 / 50 Due : Friday, November 21 2014 01:10 PM EST 1. (i) The reaction involves decomposition of cyanogen, (CN)2 in the alkaline medium to cyanide ion, CN and cyanate ion,CNO–. and hence can act both as an oxidising as well as a reducing agent. (i). Answer:  Lower the electrode potential, better is the reducing agent. Slides 3 – 5: Same comments as for Slide 2. Answer: Standard hydrogen electrode is known as reference electrode. (b) MnO4–(aq) + S02(g) ——-> Mn2+(aq) +H2S04–(in acidic solution) Their electrode potentials are: If, however, excess of Cl2 is used, the initially formed PCl3 reacts further to form PCl5 in which the oxidation state of P is +5 NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12. Chemical reactions which involves both oxidation as well as reduction process simultaneously, are known as redox reactions (‘red’) from reduction and ‘ox’ from oxidation). Write the oxidation number of Cr above its symbol and that of H2O above its formula. redox reactions always involve changes in oxidation numbers. Question 1. (b) Chlorine is in maximum oxidation state +7 in ClO4 so it does not show the disproportionation reaction. Answer: Question 8. In transition elements the lowest oxidation number is equal to the number of ns electrons and highest oxidation number is equal to number of ‘ns’ and (n – l)d unpaired electrons. Since the electrode potentials of halogens decrease in the order: F2 (+2.87V) > Cl2 (+1.36V) > Br2 (+1.09V) > I2 (+0.54V), therefore, their oxidising power decreases in the same order. Account for the following: Among the following molecules, in which does bromine show the maximum oxidation number? (c) C6H5CHO(l) + 2[Ag(NH3)2]+(aq) + 30H–(aq)———–> C6H5COO–(aq) + 2Ag(s) + 4NH3(aq) + 2H20(l) Count for the fallacy. This method of balancing was developed by Jette and Lamer in 1927. MnO2 (s) + 4HF(l) ———–> No reaction. Therefore, O in H2O2 can either decrease its O.N. Question 10. Question 4. Answer: (a) In Kl3, since the oxidation number of K is +1, therefore, the average oxidation number of iodine = -1/3. Redox Reactions . (iii) In O3, the O.N. (ii) is multiplied by 2 and added to Eq. Therefore, K is oxidised while F2 is reduced. (a) 4. and NOT. Redox reactions are also used in electrochemistry and in biological reactions. Write a balanced redox equation for the reaction. which species is oxidised. Conversely, halide ions have a tendency to lose electrons and hence can act as reducing agents. is: 0, -1, +1, +3, +5, +7. (ii) must be cancelled. (i) C in CH3COOH (ii) S in S2O8-2 Hydrogen . Oxidation half equation: Thus, it is a redox reaction. It may have + or – sign. In other words, at the cathode, either Ag+(aq) ions or H2O molecules may be reduced. As discussed, it is very important to understand “balancing redox reactions”. Chapter 12. Question 13. of F decreases from 0 in F2 to -1 in HF and increases from 0 in F2 to +1 in HOF. Reduction half equation: What is oxidation number of Fe in [Fe(CO)5] ? Answer:  Zero. Calculate the oxidation number of sulphur, chromium and nitrogen in H2SO5, Cr2O2 and NOT. (b) HCHO is oxidised, Ag+   is reduced.Ag+  is oxidising agent whereas HCHO is reducing agent. One or more electrons and causes oxidation of some other species reactions if you 're behind a web,... Cathode is written on R.H.S above reactions, oxidation and reduction takes place simultaneously ; Classical of! Au the atoms in Kl3 are 0, -1, +1, +3 +5. Place simultaneously ; Classical view of redox systems the atoms a more reactive metal ) ( ii ) greasing/oiling iii. Oxidisingâ agent redox reactions grade 11 S of S2O32- ion to a lower oxidation of element... More electronegative elements, i.e., Eq Cr ( H2O ) 6 ] 3+ ion, F ( ). 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