{"id":40084,"date":"2024-02-19T08:05:40","date_gmt":"2024-02-19T02:35:40","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=40084"},"modified":"2024-02-19T12:45:45","modified_gmt":"2024-02-19T07:15:45","slug":"plus-one-chemistry-chapter-wise-previous-questions-chapter-8","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/plus-one-chemistry-chapter-wise-previous-questions-chapter-8\/","title":{"rendered":"Plus One Chemistry Chapter Wise Previous Questions Chapter 8 Redox Reactions"},"content":{"rendered":"

Plus One Chemistry Chapter Wise\u00a0Previous Questions\u00a0Chapter 8 Redox Reactions <\/strong>is part of Kerala Plus One Chemistry Chapter Wise Previous Year Questions and Answer<\/a> . Here we have given Plus One Chemistry Previous Questions Chapter 8 Redox Reactions.<\/p>\n

Kerala Plus One Chemistry Chapter Wise Previous Questions Chapter\u00a08 Redox Reactions<\/h2>\n

Question 1.
\nFill in the blanks. (March – 2009)<\/span>
\na) The oxidation state of Cl in HCI04 is …………
\nb) A reducing agent is a substance which ………… electrons in a chemical reaction.
\nc) Among the elements Flurine and Iodine, ………… exhibit both positive and negative oxidation states.
\nAnswer:
\na) HCIO4<\/sub>
\n1 + x + \u0394x- 2 = 0
\n1+ x – 8 = 0
\nx – 7 = 0
\nx = 7
\nb) donates
\nc) Iodine<\/p>\n

Question 2.
\nChemical reactions which involve oxidation and reduction are called redox reactions. The unbalanced equation in the ionic form of a redox reaction is shown below. (March – 2010)<\/span>
\na) Identify the oxidizing agent in this reaction.
\nb) Name the species getting oxidized in the above reaction.
\nc) Balance the above equation by the oxidation number method.
\n\"Plus
\nAnswer:
\n\"Plus<\/p>\n

Question 3.
\nA farmer prepared 1% solution of copper sulphate using iron rod as the stirrer for preparing Bordeaux mixture. Next day he notices that the blue color almost disappeared and the iron get coated with reddish brown material. (Say – 2010)<\/span>
\na) What is the reddish brown material deposited on the iron rod?
\nb) Account forthe color change of the solution.
\nc) Justify that the above phenomenon is a redox reaction.
\nAnswer:
\na) Copper is the reddish brown material deposited on the iron rod.
\nb) Due to salvated electrons.
\nc) Oxidation potential of Fe is greater than that of copper.<\/p>\n

Question 4.
\nBalance the following equation by the half reaction method. (March – 2012)<\/span>
\n\"Plus
\nAnswer:
\n\"Plus<\/p>\n

Question 5.
\nThe chemical reactions taking place in electro chemical cells are redox reactions. A Daniel cell is represented below. (Say – 2011)<\/span>
\n\"Plus
\na) Asthe reaction proceeds in this cell one of the metal rod gets dissolved in its solution and the other metal get deposited from the solution to the metal rod. Which metal is getting deposited?
\nb) Identify the metal which is acting as the oxidizing agent in this reaction.
\nc) Write the chemical equation of the reaction taking place at compartment A.
\nAnswer:
\na) Cu is deposited on the copper rod from the solution.
\nb) Cu2+<\/sup>(aq)<\/sub>\u00a0is the oxidising agent.
\nc) Zn(a)<\/sub> \u2192 Z2+<\/sup>(aq)<\/sub> + 2e-<\/p>\n

Question 6.
\nIn redox reactions, oxidation and reduction occur simultaneously.\u00a0(Say – 2011)<\/span>
\na) How are oxidation and reduction related to the oxidation number?
\nb) During a group discussion, one of your friends argues that thermal decomposition of KCIO3<\/sub> is a redox reaction while that of CaCO3<\/sub> is not a redox reaction. Give your opinion and substantiate.
\nAnswer:
\na) Oxidation is a chemical process in which there is an increase in the oxidation number of an element and reduction is a chemical process in which there is a decrease in the oxidation number of an element.<\/p>\n

\"Plus<\/p>\n

Both reactions are not a redox reaction. In both reaction there is no change in oxidation state ie no loss or gain of electorns.<\/p>\n

Question 7.
\na) Using stock notation, represent the following compounds. FeO and MnO2<\/sub>. (Say – 2012)<\/span>
\nb) Redox reactions are those reactions in which oxidation and reduction takes place simultaneously. Write any two redox reactions.
\nAnswer:
\na) FeO \u2192 Fe(ll) O – Iron (II) oxide
\nMnO2<\/sub> Mn(IV) O2<\/sub> \u2192 Manganese (IV) oxide
\nb) 1) H2<\/sub>O2<\/sub> \u2192 H2<\/sub>O + 1<\/sup>\/2<\/sub> O2<\/sub>
\n2) H2<\/sub>O + F2<\/sub> \u2192 HF + HOF are Redox reactions.<\/p>\n

Question 8.
\nCompetitive electron transfer reactions are utilized in the construction of Galvanic cells. (March – 2013)<\/span>
\na) Write the redox reaction involved when metallic cobalt is placed in a nickel sulphate solution. (Note : Only the ionic reaction is expected).
\nb) In the reaction Pb + PbO2(s)<\/sub> + 2H2<\/sub>\u00a0SO4(aq)<\/sub> \u2192 2PbSO4(s)<\/sub> + 2H2<\/sub>\u00a0O(i)<\/sub> identify the following:
\ni) Substance oxidied
\nii) Substance reduced
\niii) Oxidizing agent
\niv) Reducting agent?
\nAnswer:
\na) Co + Ni2+<\/sup> \u2192 CO2+\u00a0<\/sup>+ Ni
\nb) In the reats
\nPb0<\/sup>(s)<\/sub>\u00a0+ Pb+4<\/sup> O2(s)<\/sub> + 2H2<\/sub> SO4(aq)<\/sub> \u2192\u00a02 Pb+2<\/sup> SO4(aq)<\/sub> + 2H2<\/sub> O(i)<\/sub>
\ni) Substance oxidised \u2192 Pb
\nii) Substance reduced \u2192 PbO2<\/sub>
\niii) Oxidising agent \u2192 PbO2<\/sub>
\niv) reducing agent \u2192 Pb<\/p>\n

Question 9.
\na) Calculate the oxidation number of Cr in Cr2<\/sub>O3<\/sub> and S in H2<\/sub>SO4<\/sub>. (Say – 2013)<\/span>
\nb) In disproportionation reaction an element in one oxidation state is simultaneously oxidised and reduced. Identify the element undergoing disproportionation in the following reaction
\nP4<\/sub> + 3O\\(\\bar{H}\\) + 3H2<\/sub>O \u2192 PH3<\/sub> + 3H2<\/sub>PO2<\/sub>
\nAnswer:
\na) Oxidation number of Cr in Cr2<\/sub>O3<\/sub>:
\n2 x + 3(-2) = 0
\n2 x – 6 = 0 2x = 6
\nx = 3
\nOxidation number of S in H2<\/sub>SO4<\/sub>:
\n2(+1) + x + 4(-2) = 0
\n2 + x – 8 = 0
\nx = 6
\nb) Phosphorus is simultaneously is oxidised and reduced. Hence, the element undergoing disproportionation is P.<\/p>\n

Question 10.
\na) Write the formula of the following compounds. (March – 2014)<\/span>
\ni) Nickel Sulphate
\nii) Tin Oxide
\nb) Fluorine reacts with ice as given below:
\nH2<\/sub>O(s)<\/sub> + F2<\/sub>(g)<\/sub> \u2192 HF(g)<\/sub> + HOF(g)<\/sub>
\nJustify that this is a redox reaction.
\nAnswer:
\na) i) NiSO4<\/sub>
\nii) SnO2<\/sub>
\n\"Plus
\nIn this reaction oxidation number of F2<\/sub> changes from zero to -1 in HF and HOF whereas oxidation number of oxygen changes from -2 in H2<\/sub>O to zero in HOF. Thus, F2<\/sub> is reduced, whereas oxygen is oxidised and, therefore, it is a redox reaction.<\/p>\n

Question 11.
\na) Using stock notation, represent the following compounds: (August – 2014)<\/span>
\ni) HAUCI4<\/sub>
\nii) MnO2<\/sub>
\nb) i) Define the electronic concept of oxidation and reduction.
\nii) Find out the oxidizer and reducer in the following reaction on the basis of the electronic concept. 2Na(s)<\/sub> + Cl2<\/sub>(g)<\/sub> 2NaCI(s)<\/sub>
\nAnswer:
\na) i) HAU(III)CI4<\/sub>
\nii) Mn(IV)O2<\/sub>
\nb) i) Oxidation – Loss of electron(s) by any species. Reduction – Gain of electron(s) by any species,
\n\"Plus
\nOxidiser – Cl2<\/sub>, since it is the acceptor of electrons. Reducer – Na, since it is donor of electrons.<\/p>\n

Question 12.
\na) Given the redox reaction : (March – 2015)<\/span>
\n\"Plus
\ni) Identify the species which undergo reduction and which undergo oxidation.
\nii) Identify the reductant and oxidant in the above reaction.
\nb) Among the following reactions, identify the one which is NOT a redox reaction.
\n\"Plus
\nAnswer:
\n\"Plus
\nSpecies undergoing reduction – CuO
\nSpecies undergoing reduction – H2<\/sub><\/p>\n

ii) Reductant – H2<\/sub>
\nOxidant – CuO
\n\"Plus<\/p>\n

Question 13.
\nIdentify the oxidant and reduction in the following ionic equation and balance it using oxidation number method.
\n\"Plus\u00a0(March – 2015)<\/span>
\nAnswer:
\n\"Plus<\/p>\n

Question 14.
\nRedox reactions can be considered as electron transfer reactions. In an experiment a copper rod is dipped in Ag NO3<\/sub> solution. (March – 2016)<\/span>
\na) What happens to the colour of the solution and why?
\nb) Identify the oxidizing and reducing agent in this reaction.
\nc) Calculate the oxidation number of Cr in K2\u00a0<\/sub>Cr2<\/sub> O7<\/sub> and P in H2<\/sub>P2<\/sub>O5<\/sub>.
\nAnswer:
\na) The solution develops blue colour due to the formation of Cu2+<\/sup> ions on account of the reaction: Cu(s) + 2Ag+<\/sup>(aq) \u2192 Cu2+<\/sup>(aq) + 2Ag(s)
\nb) Here Ag+(aq) is the oxidising agent and Cu(s) is the reducing agent.
\nc) Oxidation number of Cr in K2<\/sub>\u00a0Cr2<\/sub>\u00a0O7\u00a0<\/sub>is +6
\nOxidation number of P in H4<\/sub>P2<\/sub>O5<\/sub> is +4
\n(Actually, the compound is H4<\/sub>P2<\/sub>O5<\/sub> in which oxidation state of P is +3)<\/p>\n

Question 15.
\nIn a redox reaction, reduction and oxidation takes place simultaneously.\u00a0(Say – 2016)<\/span>
\na) Write the reclox reaction \u00a1n Daniefl cell.
\nb) When CuSO4<\/sub> solution stored in iron vessel, the blue colour changes to pale green. Do you agree with it? Justify.
\nAnswer:
\na) Zn(s) + Cu2+\u00a0<\/sup>(aq) \u2192 Zn2+\u00a0<\/sup>(aq) + Cu(s)
\nb) Yes.
\nSince Fe is more reactive than Cu it displaces Cu from CuSO4<\/sub> solution to form pale green coloured FeSO4<\/sub>.
\nCuSO4<\/sub>(aq) + Fe(s) \u2192 Cu(s) + FeSO4<\/sub>(aq)<\/p>\n

Question 16.
\nPermanganate ion reacts with bromide ion in basic medium to give manganese dioxide and bromate ion., Write the balanced equation for the reaction using oxidation number method. Skeletal equation is MnO4<\/sub> + Br \u2192 MnO2<\/sub> + BrO3<\/sub>. (March – 2017)<\/span>
\nAnswer:
\nStep 1: The skeletal equation is: MnO4<\/sub>(aq) + Br(aq) \u2192 MnO2<\/sub>(s) + BrO3<\/sub>(aq)
\nStep 2: Assign oxidation numbers for Mn and Br
\n\"Plus
\nStep 3: Calculate the increase and decrease of oxidation number, and make the increase equal to the decrease by multiplying with a suitable number.
\n\"Plus
\nStep 4: As the reaction occurs in the basic medium, and the ionic charges are not equal on both sides, add 20H- ions on the right to make ionic charges equal.
\n\"Plus
\nStep 5:Count the hydrogen atoms and add an appropriate number of water molecules (i.e., one H20 molecule) on the left side to achieve a balanced redox change.
\n\"Plus<\/p>\n

We hope the Kerala Plus One Chemistry Chapter Wise Previous Questions Chapter 8 Redox Reactions help you. If you have any query regarding Kerala Plus One Chemistry Chapter Wise Previous Questions Chapter 8 Redox Reactions, drop a comment below and we will get back to you at the earliest.<\/p>\n","protected":false},"excerpt":{"rendered":"

Plus One Chemistry Chapter Wise\u00a0Previous Questions\u00a0Chapter 8 Redox Reactions is part of Kerala Plus One Chemistry Chapter Wise Previous Year Questions and Answer . Here we have given Plus One Chemistry Previous Questions Chapter 8 Redox Reactions. Kerala Plus One Chemistry Chapter Wise Previous Questions Chapter\u00a08 Redox Reactions Question 1. Fill in the blanks. (March […]<\/p>\n","protected":false},"author":7,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[42728],"tags":[],"yoast_head":"\nPlus One Chemistry Chapter Wise Previous Questions Chapter 8 Redox Reactions - A Plus Topper<\/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:\/\/www.aplustopper.com\/plus-one-chemistry-chapter-wise-previous-questions-chapter-8\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Plus One Chemistry Chapter Wise Previous Questions Chapter 8 Redox Reactions\" \/>\n<meta property=\"og:description\" content=\"Plus One Chemistry Chapter Wise\u00a0Previous Questions\u00a0Chapter 8 Redox Reactions is part of Kerala Plus One Chemistry Chapter Wise Previous Year Questions and Answer . 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Here we have given Plus One Chemistry Previous Questions Chapter 8 Redox Reactions. Kerala Plus One Chemistry Chapter Wise Previous Questions Chapter\u00a08 Redox Reactions Question 1. Fill in the blanks. 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