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A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer? for Class 12 2025 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 12 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer?.

Solutions for A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12. Download more important topics, notes, lectures and mock test series for Class 12 Exam by signing up for free.

Here you can find the meaning of A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer?, a detailed solution for A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer? has been provided alongside types of A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+ / Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V.The favourable redox reaction is : [2011 M]a)I2 will be reduced to I–b)There will be no redox reactionc)I– will be oxidised to I2d)Fe2+ will be oxidised to Fe3+Correct answer is option 'C'. Can you explain this answer? tests, examples and also practice Class 12 tests.