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The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer? for Class 11 2025 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 11 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer?.

Solutions for The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11. Download more important topics, notes, lectures and mock test series for Class 11 Exam by signing up for free.

Here you can find the meaning of The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer?, a detailed solution for The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer? has been provided alongside types of The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice The more positive the value of E0, the greater is 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.E0values : Fe3 + / Fe2+ = +0.77; I2(s)/l-= +0.54; cu2+/ Cu = +0.34; Ag+/ Ag = +0.80Va)Ag+b)Fe3+c)I2 (s)d)Cu2+Correct answer is option 'A'. Can you explain this answer? tests, examples and also practice Class 11 tests.