Question Description
An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer?.

Solutions for An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for Chemistry. Download more important topics, notes, lectures and mock test series for Chemistry Exam by signing up for free.

Here you can find the meaning of An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer?, a detailed solution for An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice An electrochemical cell consists of two half-cell reactionsAgCl(s) + e– → Ag(s) + Cl–(aq)Cu(s) → Cu2+(aq) + 2e–The mass of copper (in grams) dissolved on passing 0.5 A current for 1 hour is[Given: atomic mass of Cu is 63.6; F = 96500 C mol–1]a)0.88b)1.18c)0.29d)0.59Correct answer is option 'D'. Can you explain this answer? tests, examples and also practice Chemistry tests.