Question Description
At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer?.

Solutions for At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE. Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.

Here you can find the meaning of At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer?, a detailed solution for At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer? has been provided alongside types of At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice At 298K the standard free energy of formation of H2O(l) is –257.20 kJ/mole while that of its ionisation into H+ ions and OH– ions is 80.35 kJ/mole, then the emf of the following cell at 298 K will be (Take F = 96500 C] :H2(g,1 bar) | H+ (1M) || OH¯ (1M) | O2 (g, 1bar)a)0.40 Vb)0.50 Vc)1.23 Vd)– 0.40 VCorrect answer is option 'B'. Can you explain this answer? tests, examples and also practice JEE tests.