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Verification of Tafel Equation
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 1) An electrolytic cell: Has a non-spontaneous chemical reaction None of the above All of the above Requires application of a negative potential to make the reaction occur Has a positively charged anode

 2) If we pass a current of 10.0 Amperes through a solution for 1 hour, how many moles of electrons are used? 10 x 1 x 3600 / 96487 10 x 1 10 x 1 x 3600 x 96487 10 x 1 x 3600 none of the above

 3) The REDOX reaction Zn(s) + Cu²⁺(aq) = Zn²⁺(aq) + Cu(s) has E₀ = +1.10 V. The standard free energy for this reaction can be calculated as..... DG₀ = - 3 (96487) (1.10) J/mol DG₀ = 96487 (1.10) J/mol DG₀ = - 96487 (1.10) J/mol DG₀ = - 2 (96487) (1.10) J/mol DG₀ = 2 (96487) (1.10) J/mol

 4) The fuel cell we discussed in class forms the following product. H₂SO₄ H₂S O₂ H₂ H₂O

 5) The electric charge or electrode deposition of one gram equivalent of a substance is ..... one ampere for one hour 96,500 coulombs per second one ampere for one second charge on one mole of electrons

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