The overall cell reaction occurring in an alkaline battery is                                  Zn(s) + MnO2(s) + H2O(l) → ZnO(s) + Mn(OH)2(s)(a) How many moles of electrons flow per mole of reaction?(b) If 4.50 g of zinc is oxidized, how many grams of manganese dioxide and of water are consumed?(c) What is the total mass of reactants consumed in part (b)?(d) How many coulombs are produced in part (b)?(e) In practice, voltaic cells of a given capacity (coulombs) are heavier than the calculation in part (c) indicates. Explain.

Q: Consider the voltaic cell illustrated in the figure (Figure 1), which is based on the cell reaction…

A: G = -nFE = J/mol Zn(s)-->Zn^2+(aq)+2e^- 0.765 V Cu^2+(aq)+2e^- -->Cu(s) 0.337 V   n = 2, F =…

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Q: The overall cell reaction occurring in an alkaline battery is Zn(s) +MnO₂(s) +H₂O(l) →ZnO(s)…

A: (a) The given reaction is separated into two half reactions as follows,  Observing the above half…

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Q: (19) Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu²+ (aq) →…

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Q: Balance the following redox reaction in acidic solution. NO(9)+Fe (aq) → " (aq) NO3(aq)+Fe "(aq)

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