The overall cell reaction occurring in an alkaline battery isZn(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.

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Q: current

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Q: Fe(s) |Fe2* (aq) ||CF (a9) | Cl2(g) | Pt(s)

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