Suppose the redox reaction in a certain zinc-carbon battery is Zn + 2 MnO₂ +2 NH₄ Cl$\rightarrow$ MN₂ O₃ + Zn(NH₃ )2 CL₂ + H₂ O.The battery is rated at 0.75 W _• hr at 1.5 V.How many grams of zinc must be oxidized to deliver this much electrical energy?

Question

Quizplus · Accepted Answer

To find the grams of zinc oxidized, calculate the moles of electrons transferred using the energy (0.75 Wh = 2700 J) and the voltage (1.5 V). Then, use the stoichiometry of the reaction to find the moles of zinc oxidized and convert to grams. The calculation shows that approximately 0.61 g of zinc is needed.

Suppose the Redox Reaction in a Certain Zinc-Carbon Battery Is →\rightarrow→

Suppose the Redox Reaction in a Certain Zinc-Carbon Battery Is $\rightarrow$