During a period of discharge of a lead–acid battery, 402 g of Pb from the anode is converted into PbSO41s2. (a) What mass of PbO21s2 is reduced at the cathode during this same period?

Video transcript

Hi everyone here we have a question that tells us an alkaline battery has the following overall reaction to manganese dioxide solid plus sink solid plus two water liquid forms manga to manga night plus zinc hydroxide solid. In a certain period of discharge, 131 g of zinc from the anad was converted into zinc hydroxide solid, calculate the amount in grams of manganese dioxide solid that is reduced at the cathode at the same time. So our more mass of zinc is .39 g per mole. Our more mass of manganese dioxide is 54 . g per mole plus 16 zero g per mole times two Equals 86. g per mole. Our mass of mega knees dioxide equals g of zinc Times one mole of zinc over 65.39 grams of zinc, times two moles of manganese dioxide Over one mole of zinc times 86 . g of manganese dioxide over one mole of manganese dioxide. So our grams of zinc are canceling out our molds of zinc are canceling out our moles of manganese docks that are canceling out, leaving us with 348 g of manganese dioxide. And that is our final answer. Thank you for watching. Bye.