When the nickel–zinc battery, used in digital cameras, is recharged, the following cell reaction occurs: (a) How many grams of zinc are formed when 3.35 x 10^-2 g of Ni(OH)₂ are consumed?

Video transcript

Hello. In this problem, we are told the alkaline batteries are used in most household items. The overall cell reaction is given below where asked to calculate the mass of zinc oxide produced when 6.25 times 10 to minus two g of manganese dioxide reacts. So we have 6.25 times 10 to the negative two grams of manganese dioxide. And we have one mole uh manganese dioxide Having a mass of 86.937 g. We then make use of the balanced reaction equation and we have then two moles of manganese dioxide for every one mole of zinc oxide and will make use of the more mass of zinc oxide. One more zinc oxide has a mass of 81.379 g. So our grams and manganese dioxide cancels our molds of manganese dioxide cancels, our molds of zinc oxide cancels and we're left with then 0.293 g zinc oxide. So this is the mass of zinc oxide that can be produced from 6.25 times 2 -2 g of magnesium oxide. This corresponds then to answer a thanks for watching