A silver button battery used in a watch contains 0.75 g of zinc and can run until 80% of the zinc is consumed.(b) When the battery dies, 95% of the Ag₂O has been consumed.How many grams of Ag were used to make the battery?

The balanced chemical equation is the equation in which the number of atoms on the reactant side is equal to the number of atoms on the product side in an equation.

Now write the balanced chemical equation

Zn + Ag₂O → ZnO + 2Ag

What is Stoichiometry ?

Stoichiometry helps us use the balanced chemical equation to measure quantitative relationships and it is to calculate the amount of products and reactants that are given in a reaction.

According to stoichiometry

[tex]0.00917\ \text{mol Zn} \times \frac{1\ \text{mol}\ Ag_2O}{1\ \text{mol}\ Zn} \times \frac{2\ \text{mol}\ Ag}{\text{mol}\ Ag_2O} \times \frac{107.9\ g\ Ag}{\text{mol}\ Ag}[/tex]

= 1,98 g Ag

For 100% consumption of Ag₂O obtain

[tex]\frac{1.98\ g\ Ag}{95\%\ Ag_2O} \times 100\%\ Ag_2O[/tex]

= 2.1 g Ag

Thus from the above conclusion we can say that 2.1 grams of Ag were used to make the battery.

Learn more about the Stoichiometry here: https://brainly.com/question/14935523

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