Question

The overall cell reaction occurring in an alkaline battery isZn(s) + MnO₂(s) + H₂O(l) → ZnO(s) + Mn(OH)₂(s) (b) If 4.50 g of zinc is oxidized, how many grams of manganese dioxide and of water are consumed?

Answer 1

5.911 grams of manganese dioxide and 1.224 gram of water are consumed.

What is Balanced Chemical Equation ?

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.

The given reaction balanced equation is:

Zn(s) + MnO₂(s) + H₂O(l) → ZnO(s) + Mn(OH)₂(s)

How to find the number of moles ?

To find the number of moles use the expression:

Number of moles = $\frac{\text{Given mass}}{\text{Molar mass}}$

Here,

Mass of Zn = 4.50 g

Molar mass of Zn = 65.4 g/mol

Now put the value in above expression

Number of moles of Zn = $\frac{\text{Given mass}}{\text{Molar mass}}$

                                       = $\frac{4.5\ g}{65.4\ \text{g/mol}}$

                                       = 0.068 mol

Mass of MnO₂ = Moles of MnO₂ × Molar mass of MnO₂

                        = 0.068 mol × 86.9368 g/mol

                         = 5.911 g

Mass of H₂O = Moles of H₂O × Molar mass of H₂O

                     = 0.068 mol × 18.0 g/mol

                     = 1.224 g

Thus from the above conclusion we can say that 5.911 grams of manganese dioxide and 1.224 gram of water are consumed.

                 

Learn more about the Balanced chemical equation here: brainly.com/question/26694427

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