Using the balanced equation below, how many grams of manganese(III)
oxide would be produced from the
complete reaction of 46.8 g of zinc?
Zn + 2MnO2 + H20 — Zn(OH)2 + Mn203

The mass of manganese(III) oxide produced is 113.03 g

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

......(1)

Given mass of zinc = 46.8 g

Molar mass of zinc = 65.38 g/mol

Plugging values in equation 1:

The given chemical equation follows:

By the stoichiometry of the reaction:

If 1 mole of zinc produces 1 mole of manganese(III) oxide

So, 0.716 moles of zinc will produce = of manganese(III) oxide

Molar mass of manganese(III) oxide = 157.87 g/mol

Plugging values in equation 1:

Hence, the mass of manganese(III) oxide produced is 113.03 g

(b) which contains higher levels of vitamin b, oranges or spinach?

explanation:

you can eliminate a, c, and d because they are questions based on opinions.