Question

Using the following balanced equation to the question that follows.

1 Zn + 2 MnO2 + 1 H2O → 1 Zn(OH)2 + 1 Mn2O3



How many moles of MnO2 are needed to produce 8.54 moles of Zn(OH)2?

Answer 1

17.08 moles of manganese dioxide

Step-by-step explanation:

From the balanced reaction equation;

Zn + 2 MnO2 + 1 H2O → Zn(OH)2 + Mn2O3 (notice that I did not put 1 as a stoichiometric coefficient. It is expected that any specie written without a coefficient should have a coefficient of 1)

It is clear from the reaction equation that 2 moles of manganese dioxide produced 1 mole of zinc II hydroxide

Hence x moles of manganese dioxide will produce 8.54 moles of zinc II hydroxide

x= 2× 8.54/1

x= 17.08 moles of manganese dioxide