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What mass of zinc hydroxide (Zn(OH)2) will be produced if 25.0g Zn and 30.0g MnO2 react in a battery according to the following reaction: Be sure to check the limiting reactant.

Zn + 2MnO2 + H2O → Zn(OH)2 + Mn2O3

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mickymike92

Based on the limiting reactant, the mass of Zn(OH)2 produced is 38.0 g

What is a limiting reactant?

A limiting reactant is used up in a reaction and the reaction stops afterwards.

Equation of reaction:

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

From the equation of the reaction, 1 mole of Zn reacts with 2 moles of MnO2 to produce 1 mole of Zn(OH)2

Molar mass of Zn = 65 g

Molar mass of MnO2 = 56 g

Molar mass of Zn(OH)2 = 99.0 g

Moles of An reacting = 25/65 = 0.38 moles

Moles of MnO2 reacting = 30/56 = 0.5

Therefore, MnO2 is the limiting reactant.

Mass of Zn(OH)2 produced = 25 × 99/65

Mass of Zn(OH)2 produced = 38.0 g of Zn(OH)2

Learn more about limiting reactant at: https://brainly.com/question/24945784

CintiaSalazar

Taking into account the reaction stoichiometry and limiting reagent, 17.14 grams of Zn(OH)â‚‚ will be produced if 25.0g Zn and 30.0g MnOâ‚‚ react.

Reaction stoichiometry

In first place, the balanced reaction is:

Zn + 2 MnO₂ + H₂O  → Zn(OH)₂ + Mn₂O₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • Zn: 1 mole
  • MnOâ‚‚: 2 moles
  • Hâ‚‚O: 1 mole  
  • Zn(OH)â‚‚: 1 mole
  • Mnâ‚‚O₃: 1 mole

The molar mass of the compounds is:

  • Zn: 65.37 g/mole
  • MnOâ‚‚: 86.94 g/mole
  • Hâ‚‚O: 18 g/mole
  • Zn(OH)â‚‚: 99.37 g/mole
  • Mnâ‚‚O₃: 157.88 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

  • Zn: 1 mole ×65.37 g/mole= 65.37 grams
  • MnOâ‚‚: 2 moles ×86.94 g/mole=  173.88 grams
  • Hâ‚‚O: 1 mole ×18 g/mole= 18 grams
  • Zn(OH)â‚‚: 1 mole ×99.37 g/mole= 99.37 grams
  • Mnâ‚‚O₃: 1 mole ×157.88 g/mole= 157.88 grams

Definition of limiting reagent

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

Limiting reaction of this reaction

To determine the limiting reagent, it is possible to use the reaction stoichiometry of the reaction and a simple rule of three as follows: if by stoichiometry 65.37 grams of Zn reacts with 173.88 grams of MnOâ‚‚, 25 grams of Zn react with how much mass of MnOâ‚‚?

[tex]mass of MnO_{2} =\frac{25 grams of Znx173.88 grams of MnO_{2} }{65.37 grams of Zn}[/tex]

mass of MnOâ‚‚= 66.5 grams

But 66.5 grams of MnOâ‚‚ are not available, 30 grams are available. Since you have less mass than you need to react with 30 grams of Zn, MnOâ‚‚ will be the limiting reagent.

Mass of zinc hydroxide Zn(OH)â‚‚ produced

The following rules of three can be applied, considering the limiting reaction: if by reaction stoichiometry 173.88 grams of MnOâ‚‚ form 99.37 grams of Zn(OH)â‚‚, 30 grams of MnOâ‚‚ form how much mass of Zn(OH)â‚‚?

[tex]mass of Zn(OH)_{2} =\frac{30 grams of MnO_{2}x99.37 grams of Zn(OH)_{2} }{173.88 grams of MnO_{2}}[/tex]

mass of Zn(OH)â‚‚= 17.14 grams

Finally, 17.14 grams of Zn(OH)â‚‚ will be produced if 25.0g Zn and 30.0g MnOâ‚‚ react.

Learn more about the reaction stoichiometry:

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