Chemistry, 26.02.2022 08:50 sebastianmettsovghhk

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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Taking into account the reaction stoichiometry and limiting reagent, 17.14 grams of Zn(OH)₂ will be produced if 25.0g Zn and 30.0g MnO₂ 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 MnO₂: 2 moles H₂O: 1 mole Zn(OH)₂: 1 mole Mn₂O₃: 1 mole

The molar mass of the compounds is:

Zn: 65.37 g/moleMnO₂: 86.94 g/mole H₂O: 18 g/moleZn(OH)₂: 99.37 g/moleMn₂O₃: 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 gramsMnO₂: 2 moles ×86.94 g/mole= 173.88 gramsH₂O: 1 mole ×18 g/mole= 18 gramsZn(OH)₂: 1 mole ×99.37 g/mole= 99.37 gramsMn₂O₃: 1 mole ×157.88 g/mole= 157.88 gramsDefinition 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 MnO₂, 25 grams of Zn react with how much mass of MnO₂?

$mass of MnO_{2} =\frac{25 grams of Znx173.88 grams of MnO_{2} }{65.37 grams of Zn}$

mass of MnO₂= 66.5 grams

But 66.5 grams of MnO₂ are not available, 30 grams are available. Since you have less mass than you need to react with 30 grams of Zn, MnO₂ will be the limiting reagent.

Mass of zinc hydroxide Zn(OH)₂ produced

The following rules of three can be applied, considering the limiting reaction: if by reaction stoichiometry 173.88 grams of MnO₂ form 99.37 grams of Zn(OH)₂, 30 grams of MnO₂ form how much mass of Zn(OH)₂?

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

mass of Zn(OH)₂= 17.14 grams

Finally, 17.14 grams of Zn(OH)₂ will be produced if 25.0g Zn and 30.0g MnO₂ react.

Learn more about the reaction stoichiometry:

Answer from: Quest

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.

Answer from: Quest

its mg hope this

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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...

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