Chemistry, 02.10.2019 01:30 TerronRice

For a particular redox reaction bro– is oxidized to bro3– and fe3 is reduced to fe2 . complete and balance the equation for this reaction in basic solution. phases are optional.

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Answer : The balanced chemical equation in a basic solution will be,

$BrO^-+4OH^-+4Fe^{3+}\rightarrow BrO_3^-+2H_2O+4Fe^{2+}$

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Rules for the balanced chemical equation in basic solution are :

First we have to write into the two half-reactions.Now balance the main atoms in the reaction.Now balance the hydrogen and oxygen atoms on both the sides of the reaction.If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the more number of oxygen are present.If the hydrogen atoms are not balanced on both the sides then adding hydroxide ion (OH^-)

at that side where the less number of hydrogen are present.Now balance the charge.

The oxidation-reduction half reaction will be :

Oxidation : $BrO^-+4OH^-\rightarrow BrO_3^-+2H_2O+4e^-$

Reduction : $Fe^{3+}+1e^-\rightarrow Fe^{2+}$

In order to balance the electrons, we multiply the reduction reaction by 4 and then added both equation, we get the balanced redox reaction.

The balanced chemical equation in a basic solution will be,

$BrO^-+4OH^-+4Fe^{3+}\rightarrow BrO_3^-+2H_2O+4Fe^{2+}$

Answer from: Quest

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

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For a particular redox reaction bro– is oxidized to bro3– and fe3 is reduced to fe2 . complete and b...

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