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Stoichiometry and Multiplying Electrons

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Complete and balance the following reaction:
As(s)+ClO3^-(aq) (right arrow) H3AsO3(aq)+HCLO (aq)

I have the following options:
-split into 1/2 reactions
-balance all but H and O
-balance O by adding H20
-balance H+ by adding protons
-balance charge by adding electrons

I am stuck, after adding equations to get electrons to cancel each other out, in what you need to multiply by these numbers with. This is where I have ended.

As+3H20+3e^- (right arrow) H3AsO3+3H+
CLO3^- +5H+ (right arrow) HCLO+2H2O+5e^-

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https://brainmass.com/chemistry/reaction-stoichiometry/30340

Solution Preview

Generally, you're putting your electrons on the wrong side of the equation. They should be on the same side as the hydrogen ions, so as to balance the charges. Notice this first half-reaction is completely balanced. Each chemical is ...

Solution Summary

This solution addresses how to balance a specific chemical reaction. This is achieved by balancing all the electrons within the equation and summing them all up, after excess species are taken out.

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Redox Reaction: Ferrous Ion and Permanganate Ion

The ferrous ion, Fe2+(aq), reacts with the permanganate ion, MnO4- (aq), in an acidic solution to produce the ferric ion, Fe3+(aq). A 6.893 g sample of ore was mechanically crushed and tehn treated with concentrated hydrochloric acid, which oxidized all of the iron in the ore to the ferrous ion, Fe2+(aq). Next the acid solution containing all of the ferrous ions was titrated with .100 M KMnO4 solution. The end point was reached when 13.899mL of the KMnO4 solution was used.

a. Write the oxidation half reaction
b. Write the reduction half reaction
c. Write the balanced final redox reaction
d. Identify the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced
e. Calculate the number of moles of iron in the sample or ore
f. Calculate the mass percent of the iron in the ore

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