Balancing Redox Equations with KClO: Problem 10b Explained

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In summary, when balancing redox equations, it is necessary to use appropriate coefficients to ensure that the total increase in oxidation number is equal to the total decrease in oxidation number. In this case, the coefficient 3/2 is used to balance the oxygen gas on the product side since it is the only compound whose oxidation number is changing.
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Yaqout
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Balancing Redox equations (pg. 607-8)

Step 4: Make the total increase in oxidation number equal to the total decrease in oxidation number by using appropriate coefficients.
Practice problem 10b.

KClO (s)==>KCl(aq) + O2(g)

When I did step 4 of this equation, I was unable to understand why and how the fraction 3/2 is put in front of the oxygen gas in the product side. And also why oxygen is chosen from all the other compounds to place the coefficient infront. I would like this point clarified because its been hindering me of comprehending and solving similar equations.
 
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The coefficient 3/2 is placed in front of the oxygen gas on the product side because that is what is necessary to ensure that the total increase in oxidation number is equal to the total decrease in oxidation number. In this equation, the oxidation number of chlorine increases from -1 to 0, while the oxidation number of potassium stays the same. Therefore, the oxidation number of oxygen must decrease from 0 to -1/2. Therefore, to make the total increase in oxidation number equal to the total decrease in oxidation number, you need to multiply the oxygen on the product side by 3/2. The reason why oxygen is chosen from all the other compounds is because it is the only compound whose oxidation number is changing.
 
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In order to balance a redox equation, we must ensure that the total increase in oxidation number is equal to the total decrease in oxidation number. This means that the number of electrons lost in the oxidation half-reaction must be equal to the number of electrons gained in the reduction half-reaction.

In the given equation, KClO is the oxidizing agent, which means it is being reduced. This means that the oxygen in KClO is gaining electrons and its oxidation number is decreasing from +2 to 0. On the other hand, oxygen in O2 is the reducing agent, which means it is being oxidized. This means that the oxygen in O2 is losing electrons and its oxidation number is increasing from 0 to -2.

To balance the equation, we need to make sure that the total increase in oxidation number is equal to the total decrease in oxidation number. In this case, the oxygen atoms in KClO are decreasing in oxidation number by 2 (from +2 to 0) and there are 3 oxygen atoms in KClO, so the total decrease in oxidation number is 6. On the other hand, the oxygen atoms in O2 are increasing in oxidation number by 2 (from 0 to -2) and there are 2 oxygen atoms in O2, so the total increase in oxidation number is also 4. To make these numbers equal, we need to multiply O2 by 3/2, which gives us 3O2 on the product side, making the total increase in oxidation number equal to the total decrease in oxidation number (3*2=6).

The reason why we chose to put the coefficient in front of oxygen is because it is the only element that is changing oxidation number in this equation. All other elements have a constant oxidation number. Therefore, in order to balance the equation, we need to adjust the number of oxygen atoms.

I hope this explanation clarifies your doubts and helps you understand how to balance redox equations more easily. Keep practicing and you will become more familiar with the process.
 

What is a redox equation?

A redox equation is a type of chemical equation that represents a chemical reaction where there is a transfer of electrons between the reacting species. This transfer of electrons can result in a change in oxidation states and the formation of new products.

Why is it important to balance redox equations?

Balancing redox equations is important because it ensures that the reaction follows the law of conservation of mass. This means that the number of each type of atom on the reactant side must be equal to the number on the product side. Additionally, balancing the equation allows for accurate stoichiometric calculations and predictions of the products formed.

How do you balance a redox equation with KClO?

There are a few steps to follow when balancing a redox equation with KClO specifically. First, write the unbalanced equation and identify the species that are being oxidized and reduced. Next, balance the atoms other than oxygen and hydrogen. Then, balance the oxygen atoms by adding water molecules to the side that needs oxygen. After that, balance the hydrogen atoms by adding H+ ions to the side that needs hydrogen. Finally, balance the charges by adding electrons to one or both sides of the equation. Once all steps are completed, the equation should be balanced.

What is the purpose of using KClO in a redox reaction?

KClO, or potassium chlorate, is often used in redox reactions as an oxidizing agent. This means that it is able to accept electrons from other species and become reduced itself. KClO is typically used in reactions where oxygen is needed, as it can release oxygen gas when heated.

How can I check if a redox equation with KClO is balanced?

To check if a redox equation with KClO is balanced, you can use the following method: count the number of each type of atom on both sides of the equation. If the numbers are equal, the equation is balanced. Additionally, you can check if the charges are balanced on both sides, and if the oxidation states of the species are consistent with the transfer of electrons. If all of these criteria are met, the equation is balanced.

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