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Chapter 4: Problem 41

Is it possible to have a reaction in which oxidation occurs and reduction does not? Explain.

Short Answer

Expert verified
No, it's not possible. Oxidation and reduction reactions are two halves of the same process. For oxidation to occur, reduction must also occur, because the electrons lost during oxidation have to be gained by another substance, indicating reduction. This is why they are always paired together in a redox reaction.

Step by step solution

01

Understanding Redox Reactions

Redox (or reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation states changed. In other words, redox reactions are a family of reactions that are concerned with the transfer of electrons between species.
02

Defining Oxidation and Reduction

Oxidation is defined as a process where a substance loses electrons. On the other hand, reduction is a process in which a substance gains electrons. Both these processes occur simultaneously in a redox reaction.
03

Analyzing the Interdependence of Oxidation and Reduction

The two halves of a redox reaction, oxidation and reduction, cannot occur independently. If a substance is oxidized, it means it has lost electrons, but those electrons have to be gained by another substance; hence reduction takes place. Oxidation and reduction always occur together, meaning if one substance is getting oxidized, another substance must be getting reduced. This relationship between oxidation and reduction is commonly known as 'redox pair'.

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Most popular questions from this chapter

Classify the following redox reactions. (a) \(2 \mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}\) (b) \(\mathrm{Mg}+2 \mathrm{AgNO}_{3} \longrightarrow \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}+2 \mathrm{Ag}\) (c) \(\mathrm{NH}_{4} \mathrm{NO}_{2} \longrightarrow \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{H}_{2}+\mathrm{Br}_{2} \longrightarrow 2 \mathrm{HBr}\)

What volume of \(0.416 M \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) should be added to \(255 \mathrm{~mL}\) of \(0.102 \mathrm{M} \mathrm{KNO}_{3}\) to produce a solution with a concentration of \(0.278 M \mathrm{NO}_{3}^{-}\) ions? Assume volumes are additive.

A 3.664 -g sample of a monoprotic acid was dissolved in water. It took \(20.27 \mathrm{~mL}\) of a \(0.1578 \mathrm{M}\) \(\mathrm{NaOH}\) solution to neutralize the acid. Calculate the molar mass of the acid.

Write the equation that enables us to calculate the concentration of a diluted solution. Give units for all the terms.

Oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) is present in many plants and vegetables. If \(24.0 \mathrm{~mL}\) of \(0.0100 \mathrm{M} \mathrm{KMnO}_{4}\) solution is needed to titrate \(1.00 \mathrm{~g}\) of a sample of \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) to the equivalence point, what is the percent by mass of \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) in the sample? The net ionic equation is \(2 \mathrm{MnO}_{4}^{-}+16 \mathrm{H}^{+}+5 \mathrm{C}_{2} \mathrm{O}_{4}^{2-} \longrightarrow\) \(2 \mathrm{Mn}^{2+}+10 \mathrm{CO}_{2}+8 \mathrm{H}_{2} \mathrm{O}\)
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