In the following reactions, decide which reactant is...

In the following reactions, decide which reactant is oxidized and which is reduced. Designate the oxidizing agent and the reducing agent. (a) $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+3 \mathrm{Sn}^{2+}(\mathrm{aq})+14 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow$ $2 \mathrm{Cr}^{3+}(\mathrm{aq})+3 \mathrm{Sn}^{4+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\ell)$ (b) $\mathrm{FeS}(\mathrm{s})+3 \mathrm{NO}_{3}^{-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow$ $3 \mathrm{NO}(\mathrm{g})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{Fe}^{3+}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$

In the following reactions, decide which reactant is oxidized and which is reduced. Designate the oxidizing agent and the reducing agent.
(a) $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+3 \mathrm{Sn}^{2+}(\mathrm{aq})+14 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow$
$2 \mathrm{Cr}^{3+}(\mathrm{aq})+3 \mathrm{Sn}^{4+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\ell)$
(b) $\mathrm{FeS}(\mathrm{s})+3 \mathrm{NO}_{3}^{-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow$
$3 \mathrm{NO}(\mathrm{g})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{Fe}^{3+}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$

Key Concepts

Redox Reactions

Redox reactions are chemical reactions that involve the transfer of electrons between reactants. These reactions consist of two complementary processes: oxidation, where a species loses electrons, and reduction, where a species gains electrons. Understanding redox reactions is fundamental to many areas of chemistry, including energy conversion and metabolism.

Oxidation

Oxidation is the process in a chemical reaction where a species loses electrons, leading to an increase in its oxidation state. This change is critical for identifying the species undergoing oxidation in a redox reaction and understanding how electron transfer drives chemical transformations.

Reduction

Reduction is the process in which a chemical species gains electrons, resulting in a decrease in its oxidation state. Recognizing reduction is important for determining which reactant is being reduced and for balancing redox equations appropriately.

Oxidizing Agent

An oxidizing agent is the species that accepts electrons in a redox reaction, thereby getting reduced. It is responsible for driving the oxidation of another species and plays a key role in facilitating electron transfers in many chemical processes.

Reducing Agent

A reducing agent donates electrons during a redox reaction and, in doing so, is oxidized. It initiates the reduction process in another reactant and is essential for the progress of redox reactions by providing the necessary electrons.

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