Question

The standard reduction potential of \(\mathrm{Eu}^{2+}(a q)\) is \(-0.43 \mathrm{V}\) . Using Appendix E, which of the following substances is capable of reducing Eu' \((a q)\) to \(\mathrm{Eu}^{2+}(a q)\) under standard conditions: Al, Co, \(\mathrm{H}_{2} \mathrm{O}_{2}, \mathrm{N}_{2} \mathrm{H}_{5}^{+}, \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} ?\)

Short answer

The substances that can reduce Eu'(aq) to Eu²⁺(aq) under standard conditions are Hydrogen Peroxide (H₂O₂) and Oxalic Acid (H₂C₂O₄).

Step-by-step solution

Find the standard reduction potentials of the given substances

To know which substance can reduce Eu'(aq) to Eu²⁺(aq), we need to find the standard reduction potentials of all given substances: Al, Co, H₂O₂, N₂H₅⁺, and H₂C₂O₄. These values can be found in Appendix E. Let's list them down: - Al: Given as Al³⁺(aq) + 3e⁻ → Al, E° = -1.66 V - Co: Given as Co²⁺(aq) + 2e⁻ → Co, E° = -0.28 V - H₂O₂: Given as H₂O₂(aq) + 2H⁺ + 2e⁻ → 2H₂O(l), E° = 1.77 V - N₂H₅⁺: Given as N₂H₅⁺(aq) + 3H₂O(l) → N₂(g) + 8H⁺ + 8e⁻, E° = -0.60 V - H₂C₂O₄: Given as H₂C₂O₄(aq)+ 2H⁺ + 2e⁻ → 2CO₂(g) + 2H₂O(l), E° = 0.575 V We also have the standard reduction potential of Eu²⁺(aq) provided in the question: Eu²⁺(aq) + 2e⁻ → Eu, E° = -0.43 V. Now that we have the values, let's compare them to find the substance capable of reducing Eu'(aq) to Eu²⁺(aq).

Compare standard reduction potentials and determine the substances that can reduce Eu' to Eu²⁺

Let's compare the standard reduction potentials of the given substances with that of Eu²⁺/Eu': 1. Al/Al³⁺: E° = -1.66 V < -0.43 V (Eu²⁺/Eu') 2. Co/Co²⁺: E° = -0.28 V < -0.43 V (Eu²⁺/Eu') 3. H₂O₂/2H₂O: E° = 1.77 V > -0.43 V (Eu²⁺/Eu') 4. N₂H₅⁺/N₂: E° = -0.60 V < -0.43 V (Eu²⁺/Eu') 5. H₂C₂O₄/2CO₂ + 2H₂O: E° = 0.575 V > -0.43 V (Eu²⁺/Eu') From the comparisons above, we can see that only H₂O₂ and H₂C₂O₄ have higher standard reduction potentials than Eu²⁺/Eu', which means they are capable of reducing Eu'(aq) to Eu²⁺(aq) under standard conditions. The substances that can reduce Eu'(aq) to Eu²⁺(aq) under standard conditions are Hydrogen Peroxide (H₂O₂) and Oxalic Acid (H₂C₂O₄).

Key concepts

Electrochemistry

Electrochemistry is a branch of chemistry that deals with the chemical changes caused by the movement of electrons from one substance to another, a field at the heart of batteries, corrosion, and many industrial processes. At its core, it's the study of reduction and oxidation (redox) reactions that involve electron transfer.

In a redox reaction, one substance gains electrons, undergoing reduction, while another loses electrons, which is called oxidation. These reactions are often coupled, as the electrons lost by one substance are gained by another. In the context of the exercise, hydrogens peroxide (H₂O₂) and oxalic acid (H₂C₂O₄) can donate electrons to reduce europium ions (Eu') to europium metal (Eu), showing the practical applications of electrochemistry in determining reactivity and feasibility of such reactions.

Electrochemical cells, including galvanic or voltaic cells, are practical devices that harness these redox reactions to produce electrical energy. Understanding the standard reduction potential of different substances allows for the prediction of the direction of electron flow and the ability of chemicals to act as oxidizing or reducing agents in these cells.

Reduction and Oxidation Reactions

Reduction and oxidation reactions, often referred to as redox reactions, are processes where electrons are transferred between chemical species. The mnemonic 'OIL RIG' - oxidation is loss, reduction is gain - can help students remember the essence of these processes.

In the context of the exercise, we focus on reduction: the gain of electrons. A substance that gains electrons is said to be reduced, and its oxidation state decreases. Conversely, the oxidation state of a substance that loses electrons increases, and the process is known as oxidation. For example, when Europium ion (Eu') is reduced to form Europium metal (Eu²⁺), it gains electrons.

To predict whether a substance will be oxidized or reduced in a reaction, we use standard reduction potentials. These are measured under standard conditions: solute concentrations of 1 M, a pressure of 1 atm for gases, and a temperature of 25°C (298 K). Substances with higher reduction potentials will likely gain electrons and be reduced, whereas those with lower potentials tend to lose electrons and be oxidized.

Standard Electrode Potentials

Standard electrode potentials, also known as standard reduction potentials, are a measure of the tendency of a chemical species to acquire electrons and be reduced, set under standard conditions (1 M concentration, 1 atm pressure, and 298 K temperature). The values are measured against the standard hydrogen electrode, which has a potential of 0 V.

In the exercise, different substances were compared based on their standard reduction potentials to determine if they could reduce Eu'. Substances with a more positive standard reduction potential than Eu²⁺/Eu', like H₂O₂ and H₂C₂O₄, have a greater tendency to gain electrons and can act as reducing agents for Eu'. This comparison is crucial for understanding the flow of electrons in electrochemical cells and for predicting the outcome of redox reactions.

The use of standard reduction potentials simplifies the analysis of electrochemical reactions by providing a comparative scale. However, it's important to remember that actual conditions, such as non-standard concentrations and temperatures, can shift these potentials, affecting the chemical behavior of the species involved.