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A concentration cell consists of two H2/H+ half-cells. Half-cell A has H2 at 0.…

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Wize University Chemistry Textbook > Electrochemistry

Redox Reactions

4 Activities

Wize University Chemistry Textbook > Electrochemistry

Reduction Potentials

4 Activities

A concentration cell consists of two H2/H+ half-cells. Half-cell A has H2 at 0.90 atm bubbling into 0.10 M HCl. Half-cell B has H2 atm bubbling into 2.0 M HCl. Which half-cell houses the anode? What is the voltage of this cell?
More Redox Reactions Questions:
Electrochemistry: Redox
What is the reducing agent in the following unbalanced chemical reaction?
NO + Au+ → NO3- + Au
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is the reducing agent?
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is the oxidizing agent?
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is being reduced?
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is being oxidized?
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Would you use an oxidizing or reducing agent for the following reaction to occur?
SO42- --> S2-
What product forms at each electrode in the aqueous electrolysis of the following salts? Ignore overpotential effects.
LiF
SnSO4
Redox
C2O42−(aq) + MnO4−(aq) → CO32−(aq) + MnO2(s)
Which one is the reducing agent in this equation?
Similar to Practice Exam 1 Fall 2018 (CHM 2045 UF)
What is the oxidizing agent in the following unbalanced chemical reaction?
NO + Au+ → NO3- + Au
More Reduction Potentials Questions:
Electrochemistry: Galvanic Cells
The cell pictured below is prepared under standard conditions. In this cell, what will be the anode?
𝐶𝑢2+(𝑎𝑞)+𝐻2(𝑔)⇌𝐶𝑢(𝑠)+2𝐻+(𝑎𝑞)𝐸°=0.339𝑉𝐶𝑢^{2+} (𝑎𝑞)+𝐻_2 (𝑔)\rightleftharpoons 𝐶𝑢 (𝑠)+2 𝐻^+ (𝑎𝑞) \qquad𝐸°=0.339 𝑉
Which one of the species above is the best oxidizing agent?
Zn2+(aq)+2e−⇌Zn(s)Eo=−0.74VCu2+(aq)+2e−⇌Cu(s)Eo=+0.34VCo2+(aq)+2e−⇌Co(s)Eo=−0.28VAg+(aq)+e−⇌Ag(s)Eo=+0.80V\def\arraystretch{1.5}\begin{array}{cc}Zn^{2+}(aq)+2e^-⇌Zn(s)&&E^o=-0.74V\\ Cu^{2+}(aq)+2e^-⇌Cu(s)&&E^o=+0.34V\\ Co^{2+}(aq)+2e^-⇌Co(s)&&E^o=-0.28V\\ Ag^+(aq)+e^-⇌Ag(s)&&E^o=+0.80V\end{array}
Which one of the species below is the best reducing agent?
Use the data below to answer the question:
Zn2+(aq)+2e−⇌Zn(s)                         Eo=−0.74VZn^{2+}(aq)+2e^-⇌Zn(s)\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ E^o=-0.74V
Cu2+(aq)+2e−⇌Cu(s)                         Eo=+0.34VCu^{2+}(aq)+2e^-⇌Cu(s)\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ E^o=+0.34V