The overall reaction and standard cell potential at 25oC for the rechargeable nickel–cadmium alkaline battery is Cd(s) + NiO2(s) + 2H2O(l) → Ni(OH)2(s) + Cd(OH)2(s) ϐo = 1.10 V For every mole of Cd consumed in the cell, what is the maximum useful work that can be obtained at standard conditions?
Answer to relevant QuestionsNot all spontaneous redox reactions produce wonderful results. Corrosion is an example of a spontaneous redox process that has negative effects. What happens in the corrosion of a metal such as iron? What must be present for ...A standard galvanic cell is constructed so that the overall cell reaction is 2Al3+(aq) + 3M(s) → 3M2+(aq) + 2Al(s) where M is an unknown metal. If ΔGo = –411 kJ for the overall cell reaction, identify the metal used ...A zinc–copper battery is constructed as follows: Zn | Zn2+(0.10 M) | | Cu2+(2.50 M) | Cu The mass of each electrode is 200 g. a. Calculate the cell potential when this battery is first connected. Consider the following galvanic cell: This Internet exercise requires students to visit the Web site for the company that originated the economic-value-added measure and learn about the uses of the measure.
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