357/303 Energizer 17.50 The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Calculate the free-energy change (in kilo- joules) for the cell reaction Zn(s) + Ag20(s) → ZnO(s) + 2 Ag(s) MADE Energizer 357/303 357 SILVER OXIDE/ OXYDE D'ARGENT 1.55 V BATTERIES/PILES
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Can you please solve question 17.50 and show all of the steps to the solution
![**Electrochemistry Problems**
**17.49**
How are standard reduction potentials defined?
The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Calculate the free-energy change (in kilojoules) for the cell reaction:
\[ \text{Zn(s)} + \text{Ag}_2\text{O(s)} \rightarrow \text{ZnO(s)} + 2 \text{Ag(s)} \]
**17.51**
The standard cell potential for a lead storage battery is 1.924 V. Calculate \(\Delta G^\circ\) (in kilojoules) for the cell reaction:
\[ \text{Pb(s)} + \text{PbO}_2\text{(s)} + 2 \text{H}^+\text{(aq)} + 2 \text{HSO}_4^-\text{(aq)} \rightarrow 2 \text{PbSO}_4\text{(s)} + 2 \text{H}_2\text{O(l)} \]
**17.52**
What is the value of \(x\) if \(A^{2+} + B^- \rightarrow A^{++} + B\) \(E^\circ = 1.43 \text{ V and } \Delta G^\circ = -41 \text{ kJ}\)?
The image also features an illustration showing cylindrical batteries labeled "Energizer 357" with specifications that highlight their use in small electronic devices such as watches.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e830786-058e-49dd-8798-047547f22476%2F0b043b17-ff76-4b7e-865e-f68529a8c76d%2Fzb9xqqp.jpeg&w=3840&q=75)
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