Given the following notation for an electrochemical cell,
Pt(s) $|$ H$_2$(g)$|$ H$^+$(aq) $//$ Ag$^+$(aq)$|$Ag(s)
Which of the following represents the overall balanced (net) cell reaction?
Pt(s) $|$ H$_2$(g)$|$ H$^+$(aq) $//$ Ag$^+$(aq)$|$Ag(s)
Which of the following represents the overall balanced (net) cell reaction?
Show Hint
- H$_2$(g) + Ag$^+$(aq) → 2H$^+$(aq) + Ag(s)
- H$_2$(g) + Ag(s) → H$^+$(aq) + Ag$^+$(aq)
- Ag(s) + H$^+$(aq) → Ag$^+$(aq) + H$_2$(g)
- None of the above
The Correct Option is D
Solution and Explanation
Correct cell reaction: H$_2$(g) → 2H$^+$(aq) + 2e$^-$ (oxidation at anode);
Ag$^+$(aq) + e$^-$ → Ag(s) (reduction at cathode)
Net reaction: \[ H_2(g) + 2Ag^+(aq) \rightarrow 2H^+(aq) + 2Ag(s) \] None of the given options match this.
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