Diagram the following galvanic cell, indicating the directionof flow of electron

Question

Diagram the following galvanic cell, indicating the directionof flow of electrons in the external circuit and the motion of ionsin the salt bridge. Ni(s) l Ni2+ (aq) ll HCl(aq) l H2(g) lPt(s)           l = metal solution ll = salt bridge So Ni(s) is an anode, oxidizing element, whic give upelectrons. I could write an half-reaction equation for Ni. Ni(s) Ni2+ 2e- However, what am I supposed to do with HCl andH2? How am I supposed to deal with Cl? Can I just ignore it? Does H2 have no net charge because there is nowupper letter like Ni2? Diagram the following galvanic cell, indicating the directionof flow of electrons in the external circuit and the motion of ionsin the salt bridge. Ni(s) l Ni2+ (aq) ll HCl(aq) l H2(g) lPt(s)           l = metal solution ll = salt bridge So Ni(s) is an anode, oxidizing element, whic give upelectrons. I could write an half-reaction equation for Ni. Ni(s) Ni2+ 2e- However, what am I supposed to do with HCl andH2? How am I supposed to deal with Cl? Can I just ignore it? Does H2 have no net charge because there is nowupper letter like Ni2?

Explanation / Answer

We Know that :       For the given cellreaction          Ni(s) lNi2+ (aq) ll HCl(aq) l H2(g) lPt(s)          Anode half reaction:           Ni (s)------> Ni+2 (aq.) + 2e         cathode halfreaction :          2H+ (aq.) + 2e -------> H2 (Pt)           For the given compound HCl the Cl- ions arepresent in the solution which is neutralized by the agar-agarsolution            used in the salt bridge.

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