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Stoichiometry correction, redaction
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edit approved Feb 26, 2016 at 10:58
Orr22
edit approved Feb 26, 2016 at 10:58
Orr22
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I am confused as to why galvanic cells have electrolytes. For example, a zinc-hydrogen galvanic cell has a zinc sulfate anode electrolyte and hydrochloric acid cathode electrolyte. The overall reaction of this cell is notmay be written as:

$$ \ce{ZnSO4 + HCl -> ZnCl2 + H2SO4} $$$$ \ce{ZnSO4 + 2HCl -> ZnCl2 + H2SO4} $$

RatherBut rather, it is written as:

$$ \ce{Zn(s) + 2H+(aq) -> Zn^2+(aq) + H2(g)} $$

Why is this the overall reaction? What is then the purpose of an electrolyte, if only the anodes and cathodes are written in the overall equation?

I am confused as to why galvanic cells have electrolytes. For example, a zinc-hydrogen galvanic cell has a zinc sulfate anode electrolyte and hydrochloric acid cathode electrolyte. The overall reaction of this cell is not written as:

$$ \ce{ZnSO4 + HCl -> ZnCl2 + H2SO4} $$

Rather, it is written as:

$$ \ce{Zn(s) + 2H+(aq) -> Zn^2+(aq) + H2(g)} $$

Why is this the overall reaction? What is then the purpose of an electrolyte, if only the anodes and cathodes are written in the overall equation?

I am confused as to why galvanic cells have electrolytes. For example, a zinc-hydrogen galvanic cell has a zinc sulfate anode electrolyte and hydrochloric acid cathode electrolyte. The overall reaction of this may be written as:

$$ \ce{ZnSO4 + 2HCl -> ZnCl2 + H2SO4} $$

But rather, it is written as:

$$ \ce{Zn(s) + 2H+(aq) -> Zn^2+(aq) + H2(g)} $$

Why is this the overall reaction? What is then the purpose of an electrolyte, if only the anodes and cathodes are written in the overall equation?

Improved formatting using \ce{}; Put formula in separate lines; Fixed grammar
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edit approved Feb 24, 2016 at 8:48
lcnittl
edit approved Feb 24, 2016 at 8:48
lcnittl
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I am confused as to why galvanic cells have electrolytes. For example, a zinc-hydrogen galvanic cell has a zinc sulfate anode electrolyte and hydrochloric acid cathode electrolyte. The overall reaction of this cell is not written as ZnSO4 + HCl --> ZnCl2 + H2SO4.:

$$ \ce{ZnSO4 + HCl -> ZnCl2 + H2SO4} $$

Rather, it is written as Zn(s) + 2H+ (aq) --> Zn2+(aq) + H2(g).:

$$ \ce{Zn(s) + 2H+(aq) -> Zn^2+(aq) + H2(g)} $$

Why is this the overall reaction? What is then the purpose of an electrolyte, if only the anodes and cathodes are written in the overall equation?

I am confused as to why galvanic cells have electrolytes. For example, a zinc-hydrogen galvanic cell has a zinc sulfate anode electrolyte and hydrochloric acid cathode electrolyte. The overall reaction of this cell is not written as ZnSO4 + HCl --> ZnCl2 + H2SO4. Rather, it is written as Zn(s) + 2H+ (aq) --> Zn2+(aq) + H2(g). Why is this the overall reaction? What is then the purpose of an electrolyte if only the anodes and cathodes are written in the overall equation?

I am confused as to why galvanic cells have electrolytes. For example, a zinc-hydrogen galvanic cell has a zinc sulfate anode electrolyte and hydrochloric acid cathode electrolyte. The overall reaction of this cell is not written as:

$$ \ce{ZnSO4 + HCl -> ZnCl2 + H2SO4} $$

Rather, it is written as:

$$ \ce{Zn(s) + 2H+(aq) -> Zn^2+(aq) + H2(g)} $$

Why is this the overall reaction? What is then the purpose of an electrolyte, if only the anodes and cathodes are written in the overall equation?

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user510
user510
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Purpose of electrolyte in a galvanic cell

I am confused as to why galvanic cells have electrolytes. For example, a zinc-hydrogen galvanic cell has a zinc sulfate anode electrolyte and hydrochloric acid cathode electrolyte. The overall reaction of this cell is not written as ZnSO4 + HCl --> ZnCl2 + H2SO4. Rather, it is written as Zn(s) + 2H+ (aq) --> Zn2+(aq) + H2(g). Why is this the overall reaction? What is then the purpose of an electrolyte if only the anodes and cathodes are written in the overall equation?