The reaction, 1/2H_2(g)+AgCl(s)⇌H^+...
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The reaction, ( frac{1}{2} mathrm{H}_{2}(g)+operatorname{AgCl}(s) rightleftharpoons mathrm{H}^{+}(a q)+mathrm{Cl}^{-}(a q)+mathrm{Ag}(s) ) occurs in the galvanic cell
(a) ( mathrm{Ag}|mathrm{AgCl}(s)| mathrm{KCl}(mathrm{soln})left|mathrm{AgNO}_{3}right| mathrm{Ag} )
(b) ( mathrm{Pt}left|mathrm{H}_{2}(g)right| mathrm{HCl}(mathrm{soln})left|mathrm{AgNO}_{3}(mathrm{soln})right| mathrm{Ag} )
(c) ( mathrm{Pt}left|mathrm{H}_{2}(g) mathrm{HCl}(mathrm{soln})right| mathrm{AgCl}(s) mid mathrm{Ag} )
(d) ( mathrm{Pt}left|mathrm{H}_{2}(g)right| mathrm{KCl}(mathrm{soln})|mathrm{AgCl}(s)| mathrm{Ag} )

SSC CGL
Chemistry
Solution
107
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The reaction, 1/2H_2(g)+AgCl(s)⇌H^+(aq)+Cl^−(aq)+Ag(s) occurs in the galvanic cell
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In a galvanic cell, oxidation occur in the left hand electrode chamber and reduction in right hand electrode chamber. In the following cell.
[
mathrm{Pt}left|mathrm{H}_{2}(g)right| mathrm{HCl}(mathrm{soln}) | mathrm{AgCl}(s) mid mathrm{Ag}(s)
]
The cell reactions are :
[
begin{array}{c}
frac{1}{2} mathrm{H}_{2}(g) longrightarrow mathrm{H}^{+}+e^{-} quad text { At anode }
mathrm{AgCl}(s)+e^{-} longrightarrow mathrm{Ag}+mathrm{Cl}^{-} quad text { At cathode }
text { Net: } frac{1}{2} mathrm{H}_{2}(g)+mathrm{AgCl}(s) longrightarrow mathrm{H}^{+}+mathrm{Ag}(s)+mathrm{Cl}^{-}
end{array}
]

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