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Question
Represent the cell in which the following reaction takes place $$Mg(S)+2$$Ag^+ (0.0001 M) \rightarrow MG^{2+}(0.130 M)+2Ag(s)$$ Calculate its $$E_{(cell)} \quad if $$E_{(cell)} if E_{(cell)}=3.17 V.$$
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Q1
Represent the cell in which the following reaction takes place.
Mg(s)+2Ag+(0.0001m) →Mg2+(0.130M)+2Ag(s)
Calculate its E(cell if)
EΘ(cell)=3.17V.
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Q2
Represent the cell in which the following reaction takes place Mg(s)+2Ag+(0.0001M)→Mg2+(0.130M)+2Ag(s) Calculate its E(cell)ifEo(cell)=3.17V
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Q3
In following cell reaction $$Mg(s)+2Ag^+(0.001M)\rightarrow Mg^{2+}(0.20M)+2Ag(s)$$ Calculate $$E_{cell}$$ for the reaction $$[E^o=3.17V, \dfrac{2.30 RT}{F}=0.054]$$.
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Q4
Represent the cell in which the following reaction takes place Mg(s)+2Ag+(0.0001M)→Mg2+(0.130M)+2Ag(s)
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Q5
For the cell reaction, Mg(s)+2Ag+(aq.)⇌Mg2+(aq.)+2Ag(s) E∘cell is +3.17V at 298K. The value of Ecell,△G∘ and Q at Ag+ and Mg2+ concentrations of 0.001M and 0.02M respectively are: