For the following cell `Zn(s)|ZnSO_4 (aq) ||CuSO_4 (aq)|Cu(s)` When `[Zn^(2+)]` is ten times of `[Cu^(2+)]` the expression `Delta G ` ( in `J mol^-1`) is
A
2.303 RT +1.1F
B
1.1F
C
2.303RT -2.2F
D
2.2F
Text Solution
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C `Delta G=Delta G^@+2.303RT log""([Zn^(2+)])/([Cu^(2+)])` and `Delta G^@=-nFE^@=2 times 1.1F` find `Delta G (E_(cell)^@=1.1V)]`
For the following cell, Zn(s)|ZnSO_(4)(aq)||CuSO_(4)(aq)||Cu(s) When the concentration of Zn^(2+) is 10 times the concentration of Cu^(2+) , the expression for DeltaG (in J "mol"^(-1) ) [F is Faraday constant, R is gas constant] T is temperaure, E^(@)("cell")=1.1V
For the following cell , Zn_(s)|ZnSO_(4)((aq)) CuSO_(4)((aq)) |Cu(s) When the concentration of Zn^(2+) is 10 times the concentration of Cu^(2+) , the expression for DeltaG ("in " J mol^(-1) is [F is Faraday constant , R is gas constant , T is temperature , E_(cell)^(@) = 1.1V ]
Zn(s)+CuSO_4(aq) to ZnSO_4(aq) + Cu(s) The above equation is an example of:
Consider the Galvanic cell Zn^- |ZnSO_4 ||CuSO_4 +Cu^(o+) the reaction at cathode is .
Does the following reaction occur ? Cu + ZnSO_(4) to CuSO_(4) + Zn
Complete the following equation: Zn + CuSO_4 to ………. + Cu
