Equilibrium constant $$ (K_c) $$ for the given cell reaction is $$ 10 $$. calculate $$ E^{\circ}_{cell} $$ . $$ A(s) + B^{2+}(aq) \rightleftharpoons A^{2+} (aq) + B(s) $$
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Q2
The following reaction takes place at 298K in an electrochemical cell involving two metals A and B, A2+(aq)+B(s)→B2+(aq)+A(s) With [A2+]=4×10−3 and [B2+]=2×10−3M in the respective half cells, the cell EMF is 1.091V. The equilibrium constant of the reaction is closest to ________.
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Q3
The following reaction takes place at 298K in an electrochemical cell involving two metals A and B, A2+(aq.)+B(s)→B2+(aq.)+A(s). With [A2+]=4×10−3M and [B2+]=2×10−3M in the respective half-cells, the cell EMF is 1.091V. The equilibrium constant of the reaction is closest to:
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Q4
The efficiency of a cell with cell reaction under standard conditions: A(s)+B2+(aq)⇌A2+(aq)+B(s);ΔH=−285kJ is 85%. The standard electrode potential for the cell is:
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Q5
The efficiency of a cell is 60%. Its cell reaction is: A(s)+B2+(aq)→A2+(aq)+B(s);ΔH=−240kJ The standard electrode potential of cell is