Calculate the equilibrium constant for the reaction `Cu(s)+2Ag^(+)(aq)rarrCu^(2+)(aq)+2Ag(s), E_(cell)^(@)=0.46 V`.A. `4.0 xx 10^(10)`B. `4.0 xx 10^(15)`C. `2.4 xx 10^(10)`D. `2.0 xx 10^(10)`

Calculate the equilibrium constant for the reaction `Cu(s)+2Ag^(+)(aq)

1.	Calculate the equilibrium constant for the reaction `Cu(s)+2Ag^(+)(aq)rarrCu^(2+)(aq)+2Ag(s), E_(cell)^(@)=0.46 V`.A. `4.0 xx 10^(10)`B. `4.0 xx 10^(15)`C. `2.4 xx 10^(10)`D. `2.0 xx 10^(10)`
Answer» Correct Answer - B According to Nernst equation `E_("cell")^(@) = (2.303 RT)/(nF) log K_(eq.)` or `log K_(eq.) = (nFE_("cell")^(@))/(2.303 RT)` `= ((2 mol)(96500 C mol^(-1))(0.46 V))/((2.303)(8.314 JK^(-1))(298 K))` `= 15.56` Thus `K_(eq.) = 4.0 xx 10^(15)`

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Calculate the equilibrium constant for the reaction `Cu(s)+2Ag^(+)(aq)rarrCu^(2+)(aq)+2Ag(s), E_(cell)^(@)=0.46 V`.A. `4.0 xx 10^(10)`B. `4.0 xx 10^(15)`C. `2.4 xx 10^(10)`D. `2.0 xx 10^(10)`

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