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Consider the reaction 2 Ag^+("(aq)") ...

Consider the reaction ` 2 Ag^+_("(aq)") + Cd_("(s)") to 2 Ag ("(s)") + Cd ^( +2 ) _ ("(aq)") `. The standard electrode potential for ` Ag ^+|Ag and Cd ^ ( + 2 ) | Cd ` coples are + 0.80 volt and -0.40 volt respectively. The standard cell potential for this reaction will be

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Consider the reaction, 2Ag^(+)+Cd rarr 2Ag+Cd^(2+) The standard electrode potentials for Ag^(+) rarr Ag and Cd^(2+) rarr Cd couples are 0.80 volt and -0.40 volt respectively. (i) What is the standard potential E^(@) for this reaction ? (ii) For the electrochemical cell, in which this reaction takes place which electrode is negative electrode ?

Consider the reaction, 2Ag^(+)+Cd rarr 2Ag+Cd^(2+) The standard electrode potentials for Ag^(+) rarr Ag and Cd^(2+) rarr Cd couples are 0.80 volt and -0.40 volt respectively. (i) What is the standard potential E^(@) for this reaction ? (ii) For the electrochemical cell, in which this reaction takes place which electrode is negative electrode ?

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Consider the reaction 2Ag^(+) + Cd to 2Ag + Cd^(2+) . The standard reduction potentials of Ag^(+)//Ag and Cd^(2+)//Cd are + 0*80 " volt and " 0*40 volt, respectively. Give the cell representation.

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Consider the reaction 2Ag^(+) + Cd to 2Ag + Cd^(2+) . The standard reduction potentials of Ag^(+)//Ag and Cd^(2+)//Cd are + 0*80 " volt and " 0*40 volt, respectively. What will be the emf of the cell if concentration of Cd^(2+) is 0*1 M and Ag^(+) is 0*2 M ?

Consider the reaction 2Ag^(+) +Cd to 2Ag to 2Ag +Cd^(2+) . The standard reduction potentials of Ag^(+)//Ag and Cd^(2+)//Cd are + 0.80 volt and - 0.40, respectively. (i) Give the cell representation. (ii) What is the standard cell emf. E^(Theta) ? (iii) What will the emf of the cell if concentration of Cd^(2+) is 0.1 M and Ag^(+) is 0.2 M? (iv) Will the cell work spontaneously for the condition given in (ii) above ?

Consider the following cell reaction at 298 K : 2Ag^(+)+Cdrarr2Ag+Cd^(2+) The standard reduction potentials (E^(@)) for Ag^(+)//Ag and Cd^(2+)//Cd are 0.80 V and -0.40V respectively : (1) Write the cell representation. (2) What will be the emf of the cell if the concentration of Cd^(2+) is 0.1 M and that of Ag^(+) is 0.2 M? (3) Will the cell work spontaneously for the condition given in (2) above?

The standard electrode potentials for the reactions, Ag^(+) (a.q) + e^(-) rarr Ag (s) Sn^(2+) (a.q) + 2e^(-) rarr Sn (s) at 25^(@)C are 0.80 volt and -0.14 volt respectively. The emf of the cell Sn|Sn^(2+) (1M)|| Ag^(+) (1M) | Ag is: