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What does the negative sign in the expre...

What does the negative sign in the expression `E_(Zn^(2+) //Zn)^(@) = -0.76V` mean ?

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Calculate the electrode potential given that E° (Zn^(2+) // Zn) = -0.76V , when a zinc rod is dipped in 0.1 M solution of ZnSO_(4) .The salt is 95% dissociated at this solution at 298K.

The emf of a cell corresponding to the reaction, Zn(s) + 2H^(+) ( aq) rarr Zn^(2+) ( 0.1 M ) + H_(2) ( g , 1 atm) is 0.28 V at 25^(@)C . Write the half-cell reaction and calculate the pH of the solution at the hydrogen electrode. E_(Zn^(2+)//Zn)^(@) = - 0.76V, E_(H^(+) //H_(2))^(@) = 0

Predict whether we can store CuSO_(4) solution in a zinc vessel from the following data. Show your calculation. E_(Zn^(2+)//Zn)^(@) = 0.76V E_(Cu^(2+)//Cu)^(@) = 0.34V

Find the stability constant of the complex [ Zn ( NH_(3))_(4)]^(2+) formed in the reaction, Zn^(2+) + 4NH_(3) hArr [ Zn ( NH_(3))_(4)]^(2+) Given that , E_(Zn^(2+) //Zn)^(@) = - 0.76 V and E_([Zn(NH_(3))_(4)]^(2+)//Zn,4NH_(3))^(@) = - 1.03 V

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What is the role of Zn metal in the extraction of silver ?

In the button cells, widely used in watches and other devices, the following reaction takes place Zn (s) + Ag_(2) O(s) + H_(2) O (l) rarrZn^(2+) (aq) + 2Ag(s) + 2OH^(-) (aq) Determine E^(@) and Delta G^(@) for the reaction. (Given, E_(Ag^(+)//Ag)^(@) = + 0.80 V, E_(Zn^(2+)//Zn)^(@) = -0.76 V )