For the cell
`Zn(s) + 2H^(+)(aq) rightarow Zn^(2+)(aq) + H_(2)(g)`, `E^(@) = 0.76`V
Which change will increase the voltage of the cell?

The electrochemical cell reaction of the Daniel cell is Zn_((s))+Cu^(2+)""_((aq)) rarr Zn^(2+)""_((aq))+Cu_((s)) What is the change in the cell voltage on increasing the ion concentration in the anode compartment by a factor 10?

For the cell reaction Zn(s) + Cu^(2+)(aq) rarr Cu(s) + Zn^(2+)(aq) E_("cell")^(@) = 1.10 V, DeltaG^(@) is :

For the reaction Fe(s) + Zn^(2+)(aq) rarr Fe^(2+)(aq) + Zn(s), E_(cell)^(@) = -0.32V . What does the negative value of E' cell indicate?

The emf of a cell corresponding to the reaction. Zn(s)+ 2H^(+)(aq)rightarrow Zn^(2+)(0.1M)+H_(2) (g,1atm) is 0.28 V at 25^(@) C . Calculate pH of the solution.

In a cell that utilizes the reactions. Zn(s) + 2H^(+) (aq) rightarrow Zn^(2+)(aq) + H_(2)(g) addition of H_(2)SO_(4) to cathode compartment, will

In a cell that utilizes the reactions. Zn(s) + 2H^(+) (aq) rightarrow Zn^(2+)(aq) + H_(2)(g) addition of H_(2)SO_(4) to cathode compartment, will

Zn(s) | zn^(2+)(aq) || H_(+)(aq)|H_(2)(g) E^9@) = 0.76V What must be the pH in the hydrogen compartment of the cell designated above if the cell voltage is 0.70 V? (Assume that both the [Zn^(2+)] and the H_(2)(g) pressure are at standard values and T= 25^(@)C

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