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Explain the following : Zinc displaces h...

Explain the following : Zinc displaces hydrogen from acid solution.
`E_(Zn^(2+)//Zn)^(Theta)= -0.76V`

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Calculate the e.m.f. of a cell in which the following reactions take place at different electrodes. Zn^(2+) +2e^(-) to Zn, E^(Theta)= -0.76V " "...(i) Ag^(+)+e^(-) to Ag, E^(Theta)=0.79V" "...(ii)

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

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknown concentration . Its other half-cell consists of a zinc electrode dipping in 1.0 M solution of Zn(NO_(3))_(2) . A voltage of 1.48 V is measured for this cell . Use this information to calculate the concentration of silver nitrate solution used. (E_(Zn^(2+)|Zn)^(@) = -0.76V , E_(Ag^(+)|Ag)^(@) = + 0.80V ).

What does the standard electrode potential of a metal being negative (E_(Zn^(2+)//Zn)^(Theta)= -0.7632) indicate ?

Statement-1: Zinc displaces copper from copper sulphate solution. Statement-2: The E_(298)^(@) of Zn is -0.76 volts and that of Cu is +0.34 volts.

If [Zn^(2+)] is maintained at 1.0 M (i) What is the minimum (Cu^(2+)) for which the reaction Zn_((s))+Cu_((aq))^(2+) to Cu_((s))+Zn_((aq))^(2+) is still spontaneous in forward direction. (ii) Does the displacement of Cu_((aq))^(2+)" by "Zn_((s)) go to completion? E_(Zn^(2+)//Zn)^(0)=-0.76V E_(Cu^(2+)//Cu)=0.34V

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