Out of aluminium and silver vessel which one will be more suitable to store 1(M) HCl solution .
`(E^0)_((Al^(+3))/(Al) =-1.66v)`, ` (E^0)_((Ag^+)/(Ag))=0.80V`

A solution of AgNO_3 was stirred with iron rod. Will it cause any change in the concentration of silver and nitrate ions? ( (E^0)_((Fe^(2+))/(Fe)=-0.44V) , ((E^0)_((Ag^+)/(Ag))=0.80V)

Explain Can Cl_2 be stored in copper cylinder ? (E^0)_((Cu^(2+))/(Cu)=0.34V , (E^0)_(Cl^-)/(Cl)=0.36V

Can Fe^(2+) be produced in the reaction of Fe with 1(M) HCl solution? Explain. Given : E_(Fe^(2+)|Fe)^(@)=-0.44V

Which among the following vessels is used to store CuSO_(4) solution ? a Ag vessel [ Given E_(Zn^(2+)|Zn)^(0)=-0.76V, E_(Cu^(2+)|Cu)^(0)=+0.34V and E_(Ag^(+)|Ag)^(0)=0.80V ]

Which among the following vessels is used to store CuSO_(4) solution ? a Zn vessel [ Given E_(Zn^(2+)|Zn)^(@)=-0.76V, E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Ag^(+)|Ag)^(0)=0.80V ]

If Fe is allowed to react with 1(M) HCl solution, will Fe be oxidised to Fe^(2+)? E_(Fe^(+2)|Fe)^(@)=-0.44V

A cell is prepared by dipping a copper rod in 1 M CusO_4 and nickel rod in 1 M NiSO_4 solution. (E^0)_((Cu^(+2))/Cu=0.34V , (E^0)_((Cl^-)/(Cl))=0.36V Give cell construction.

Of the elements Zn , Mg Cu and Ag , which are able to produce H_(2) gas when they are treated with dilute HCl solutions ? [ Given E_(Zn^(2+)|Zn)^(@)= -0.76 V , E_(Mg^(2+)|Mg)^(@) = - 1.20 V, E_(Cu^(2)+|Cu)^(@)+0.34 V and E_(Ag^(+)|Ag)^(@) = + 0.80 V ]

An aqueous solution containing Cu^(2+), Hg_(2)^(2+) and Ag^(+) ions, each with a concentration of 1M, is being electrolysed by using Pt - electrodes. If the voltage between the electrodes is increased gradually, which one of these ions will be deposited first and which one will be deposited last at the cathode? E_(Ag^(+)|Ag)^(@)=0.8V, E_(Cu^(+)|Cu)^(@)=0.34V & E_(Hg^(+)|2Hg)^(@)=0.79

Will Cu dissolve as Cu^(2+) in 1 (M) HCl solution? Will it do so in 1 (M) HNO_(3) solution? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34 and E_(NO_(3)^(-)|NO)^(@)=+0.96]