Cell voltages and half-cell potentials a...

Cell voltages and half-cell potentials are often compeared under standard conditions called the standard state at a specified temperature (298K). The standard state requires all reagents to be pure with all gases at unit fugacity, all ions at unit activity and all electrical connections between half-cells to be made with platinum. Suppose following are half cell reaction, with respective emf (s) are -0.25 V and -0.3V.
Cell reaction I `underset("1 atm")(Pt(H_(2))|HCl)`
Cell reaction II `underset("1 atm")(Pt(H_(2))|H_(2)SO_(4))`
pH value of cell reaction I is

4.23

5.23

5.08

5.32

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Cell voltages and half-cell potentials are often compeared under standard conditions called the standard state at a specified temperature (298K). The standard state requires all reagents to be pure with all gases at unit fugacity, all ions at unit activity and all electrical connections between half-cells to be made with platinum. Suppose following are half cell reaction, with respective emf (s) are -0.25 V and -0.3V. Cell reaction I underset("1 atm")(Pt(H_(2))|HCl) Cell reaction II underset("1 atm")(Pt(H_(2))|H_(2)SO_(4)) Zinc gives H_2 with H_2SO_4 and HCI but not with HNO3 because:

zinc acts as oxidizing agent when reacts with `HNO_3`

`HNO_3` is a weaker acid than `H_2SO_4 and HCI`

in electrochemical series zinc is above than hydrogen

`NO_(3)^(-)` is reduced in preference to hydronium ion

I and II

I and III

I and IV

II and IV

`-0.3125 V`

`0.3125 V`

`1.114 V`

`-1.114V`