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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

A

4.23

B

5.23

C

5.08

D

5.32

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Knowledge Check

  • 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:

    A
    zinc acts as oxidizing agent when reacts with `HNO_3`
    B
    `HNO_3` is a weaker acid than `H_2SO_4 and HCI`
    C
    in electrochemical series zinc is above than hydrogen
    D
    `NO_(3)^(-)` is reduced in preference to hydronium ion

  • Consider the following half-cell reactions. What combination of two half-cells would result in a cell with the largest potential?

    A
    I and II
    B
    I and III
    C
    I and IV
    D
    II and IV

  • The two half cell reactions of an electrochemical cell is given as the value of cell EMF will be

    A
    `-0.3125 V`
    B
    `0.3125 V`
    C
    `1.114 V`
    D
    `-1.114V`