The positive value of the standard elect...

The positive value of the standard electrode potential of `Cu^(2+)|Cu` indicates that -

this redox couple is a stronger reducing agent than the `H^(+)|H_(2)` couple

this redox couple is stronger oxidising agent than `H^(+)|H_(2)`

`Cu` can displace `H_(2)` from acid

`Cu` cannot displace `H_(2)` from acid

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The correct Answer is:

B, D

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Consider the following four electrodes : P=Cu^(2+)"(0.001 M)|Cu(s) Q=Cu^(2+)("(0.1 M)"|Cu(s) R=Cu^(2+)"(0.01 M)"|Cu(s) S=Cu^(2+)"(0.001)"|Cu(s) If the standard electrode potential of Cu^(2+)|Cu is +0.34V , the reduction potential in volts of the above electrodes follows the order-

`P gt S gt R gt Q`

`S gt R gt O gt P`

`R gt S gt O gt P`

`Q gt R gt S gt P`

hydrogen has a high reducing power

hydrogen is the lightest element

according to convention, its potntilal is taken as zero

this electrode can be easily constructed

`Pt(s)|H_(2)("g, 0.1 bar")|H^(+)(aq, 1M)|Cu^(2+)(aq, 1M)|Cu(s)`

`Pt(s)|H_(2)("g, 1bar")|H^(+)(aq, 1M)|Cu^(2+)("aq, 2M")|Cu(s)`

`Pt(s)|H_(2)("g, 1bar")|H^(+)(aq, 1M)|Cu^(2+)("aq, 1M)|Cu(s)`

`Pt(s)|H_(2)("g, 1bar")|H^(+)(aq, 0.1M)|Cu^(2+)("aq, 1M")|Cu(s)`