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Write the cell reaction that occurs when...

Write the cell reaction that occurs when the folowing half cells are combined.
`I_(2)+2e^(-)rarr2I^(-)(1M), E^(@)=+0.54 V`
`Br_(2)+2e^(-)rarrBr^(-)(1M),e^(@)=+1.08 V`

Text Solution

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`(i) Pb_(3)O_(4)` is a stoichiometric mixtrue of two oxides i.e 2 mole of PbO and 1 mole of `PbO_(2)` In phO, the oxidation state of Pb is + 2 while it is +4 in `PbO_(2)`.Both these oxides can react with HCI .Therefore, the reaction may be split in to.
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Write the cell reaction that occurs when the following half-cells are combined. I_(2)+2e^(-)to 2l^(-)(IM) , " "E^(@)=0.54 V Br_(2)+2e^(-)to 2Br^(-)(IM) , " "E^(@)=1.08 V

Which of the following is the cell reaction that occurs when the following half-cells are combined? I_2 + 2e^(-) to 2I^(-) (1M) , E^@=+0.54 V Br_2+2e^(-) to 2Br (1 M) , E^@=+1.09 V

Given that I_(2)+2e^(-)rarr2I^(-): E^(@)=0.54V Br_(2)+2e^(-)rarr2Br^(-):E^(@)=1.09V Predict which of the following is true

The standard reduction potential for half reactions for four different elements. A, B, C and D are: (i) A_(2) + 2e^(-) rarr 2A^(-), E^(@) = + 2.85 V (ii) B_(2) + 2e^(-) rarr 2B^(-), E^(@) = + 1.36 V (iii) C_(2) + 2e^(-) rarr 2C^(-), E^(@) = + 1.06 V (iv) D_(2) + 2e^(-) rarr 2D^(-), E^(@) = + 0.53 V The strongest oxidising reducing agents smong these :

I2 and Br2 are added to a solution containing Br– and I– ions. What reaction will occur if, I_(2) + 2e^(-) rarr 2I^(-) , E^(0) = + 0.54V and Br_(2) + 2e^(-) rarr 2Br^(-) , E^(0) = +1.09 V?