Answer
Verified
401.1k+ views
Hint: Analyze what is happening in the problem carefully, we have to find the single electrode potential of the oxidation half of the reaction. We can use a derivative of the Nernst equations and arrive at the answer.
Complete step by step solution:
Zinc is considered to be a good reducing agent due to the fact that it is a metal. Metals tend to lose electrons to another species and reduce it. In this process, metals themselves get oxidized. Hence, as zinc here is going from $Zn$ to $Z{{n}^{2+}}$, it is getting oxidized. Therefore, we will use the ${{E}_{oxi}}$ form of the Nernst equation.
The Nernst equation is used to find out the cell potential under non-standard conditions if the potential under standard conditions is given.
The Nernst equation is as follows:
\[{{E}_{oxi}}={{E}^{0}}_{oxi}-\dfrac{0.0592}{n}{{\log }_{10}}[ion]\]
Where,
${{E}_{oxi}}$= electrode potential
${{E}^{0}}_{oxi}$= standard electrode potential
$n$= number of moles of electrons exchanged
[ion] = concentration of ions
Here, the ${{E}^{0}}_{oxi}$ is the standard electrode potential, it is obtained when the concentration of all the species involved in the half-cell is 1M, at a certain temperature. If the concentration is anything other than 1M, we have to find out the electrode potential (${{E}_{oxi}}$) using the standard electrode potential.
Thus, from the given information, we know that
${{E}^{0}}_{oxi}$= 0.763 $V$
$n$= 2 (from ${Zn}/{Z{{n}^{2+}}}\;$)
[ion] = 0.01$M$
Therefore, plugging in all the values in the equation, we get:
\[{{E}_{oxi}}=0.763-\dfrac{0.0592}{2}{{\log }_{10}}(0.01)\]
${{E}_{oxi}}=0.763-[(\dfrac{0.0592}{2})\times (-2)]$
${{E}_{oxi}}=0.763+0.0592$
${{E}_{oxi}}=0.8222$
Hence, the answer for this equation is ${{E}_{oxi}}=0.8222$
Additional information:
The Nernst equation has many forms and any one of them can be used as per the requirements of the sums. If the reaction is a reduction half reaction and the standard electrode(reduction) potential is given, then it can be converted to the standard oxidation potential and used in the same formula.
Note: Always check whether the reaction is an oxidation half reaction or a reduction half reaction before applying any formulae. This may cause confusion regarding which sign should be applied. An easy way to remember this is OIL RIG whose full form is ‘Oxidation Is Losing (electrons), Reduction Is Gaining (electrons)’. Here the electrode potential is given as ${Zn}/{Z{{n}^{2+}}}\;$ where zinc is losing electrons.
Hence, it is an oxidation half reaction.
Complete step by step solution:
Zinc is considered to be a good reducing agent due to the fact that it is a metal. Metals tend to lose electrons to another species and reduce it. In this process, metals themselves get oxidized. Hence, as zinc here is going from $Zn$ to $Z{{n}^{2+}}$, it is getting oxidized. Therefore, we will use the ${{E}_{oxi}}$ form of the Nernst equation.
The Nernst equation is used to find out the cell potential under non-standard conditions if the potential under standard conditions is given.
The Nernst equation is as follows:
\[{{E}_{oxi}}={{E}^{0}}_{oxi}-\dfrac{0.0592}{n}{{\log }_{10}}[ion]\]
Where,
${{E}_{oxi}}$= electrode potential
${{E}^{0}}_{oxi}$= standard electrode potential
$n$= number of moles of electrons exchanged
[ion] = concentration of ions
Here, the ${{E}^{0}}_{oxi}$ is the standard electrode potential, it is obtained when the concentration of all the species involved in the half-cell is 1M, at a certain temperature. If the concentration is anything other than 1M, we have to find out the electrode potential (${{E}_{oxi}}$) using the standard electrode potential.
Thus, from the given information, we know that
${{E}^{0}}_{oxi}$= 0.763 $V$
$n$= 2 (from ${Zn}/{Z{{n}^{2+}}}\;$)
[ion] = 0.01$M$
Therefore, plugging in all the values in the equation, we get:
\[{{E}_{oxi}}=0.763-\dfrac{0.0592}{2}{{\log }_{10}}(0.01)\]
${{E}_{oxi}}=0.763-[(\dfrac{0.0592}{2})\times (-2)]$
${{E}_{oxi}}=0.763+0.0592$
${{E}_{oxi}}=0.8222$
Hence, the answer for this equation is ${{E}_{oxi}}=0.8222$
Additional information:
The Nernst equation has many forms and any one of them can be used as per the requirements of the sums. If the reaction is a reduction half reaction and the standard electrode(reduction) potential is given, then it can be converted to the standard oxidation potential and used in the same formula.
Note: Always check whether the reaction is an oxidation half reaction or a reduction half reaction before applying any formulae. This may cause confusion regarding which sign should be applied. An easy way to remember this is OIL RIG whose full form is ‘Oxidation Is Losing (electrons), Reduction Is Gaining (electrons)’. Here the electrode potential is given as ${Zn}/{Z{{n}^{2+}}}\;$ where zinc is losing electrons.
Hence, it is an oxidation half reaction.
Recently Updated Pages
Basicity of sulphurous acid and sulphuric acid are
Three beakers labelled as A B and C each containing 25 mL of water were taken A small amount of NaOH anhydrous CuSO4 and NaCl were added to the beakers A B and C respectively It was observed that there was an increase in the temperature of the solutions contained in beakers A and B whereas in case of beaker C the temperature of the solution falls Which one of the following statements isarecorrect i In beakers A and B exothermic process has occurred ii In beakers A and B endothermic process has occurred iii In beaker C exothermic process has occurred iv In beaker C endothermic process has occurred
What is the stopping potential when the metal with class 12 physics JEE_Main
The momentum of a photon is 2 times 10 16gm cmsec Its class 12 physics JEE_Main
How do you arrange NH4 + BF3 H2O C2H2 in increasing class 11 chemistry CBSE
Is H mCT and q mCT the same thing If so which is more class 11 chemistry CBSE
Trending doubts
Difference Between Plant Cell and Animal Cell
Difference between Prokaryotic cell and Eukaryotic class 11 biology CBSE
Fill the blanks with the suitable prepositions 1 The class 9 english CBSE
Change the following sentences into negative and interrogative class 10 english CBSE
Summary of the poem Where the Mind is Without Fear class 8 english CBSE
Give 10 examples for herbs , shrubs , climbers , creepers
Write an application to the principal requesting five class 10 english CBSE
What organs are located on the left side of your body class 11 biology CBSE
What is the z value for a 90 95 and 99 percent confidence class 11 maths CBSE