Question
What is the standard electrode potential? Explain it details.
✓
Answer
$\rightarrow$ "Reduction potential of electrode at standard condition at $298 \ K$ temperature and $1$ bar pressure is known as standard electrode potential."
$\rightarrow$ The standard electrode potentials are very important and we can extract a lot of useful information from them.
$\rightarrow$ If the standard electrode potential of an electrode is greater than zero then its reduced from is more stable compared to hydrogen gas If the standard electrode potential is negative then hydrogen gas is more stable than the reduced form of the species.
$\rightarrow$ It can be seen that the standard electrode potential for fluorine is the highest in the table indication that fluorine gas $(F_2)$ has the maximum tendency to get reduced to fluoride ions $(F^-)$
$\rightarrow$ Therefore, fluorine gas is the strongest oxidising agent and fluoride ion is the weakest reducing agent
$\rightarrow$ Lithium has the lowest electrode potentia indicating that lithium ion is the weakes oxidising agent while lithium metal is the mos powerful reducing agent in an aqueous solution
$\rightarrow$ It may be seen that as we go form top to bottom in Table the standard electrode potentia decreases. With this decrease, the oxidizing power of the species on the left diminishes and the reducing power of the species on the right hand side of the reaction increases.
$1.$ A negative $E ^{\ominus}$ means that the redox couple is a stronger reducing agent than the $H ^{+} / H _2$ couple
$2.$ A positive $E ^{\ominus}$ means that the redox couple is a weaker reducing agent than the $H ^{+} / H _2$ couple.
$\rightarrow$ The standard electrode potentials are very important and we can extract a lot of useful information from them.
$\rightarrow$ If the standard electrode potential of an electrode is greater than zero then its reduced from is more stable compared to hydrogen gas If the standard electrode potential is negative then hydrogen gas is more stable than the reduced form of the species.
$\rightarrow$ It can be seen that the standard electrode potential for fluorine is the highest in the table indication that fluorine gas $(F_2)$ has the maximum tendency to get reduced to fluoride ions $(F^-)$
$\rightarrow$ Therefore, fluorine gas is the strongest oxidising agent and fluoride ion is the weakest reducing agent
$\rightarrow$ Lithium has the lowest electrode potentia indicating that lithium ion is the weakes oxidising agent while lithium metal is the mos powerful reducing agent in an aqueous solution
$\rightarrow$ It may be seen that as we go form top to bottom in Table the standard electrode potentia decreases. With this decrease, the oxidizing power of the species on the left diminishes and the reducing power of the species on the right hand side of the reaction increases.
$1.$ A negative $E ^{\ominus}$ means that the redox couple is a stronger reducing agent than the $H ^{+} / H _2$ couple
$2.$ A positive $E ^{\ominus}$ means that the redox couple is a weaker reducing agent than the $H ^{+} / H _2$ couple.
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