# Balance the reaction between Ag2O and I^- to form I2 and Ag in basic solution. When you have...

## Question:

Balance the reaction between Ag2O and I{eq}^- {/eq} to form I2 and Ag in basic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown.

_____Ag2O + _____I{eq}^- {/eq} \rightarrow_____I2 + _____Ag

Water appears in the balanced equation as a _____(reactant, product, neither) with a coefficient of . (Enter 0 for neither.)

How many electrons are transferred in this reaction? _____

## Reactivity of Halogens:

Halogens are strong electronegative elements. Hence, they attract electrons quite strongly. Therefore, they are highly oxidizing in nature and acts as an oxidizing agent in most chemical reactions.

The oxidation half-reaction is shown below:

{eq}I^{-}\rightarrow I_{2} {/eq}

Balancing {eq}I {/eq}, we get: {eq}2I^{-}\rightarrow I_{2} {/eq}

Balancing charge, we get: {eq}2I^{-}\rightarrow I_{2}+2e^- {/eq}

So, the balanced oxidation half-reaction is:

{eq}2I^{-}\rightarrow I_{2}+2e^- {/eq} ............... (1)

The reduction half-reaction is shown below:

{eq}Ag_{2}O\rightarrow Ag {/eq}

Balancing {eq}Ag {/eq}, we get: {eq}Ag_{2}O\rightarrow 2Ag {/eq}

Balancing {eq}O {/eq} and {eq}H {/eq} in the basic medium, we get: {eq}Ag_{2}O+H_2O\rightarrow 2Ag+2OH^- {/eq}

Balancing charge, we get: {eq}Ag_{2}O+H_2O+2e^-\rightarrow 2Ag+2OH^- {/eq}

The balanced reduction half-reaction is:

{eq}Ag_{2}O+H_2O+2e^-\rightarrow 2Ag+2OH^- {/eq} ................. (2)

{eq}Equation-(1)+Equation-(2): {/eq}

{eq}Ag_{2}O+2I^{-}+H_2O\rightarrow 2Ag+I_2+2OH^- {/eq}

So, the balanced equation ("1" is explicitly shown) is shown below:

{eq}1Ag_{2}O+2I^{-}+1H_2O\rightarrow 2Ag+1I_2+2OH^- {/eq}

Water appears in the balanced equation as a reactant with a coefficient of 1.

Two electrons are transferred in the given reaction.