Balance the following equation:

$I_2+Cl_2+H_2 O \rightarrow HIO_3+HCl$

Question

auntnonee auntnonee

04-11-2026
Chemistry

Answered

Balance the following equation:

$I_2+Cl_2+H_2 O \rightarrow HIO_3+HCl$

Verified Answer :

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GinnyAnswer GinnyAnswer · Answer 1 · 2026-11-04T11:26:23-05:00

Identify the change in oxidation states for Iodine ($0$ to $+5$) and Chlorine ($0$ to $-1$).
Use the half-reaction method to balance the electron transfer: $1$ molecule of $I_2$ requires $5$ molecules of $Cl_2$.
Balance the remaining oxygen and hydrogen atoms by adding $6H_2O$ to the reactant side.
The final balanced equation is $\boxed{I_2 + 5Cl_2 + 6H_2O \rightarrow 2HIO_3 + 10HCl}$.

Explanation

Analyze the Redox Reaction

The given equation is a chemical reaction involving iodine ($I_2$), chlorine ($Cl_2$), water ($H_2O$), iodic acid ($HIO_3$), and hydrochloric acid ($HCl$). This is a redox reaction where iodine is oxidized and chlorine is reduced. To balance it, we track the changes in oxidation states:

Iodine ($I$) in $I_2$ has an oxidation state of $0$, and in $HIO_3$, its oxidation state is $+5$. Since there are two iodine atoms in $I_2$, the total change is $2 \times (+5 - 0) = +10$ electrons.
Chlorine ($Cl$) in $Cl_2$ has an oxidation state of $0$, and in $HCl$, it is $-1$. Each chlorine atom gains $1$ electron, and since there are two chlorine atoms in $Cl_2$, the total change is $2 \times (-1 - 0) = -2$ electrons.

Balance the Electrons

To balance the electrons, we match the loss and gain:

Oxidation: $I_2 \rightarrow 2HIO_3 + 10e^-$
Reduction: $Cl_2 + 2e^- \rightarrow 2HCl$

To equate the electrons, multiply the reduction half-reaction by $5$:
$5 \times (Cl_2 + 2e^- \rightarrow 2HCl) = 5Cl_2 + 10e^- \rightarrow 10HCl$
Adding the two half-reactions gives:
$I_2 + 5Cl_2 \rightarrow 2HIO_3 + 10HCl$

Balance Atoms and Finalize the Equation

Now we balance the atoms of oxygen and hydrogen:

Oxygen: There are $2 \times 3 = 6$ oxygen atoms on the right side in $2HIO_3$. To balance this, we need $6H_2O$ on the left.
Hydrogen: With $6H_2O$ on the left, there are $12$ hydrogen atoms. On the right, we have $2H$ from $2HIO_3$ and $10H$ from $10HCl$, totaling $12$ hydrogen atoms.

The equation is now balanced:
$I_2 + 5Cl_2 + 6H_2O \rightarrow 2HIO_3 + 10HCl$

Examples

Redox reactions are fundamental in everyday chemistry, such as in batteries or water purification systems. For instance, when treating water with chlorine to kill bacteria, or when iodine is used as an antiseptic, understanding these reactions helps determine the exact amounts of chemicals needed to achieve the desired effect without leaving harmful residuals. Balancing equations like this ensures that reactants are used efficiently in these vital processes.

Balance the following equation:$I_2+Cl_2+H_2 O \rightarrow HIO_3+HCl$

Verified Answer :

Explanation

Examples

Related Questions

Balance the following equation:

$I_2+Cl_2+H_2 O \rightarrow HIO_3+HCl$