Balance the following equation in acidic conditions Phases are optional.
S2O3 2- + Cu 2+ —> S4O6 2- + Cu+
Concepts and reason
Write the given unbalanced reaction in two half reactions separately.
Balance the atoms other than O and H on both sides. Then, balance the O and H.
Balance the electrons at last. Add the two half reactions to get the final balanced reaction.
A balanced equation is an equation which contains all the reactants and products in a fixed ratio. A balanced equation has the following characteristics:
- It should follow the law of conservation of mass.
- The total number of different types of elements on reactant side should be equal to the product side.
- Stoichiometric coefficients are put in front of the molecules on both the reactant and product side to balance a given reaction. The coefficients to be used are whole number or fractional number.
The unbalanced reaction is written as follows:
The half reactions are written as follows:
Separate the given unbalanced reaction in two half reactions involving the two species.
On balancing the S atoms, the reactions obtained are as follows:
Add a coefficient of 2 before to balance S atoms.
The Cu atoms are balanced.
On balancing the O atom and electrons, the reactions obtained are as follows:
The O atoms are balanced. Balance the charge using the electrons.
There are two atoms with a charge of -2. So, total charge is -4.
The charge of is -2. So, add 2 electrons to the product side to balance the electrons in the first equation.
has +2 charge and has +1 charge. So, add one electron to the reactants in the second equation.
Multiply the second equation by 2 to equate the number of electrons in both the half reactions:
The balanced reaction is written as follows:
The two reactions after balancing the electrons and atoms are as follows:
Add both half reactions as follows:
This is the final balanced reaction.