A double-replacement reaction takes place when aqueous K2SO4 reacts with aqueous Pb(NO3)2. You would expect one of the products
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Balancing redox reactions:
Oxygen should be balanced by adding as needed, while hydrogen should be balanced by adding
.
What is a redox reaction?
Redox reactions, also known as oxidation-reduction reactions, involve the simultaneous oxidation and reduction of two different reactants.
The Half-Equation Method is one technique used to balance redox processes. The equation is divided into two half-equations using this technique: one for oxidation and one for reduction.
By changing the coefficients and adding ,
, and
in that order, each reaction is brought into equilibrium:
- By putting the right number of water (
) molecules on the other side of the equation, the oxygen atoms are brought into balance.
- By adding
ions to the opposing side of the equation, one can balance the hydrogen atoms (including those added in step 2 to balance the oxygen atom).
- Total the fees for each side. Add enough electrons (
) to the more positive side to make them equal. (As a general rule,
- The
- One balanced equation is created by adding the two half-equations and canceling out the electrons. Additionally, common terms should be eliminated.
- Now that the equation has been verified, it can be balanced.
Learn more about redox reaction here,
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