Balancing of Redox Reactions
C2 H5 OH + Cr2 07 +H ----> Cr 3+ + C₂H4O +H2O
Answers
Answer:
3 C2H5OH + 2 K2Cr2O7 + 8 H2SO4 → 3 CH3COOH + 2 Cr2(SO4)3 + 2 K2SO4 + 11 H2O
Answer:
Explanation:
Steps in Balancing Oxidation-Reduction Equations in Acidic Solution: Half reaction method:
1. Split the skeleton equation into two half-reactions, proceeding as follows. Note the species containing the
element that increases in oxidation number and write those species to give the oxidation half-reaction. Similarly,
note the species containing the element that decreases in oxidation number and write the reduction halfreaction.
2. Complete and balance each half-reaction.
a. Balance all atoms except O and H.
b. Balance O atoms by adding H2O’s to one side of the equation.
c. Balance H atoms by adding H+ to one side of the equation.
d. Balance electric charge by adding electrons (e−
) to the more positive side.
3. Combine the two half-reactions to obtain the final balanced oxidation-reduction equation.
a. Multiply each half-reaction by a factor such that when the half-reactions are added, the electrons
cancel. (Electrons cannot appear in the final equation.)
b. Simplify the balanced equation by canceling species that occur on both sides and reduce the coefficients
to smallest whole numbers. Check that the equation is indeed balanced.
Additional Steps for Balancing Oxidation-Reduction Equations in Basic Solution
4. Note the number of H+ ions in the equation. Add this number of OH− ions to both sides of the equation.
5. Simplify the equation by noting that H+ reacts with OH− to give H2O.
6. Cancel any H2O’s that occur on both sides of the equation and reduce the equation to simplest terms.