What is the balanced equation for the redox reaction between Cr2O7^2- and Fe^2+ in acidic medium? (2020)
Practice Questions
1 question
Q1
What is the balanced equation for the redox reaction between Cr2O7^2- and Fe^2+ in acidic medium? (2020)
Cr2O7^2- + 6Fe^2+ → 2Cr^3+ + 3Fe^3+
Cr2O7^2- + 3Fe^2+ → 2Cr^3+ + 3Fe^3+
Cr2O7^2- + 4Fe^2+ → 2Cr^3+ + 4Fe^3+
Cr2O7^2- + 2Fe^2+ → 2Cr^3+ + Fe^3+
The balanced equation in acidic medium is Cr2O7^2- + 6Fe^2+ → 2Cr^3+ + 3Fe^3+.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the balanced equation for the redox reaction between Cr2O7^2- and Fe^2+ in acidic medium? (2020)
Solution: The balanced equation in acidic medium is Cr2O7^2- + 6Fe^2+ → 2Cr^3+ + 3Fe^3+.
Steps: 5
Step 1: Identify the reactants and products. The reactants are Cr2O7^2- (dichromate ion) and Fe^2+ (iron(II) ion). The products are Cr^3+ (chromium ion) and Fe^3+ (iron(III) ion).
Step 2: Write the half-reactions for the oxidation and reduction processes. The reduction half-reaction is Cr2O7^2- → Cr^3+, and the oxidation half-reaction is Fe^2+ → Fe^3+.
Step 3: Balance the half-reactions. For the reduction half-reaction, balance the chromium atoms and add H+ ions to balance the charge. For the oxidation half-reaction, balance the iron atoms.
Step 4: Combine the half-reactions. Make sure the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.
Step 5: Write the final balanced equation. Combine the balanced half-reactions to get the overall balanced equation: Cr2O7^2- + 6Fe^2+ → 2Cr^3+ + 3Fe^3+.
