Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
Show the Overall Iconic reaction k2cr2o7 fecl with steps
Accepted Answer
The reaction of potassium dichromate (K2Cr2O7) and iron(II) chloride (FeCl2) is a redox reaction. Here's a breakdown of the balanced ionic equation and the steps involved:
1. Identify the reactants and products:
Reactants: K2Cr2O7 (aq) and FeCl2 (aq)
Products: CrCl3 (aq), FeCl3 (aq), KCl (aq), and H2O (l)
2. Write the unbalanced ionic equation:
Cr2O7^2- (aq) + Fe^2+ (aq) → Cr^3+ (aq) + Fe^3+ (aq)
3. Balance the half-reactions:
Oxidation half-reaction:
Fe^2+ (aq) → Fe^3+ (aq) + e^-
Reduction half-reaction:
Cr2O7^2- (aq) + 14H+ (aq) + 6e^- → 2Cr^3+ (aq) + 7H2O (l)
4. Multiply the half-reactions to balance electrons:
Oxidation half-reaction (multiply by 6):
6Fe^2+ (aq) → 6Fe^3+ (aq) + 6e^-
Reduction half-reaction (as is):
Cr2O7^2- (aq) + 14H+ (aq) + 6e^- → 2Cr^3+ (aq) + 7H2O (l)
5. Add the half-reactions together and cancel out common terms:
Cr2O7^2- (aq) + 14H+ (aq) + 6Fe^2+ (aq) → 2Cr^3+ (aq) + 7H2O (l) + 6Fe^3+ (aq)
6. Include spectator ions:
K2Cr2O7 (aq) + 14HCl (aq) + 6FeCl2 (aq) → 2CrCl3 (aq) + 7H2O (l) + 6FeCl3 (aq) + 2KCl (aq)
Note: The reaction is carried out in acidic conditions, hence the use of HCl. The potassium ions (K+) and chloride ions (Cl-) are spectator ions, meaning they do not participate in the reaction.
Articles you might like