How would you balance the following equation: Fe + Cl2 + H2O → [Fe(H2O)6]3+ + Cl-?

Question

How would you balance the following equation: Fe + Cl2  	+      H2O  	→	[Fe(H2O)6]3+  	+  	Cl-?

Naomi Aronson · Accepted Answer

You are oxidizing iron, and then making a coordination complex. I will give you a reaction scheme.

EXOXIDATION #Fe(s) + 3/2Cl_2(g) rarr FeCl_3(s)# COMPLEXITY #FeCl_3(s) + 6H_2O(l) rarr [Fe(OH_2)_6]^(3+)(Cl^-)_3# I'm not sure if this is everything you were hoping for.

Cameron Andrews · Answer

#2"Fe" + "3Cl"_2 + "12H"_2"O" → 2["Fe"("H"_2"O")_6]^(3+) + "6Cl"^(-)#

This Socratic response demonstrates how to solve redox equations.

Your formula is:

#"Fe"color(white)(l) + "Cl"_2 + "H"_2"O" → ["Fe"("H"_2"O")_6]^(3+) + "Cl"^(-)#

RESOLUTION:

1: The two partial responses are

#"Fe" → ["Fe"("H"_2"O")_6]^(3+)# #"Cl"_2 → "Cl"^(-)#

2: Balance all atoms other than #"H"# and #"O"#.

#"Fe" → ["Fe"("H"_2"O")_6]^(3+)# #"Cl"_2 → color(red)(2)"Cl"^(-)#

3: Balance #"O"#.

#"Fe"color(white)(l) + color(red)("6H"_2"O") → ["Fe"("H"_2"O")_6]^(3+)# #"Cl"_2 → 2"Cl"^(-)#

4: Harmonize H.

Completed.

5: Charge balance.

#"Fe"color(white)(l)+ "6H"_2"O" → ["Fe"("H"_2"O")_6]^(3+) + color(red)("3e"^(-))# #"Cl"_2 + color(red)("2e"^(-)) → 2"Cl"^(-)#

6: Balance the transferred electrons.

#color(red)(2 ×) {"Fe" + "6H"_2"O" → ["Fe"("H"_2"O")_6]^(3+) + + "3e"^(-)}# #color(red)(3 ×){"Cl"_2 + "2e"^(-) → 2"Cl"^(-)}#

7: Incorporate both half-reactions.

#2"Fe" + 3"Cl"_2 + "12H"_2"O" → 2["Fe"("H"_2"O")_6]^(3+) + "6Cl"^(-)#

8: Verify the mass balance.

On the left: #"2 Fe"; "6 Cl"; "24 H"; "12 O"# On the right: #"2 Fe"; "24 H"; "12 O"; "6 Cl"#

9: Verify the amount due.

On the left: #0# On the right: #"6+ + 6-" = 0#

The equation that is balanced is

#2"Fe" + 3"Cl"_2 + "12H"_2"O" → 2["Fe"("H"_2"O")_6]^(3+) + "6Cl"^(-)#

Henry Antrim · Answer

undefined 6 Fe + 2 Cl₂ + 12 H₂O → 6 [Fe(H₂O)₆]³⁺ + 2 Cl⁻