write the equation for the reaction of fecl2 with k3[fe(cn)6]???
To write the equation for the reaction between FeCl2 and K3[Fe(CN)6], we need to determine the oxidation states of the elements involved.
1. Start by identifying the elements and their respective known oxidation states:
- Fe (Iron)
- Cl (Chlorine)
- K (Potassium)
- C (Carbon)
- N (Nitrogen)
2. Assign oxidation states to the elements:
- Fe in FeCl2 has an oxidation state of +2. This is because chlorine usually has an oxidation state of -1, and there are two chlorine ions (Cl-) in FeCl2, so Fe must be +2 to balance the charge.
- K in K3[Fe(CN)6] has an oxidation state of +1 because it usually has a +1 oxidation state in most compounds.
- C in [Fe(CN)6] has an oxidation state of -1. This is because the overall charge of the complex is -6 (since K has a +1 charge), and there are six cyanide ions (CN-) that each carry a -1 charge. Hence, Fe should have an oxidation state of +4 to balance the charges.
- N in [Fe(CN)6] has an oxidation state of -3. This is because each cyanide ion (CN-) has a -1 charge, and there are six CN- ions in total.
- Cl in FeCl2 has an oxidation state of -1.
3. Based on the oxidation states, we can write the balanced equation for the reaction:
FeCl2 + K3[Fe(CN)6] -> K4[Fe(CN)6] + KCl
Note: The products of the reaction are potassium hexacyanoferrate(II) [K4[Fe(CN)6]] and potassium chloride (KCl).