What are the Oxidation and Reducation reactions for these equations :
BaCl2 + NaHCO3 -> BaCO3 + NaCl + HCl
(carbon is the reduction reaction, but I don't know what the oxidation reaction is)
CaCO3 + HCl -> CaCl2 + CO2 + H2O
Neither equation you have written is a redox equation. Check them out. Nothing changes oxidation state (at least I don't think so unless you can point them out to me).
To determine the oxidation and reduction reactions in chemical equations, we need to identify the changes in oxidation states of the atoms. Here's how to find them:
1. BaCl2 + NaHCO3 -> BaCO3 + NaCl + HCl
In this equation, the oxidation states change for carbon (C) and chlorine (Cl) atoms. Let's start with carbon:
Carbon (C) in NaHCO3 has an oxidation state of +4 (from HCO3-), while in BaCO3, it has an oxidation state of +4. Therefore, there is no change in the oxidation state of carbon.
Next, let's consider chlorine:
Chlorine (Cl) in BaCl2 has an oxidation state of -1 (from BaCl2), and in NaCl and HCl, it also has an oxidation state of -1. There is no change in the oxidation state of chlorine either.
Since there is no change in oxidation states for the involved elements (C, Cl), there is neither an oxidation reaction nor a reduction reaction in this equation.
2. CaCO3 + HCl -> CaCl2 + CO2 + H2O
In this equation, the major changes in oxidation states occur for carbon (C) and hydrogen (H):
Carbon (C) in CaCO3 has an oxidation state of +4, while in CO2, it has an oxidation state of +4. There is no change in carbon's oxidation state.
Hydrogen (H) in HCl has an oxidation state of +1, while in H2O, it has an oxidation state of +1. Again, no change in hydrogen's oxidation state.
Similar to the first equation, since there is no change in oxidation states for the elements involved (C, H), there is neither an oxidation nor a reduction reaction in this equation.
In both equations, there are no distinct oxidation or reduction reactions because there are no changes in oxidation states for any of the elements involved.