2NaHCO3 --- Na2CO3 + H2O + CO2
2Fe + 6 HCl -- 2 FeCl3 + 3H2
2HBr + Ca(OH)2 -- CaBr2 + 2H2O
N2 + 3H -- 2NH3
2H2O -- 2H2O + O
is this a redox ? what is oxidized, reduced
To determine if a chemical reaction is a redox reaction, you need to identify the changes in oxidation states of the elements involved. An oxidation state is a measure of the number of electrons an atom has gained or lost to form an ion or bond.
Let's analyze each reaction:
1. 2NaHCO3 → Na2CO3 + H2O + CO2
- In this reaction, the oxidation states of the elements involved (Na, H, C, and O) remain unchanged. There is no change in oxidation states, so this is not a redox reaction.
2. 2Fe + 6HCl → 2FeCl3 + 3H2
- Iron (Fe) goes from an oxidation state of 0 on the reactant side to +3 on the product side. This means iron is oxidized (loses electrons) and is the reducing agent (oxidizing another species) in this redox reaction.
3. 2HBr + Ca(OH)2 → CaBr2 + 2H2O
- In this reaction, the oxidation states of the elements involved (H, Br, Ca, and O) remain unchanged. There is no change in oxidation states, so this is not a redox reaction.
4. N2 + 3H2 → 2NH3
- Nitrogen (N) goes from an oxidation state of 0 to -3 in NH3. This means nitrogen is reduced (gains electrons) and is the oxidizing agent (reducing another species) in this redox reaction.
5. 2H2O → 2H2O + O
- In this reaction, there is a change in the number of oxygen atoms (O2 on the reactant side and O on the product side) but no change in the oxidation states. There is no change in oxidation states, so this is not a redox reaction.
In summary, only reactions 2 and 4 are redox reactions. In reaction 2, iron is oxidized, and in reaction 4, nitrogen is reduced.