Final answer:
The decomposition of Na2CO3 into Na2O and CO2 is not a redox reaction as there is no change in the oxidation states involved. The formation of baking soda (NaHCO3) from Na2CO3, water, and CO2 is not a Brønsted-Lowry acid-base reaction as it does not involve the transfer of protons.
Step-by-step explanation:
The decomposition of sodium carbonate (Na2CO3) into sodium oxide (Na2O) and carbon dioxide (CO2) is a chemical reaction that can be assessed for its redox properties. To determine if this is a redox reaction, we would need to look at the oxidation states of the elements involved before and after the reaction. However, it is evident that there is no change in the oxidation number of sodium (Na) from Na2CO3 to Na2O. The carbon in CO2 is at an oxidation state of +4, which is the same as it is in Na2CO3. Since there is no change in the oxidation states of the elements, this reaction is not a redox reaction. Therefore, the correct answer to the statement "Na2CO3 → Na2O + CO2 (Redox or not)" is b) False.
Baking soda, known as NaHCO3, is indeed formed by adding water (H2O) and carbon dioxide (CO2) to sodium carbonate (Na2CO3) according to the reaction:
Na2CO3 + H2O + CO2 → 2NaHCO3
This reaction is not a Brønsted-Lowry acid-base reaction because it does not involve the transfer of an H+ ion. In a Brønsted-Lowry acid-base reaction, a Brønsted-Lowry acid is defined as a proton donor, and a Brønsted-Lowry base is defined as a proton acceptor.