Question

Zn(OH) 2 → H 2 O → HNO 3 → Zn(NO 3 ) 2 → ZnO → CaZnO 2

Answer 1

Zn(OH)2 → H2O → HNO3 → Zn(NO3)2 → ZnO → CaZnO2.

(1) Zn(OH)2 → ZnO + H2O.

(2) N2O5 + H2O → 2HNO3.

(3) ZnO + 2HNO3 → Zn(NO3)2 + H2O.

(4) 2Zn(NO3)2 → 2ZnO + 4NO2 + O2.

(5) ZnO + CaO → CaZnO2.

Answer 2

The series of reactions you've provided appears to describe the transformation of zinc hydroxide (Zn(OH)2) into calcium zincate (CaZnO2) via several intermediate steps. Let's break down each step:

1. Zn(OH)2 → H2O:

   • In this step, zinc hydroxide (Zn(OH)2) loses water (H2O) to form zinc oxide (ZnO).

2. H2O → HNO3:

   • This step suggests that water (H2O) is converted into nitric acid (HNO3). This typically involves a chemical reaction between water and nitric oxide (NO) or nitrogen dioxide (NO2) to form nitric acid.

3. HNO3 → Zn(NO3)2:

   • Here, nitric acid (HNO3) reacts with zinc (Zn) to form zinc nitrate (Zn(NO3)2). This is an acid-base reaction.

4. Zn(NO3)2 → ZnO:

   • Zinc nitrate (Zn(NO3)2) decomposes to yield zinc oxide (ZnO) as a product. This is typically accomplished by heating the nitrate salt, causing it to break down into the metal oxide and nitrogen oxides.

5. ZnO → CaZnO2:

   • Finally, zinc oxide (ZnO) appears to react with calcium oxide (CaO) to form calcium zincate (CaZnO2). This step involves the combination of the two metal oxides to produce a compound containing both calcium and zinc.

Please note that specific reaction conditions and stoichiometries would be necessary to carry out these reactions successfully in a laboratory setting. Additionally, it's important to consider safety precautions when working with chemicals, especially strong acids like nitric acid. Always consult appropriate references and perform experiments in a controlled environment if attempting these reactions.