Question

Ca→CaO->Ca(OH)2->CaCO3 C->CO2->CaCO3S->SO2->H2SO3->MgSO3CL2→ HCL → AlCI3​

Answer 1

Ответ: C+O2=CO2

CO2+CaO=CaCO3

S+O2=SO2

SO2+H2O=H2SO3

H2SO3+MgO=MgSO3+H2O

Cl2+H2=2HCl

2Al + 6HCl= 2AlCl3+3H2

Объяснение:

Answer 2

It seems like you're describing a series of chemical reactions involving different elements and compounds. Let's break down each reaction step by step:

1. Ca → CaO: This represents the reaction of calcium (Ca) with oxygen (O) to form calcium oxide (CaO). This is a typical example of a metal reacting with oxygen to form a metal oxide.

2. CaO → Ca(OH)2: Calcium oxide (CaO) reacts with water (H2O) to produce calcium hydroxide (Ca(OH)2). This is an example of a basic oxide reacting with water to form a base.

3. Ca(OH)2 → CaCO3: Calcium hydroxide (Ca(OH)2) can undergo carbonation, a process in which it reacts with carbon dioxide (CO2) from the atmosphere to form calcium carbonate (CaCO3). This is a common reaction that occurs when calcium hydroxide is exposed to carbon dioxide.

4. C → CO2: Carbon (C) reacts with oxygen (O) to produce carbon dioxide (CO2). This is a combustion reaction where carbon oxidizes.

5. CaCO3S → SO2: It appears that sulfur dioxide (SO2) is produced from the decomposition of calcium carbonate sulfate (CaCO3S). This reaction likely involves the release of carbon dioxide and sulfur dioxide gases.

6. SO2 → H2SO3: Sulfur dioxide (SO2) can react with water (H2O) to form sulfurous acid (H2SO3). This is an acid-base reaction.

7. H2SO3 → MgSO3: It seems that sulfurous acid (H2SO3) reacts with magnesium oxide (MgO) to produce magnesium sulfite (MgSO3). This reaction likely involves the displacement of hydrogen from the acid by magnesium.

8. Cl2 → HCl: Chlorine gas (Cl2) reacts with water (H2O) to form hydrochloric acid (HCl). This is an example of a redox reaction where chlorine is reduced.

9. HCl → AlCl3: Hydrochloric acid (HCl) reacts with aluminum (Al) to produce aluminum chloride (AlCl3). This is a typical acid-base reaction involving a metal.

Please note that the above reactions are general representations, and the actual reaction conditions, stoichiometry, and products may vary depending on the specific reaction conditions and the presence of catalysts or other reactants.