Question

НАПИШИТЕ, ПОЖАЛУЙСТА, УСЛОВИЯ ПРОТЕКАНИЯ ДАННЫХ (УЖЕ РЕШЁННЫХ!!!) РЕАКЦИЙ:1. C + O2 → CO2↑2. CaO + CO2 → CaCO3↓3. CaCO3 + 2HCl (разб.) = CaCl2 + CO2↑ + H2O4. CaCO3 –t→ CaO + CO2↑5. CaO + H2O → Ca(OH)26. Ca(OH)2 + 2HClO → Ca(OCl)2 + 2H2O7. CaOCl2 + H2SO4 = CaSO4 + НСl + НСlO8. CaCO3 + H2CO3 → Ca(HCO3)29. Ca(HCO3)2 –t→ CaCO3 + CO2 + H2O

Answer 1

1) 600—700°C, сжигание на воздухе

2) при комнатной температуре

3) 

4) 900—1200°C

5) при комнатной температуре

6) 

7) при кипячении

8) 

9)

Answer 2

Conditions for the Given Reactions:

1. C + O2 → CO2↑: - This is the combustion reaction of carbon (C) with oxygen (O2) to produce carbon dioxide (CO2). - The reaction occurs in the presence of oxygen gas. - The reaction is exothermic, meaning it releases heat. - The reaction is typically initiated by heating or by the presence of a spark. - The balanced chemical equation for this reaction is: 2C + O2 → 2CO2 [[1]].

2. CaO + CO2 → CaCO3↓: - This is a precipitation reaction between calcium oxide (CaO) and carbon dioxide (CO2) to form calcium carbonate (CaCO3). - The reaction occurs when calcium oxide reacts with carbon dioxide gas. - The reaction is exothermic and releases heat. - The balanced chemical equation for this reaction is: CaO + CO2 → CaCO3 [[2]].

3. CaCO3 + 2HCl (dissolved) = CaCl2 + CO2↑ + H2O: - This is an acid-base reaction between calcium carbonate (CaCO3) and hydrochloric acid (HCl) to form calcium chloride (CaCl2), carbon dioxide (CO2), and water (H2O). - The reaction occurs when calcium carbonate reacts with hydrochloric acid. - The reaction is exothermic and releases heat. - The balanced chemical equation for this reaction is: CaCO3 + 2HCl → CaCl2 + CO2 + H2O [[3]].

4. CaCO3 –t→ CaO + CO2↑: - This is a thermal decomposition reaction of calcium carbonate (CaCO3) to form calcium oxide (CaO) and carbon dioxide (CO2). - The reaction occurs when calcium carbonate is heated. - The reaction is endothermic, meaning it absorbs heat. - The balanced chemical equation for this reaction is: CaCO3 → CaO + CO2 [[4]].

5. CaO + H2O → Ca(OH)2: - This is a hydration reaction between calcium oxide (CaO) and water (H2O) to form calcium hydroxide (Ca(OH)2). - The reaction occurs when calcium oxide reacts with water. - The reaction is exothermic and releases heat. - The balanced chemical equation for this reaction is: CaO + H2O → Ca(OH)2 [[5]].

6. Ca(OH)2 + 2HClO → Ca(OCl)2 + 2H2O: - This is a displacement reaction between calcium hydroxide (Ca(OH)2) and hypochlorous acid (HClO) to form calcium hypochlorite (Ca(OCl)2) and water (H2O). - The reaction occurs when calcium hydroxide reacts with hypochlorous acid. - The reaction is exothermic and releases heat. - The balanced chemical equation for this reaction is: Ca(OH)2 + 2HClO → Ca(OCl)2 + 2H2O [[6]].

7. CaOCl2 + H2SO4 = CaSO4 + HCl + HClO: - This is a double displacement reaction between calcium hypochlorite (CaOCl2) and sulfuric acid (H2SO4) to form calcium sulfate (CaSO4), hydrochloric acid (HCl), and hypochlorous acid (HClO). - The reaction occurs when calcium hypochlorite reacts with sulfuric acid. - The reaction is exothermic and releases heat. - The balanced chemical equation for this reaction is: CaOCl2 + H2SO4 → CaSO4 + HCl + HClO [[7]].

8. CaCO3 + H2CO3 → Ca(HCO3)2: - This is a neutralization reaction between calcium carbonate (CaCO3) and carbonic acid (H2CO3) to form calcium bicarbonate (Ca(HCO3)2). - The reaction occurs when calcium carbonate reacts with carbonic acid. - The reaction is exothermic and releases heat. - The balanced chemical equation for this reaction is: CaCO3 + H2CO3 → Ca(HCO3)2 [[8]].

9. Ca(HCO3)2 –t→ CaCO3 + CO2 + H2O: - This is a thermal decomposition reaction of calcium bicarbonate (Ca(HCO3)2) to form calcium carbonate (CaCO3), carbon dioxide (CO2), and water (H2O). - The reaction occurs when calcium bicarbonate is heated. - The reaction is endothermic, meaning it absorbs heat. - The balanced chemical equation for this reaction is: Ca(HCO3)2 → CaCO3 + CO2 + H2O [[9]].

Please note that these reactions are described based on the information provided and may vary depending on specific conditions and concentrations.