Question

5 Хлор проявляет свойства окислителя в реакциях:1) Сl2 + H2O--> HCl + HClO2) HCl + O2--> H2O+ Cl3) PbO+ NH4Cl--> Pb+ H2O+ N2+ HCl4) HCl + Ca--> CaCl2+ H25) H2+ Cl2--> HCl6 Второе вещество является окислителем в реакциях:1) K2SO3+ NaMnO4+ NaOH--> K2SO4+ Na2MnO4+ H2O2) SO2+ H2S--> S+ H2O3) H2S+ K2Cr2O7+ H2SO4--> K2SO4+ Cr2(SO4)3+ H2O4) SO4+ HI--> I2+ S+ H2O5) SO2+ NO2--> SO3+ NO

Answer 1

Хлор проявляет свойства окислителя в реакции 1 (реакция диспропорционирования); 5.

 

  Второе вещество является окислителем в следующих реакциях: 1; 3; 5.  

Answer 2

Properties of Chlorine as an Oxidizing Agent:

Chlorine (Cl2) exhibits oxidizing properties in various reactions. Let's examine each reaction mentioned and discuss how chlorine acts as an oxidizing agent in each case.

1) Cl2 + H2O → HCl + HClO: - In this reaction, chlorine (Cl2) oxidizes water (H2O) to form hydrochloric acid (HCl) and hypochlorous acid (HClO). - Chlorine gains electrons from water, causing the oxidation of water molecules. - The oxidation state of chlorine decreases from 0 to -1 in HClO, indicating its role as an oxidizing agent [[1]].

2) HCl + O2 → H2O + Cl2: - In this reaction, hydrogen chloride (HCl) acts as a reducing agent, while oxygen (O2) acts as an oxidizing agent. - Chlorine in HCl is reduced from an oxidation state of +1 to 0 in Cl2, indicating its role as a reducing agent. - Oxygen is oxidized from an oxidation state of 0 to -2 in H2O, indicating its role as an oxidizing agent [[2]].

3) PbO + NH4Cl → Pb + H2O + N2 + HCl: - In this reaction, chlorine in ammonium chloride (NH4Cl) acts as an oxidizing agent. - Chlorine oxidizes lead(II) oxide (PbO) to produce lead (Pb) and chlorine gas (Cl2). - The oxidation state of chlorine decreases from -1 in NH4Cl to 0 in Cl2, indicating its role as an oxidizing agent [[3]].

4) HCl + Ca → CaCl2 + H2: - In this reaction, hydrogen chloride (HCl) acts as a reducing agent, while calcium (Ca) acts as an oxidizing agent. - Chlorine in HCl is reduced from an oxidation state of +1 to 0 in Cl2, indicating its role as a reducing agent. - Calcium is oxidized from an oxidation state of 0 to +2 in CaCl2, indicating its role as an oxidizing agent [[4]].

5) H2 + Cl2 → 2HCl: - In this reaction, hydrogen (H2) acts as a reducing agent, while chlorine (Cl2) acts as an oxidizing agent. - Chlorine in Cl2 is reduced from an oxidation state of 0 to -1 in HCl, indicating its role as a reducing agent. - Hydrogen is oxidized from an oxidation state of 0 to +1 in HCl, indicating its role as an oxidizing agent [[5]].

Second Substance as an Oxidizing Agent:

Now let's examine the reactions where the second substance acts as an oxidizing agent.

1) K2SO3 + NaMnO4 + NaOH → K2SO4 + Na2MnO4 + H2O: - In this reaction, sodium permanganate (NaMnO4) acts as an oxidizing agent. - Sodium permanganate oxidizes potassium sulfite (K2SO3) to produce potassium sulfate (K2SO4). - The oxidation state of manganese in NaMnO4 increases from +7 to +6 in Na2MnO4, indicating its role as an oxidizing agent [[6]].

2) SO2 + H2S → S + H2O: - In this reaction, sulfur dioxide (SO2) acts as an oxidizing agent. - Sulfur dioxide oxidizes hydrogen sulfide (H2S) to produce elemental sulfur (S) and water (H2O). - The oxidation state of sulfur in H2S increases from -2 to 0 in S, indicating the role of SO2 as an oxidizing agent [[7]].

3) H2S + K2Cr2O7 + H2SO4 → K2SO4 + Cr2(SO4)3 + H2O: - In this reaction, potassium dichromate (K2Cr2O7) acts as an oxidizing agent. - Potassium dichromate oxidizes hydrogen sulfide (H2S) to produce potassium sulfate (K2SO4) and chromium(III) sulfate (Cr2(SO4)3). - The oxidation state of chromium in K2Cr2O7 decreases from +6 to +3 in Cr2(SO4)3, indicating its role as an oxidizing agent [[8]].

4) SO4 + HI → I2 + S + H2O: - In this reaction, iodine (I2) acts as an oxidizing agent. - Iodine oxidizes sulfur dioxide (SO2) to produce iodine (I2), sulfur (S), and water (H2O). - The oxidation state of iodine increases from 0 to -1 in I2, indicating its role as an oxidizing agent [[9]].

5) SO2 + NO2 → SO3 + NO: - In this reaction, nitrogen dioxide (NO2) acts as an oxidizing agent. - Nitrogen dioxide oxidizes sulfur dioxide (SO2) to produce sulfur trioxide (SO3) and nitrogen monoxide (NO). - The oxidation state of nitrogen in NO2 decreases from +4 to +2 in NO, indicating its role as an oxidizing agent [[10]].

In conclusion, chlorine exhibits oxidizing properties in reactions where it undergoes reduction, while the second substances mentioned in the reactions act as oxidizing agents by undergoing oxidation.