Question

Умоляю, помогите!!!!! Совершенно не понимаю окислительно-восстановительные реакции завтра пилить по полной будут... Нужно написать уравнения реакций между следующими веществами: Оксид углерода (IV) + гидроксид бария Оксид хрома (III) + водород Кальциий + вода Оксид углерода (II) + кислород = оксид углерода (IV) Сульфат меди (II) + гидроксид калия Железо + соляная кислота Йодид калия + хлор Определить, какие из этих реакций являются окислительно-восстановительными, указать окислитель и восстановитель, написать переход электронов.

Answer 1

2) Cr2O3 + 3H2 = 3H2O + 2Cr
Электроны переходят от водорода к хрому.
Электронный баланс (методом полуреакций уравнивать не буду, здесь полуреакции будут страшными):
2Cr(+3) + 6e = 2Cr(0)
H2(0) - 2e = 2H(+1)
() - степень окисления, без () - заряд иона

3) Ca + 2H2O = Ca(OH)2 + H2
Ca - 2e = Ca2+
2H(+1) + 2e = H2

4) 2CO + O2 = 2CO2
C(+2) - 2e = C(+4)
O2(0) + 4e = 2O(-2)

6) Fe + 2HCl = FeCl2 + H2
2H+ + 2e = H2
Fe(0) - 2e = Fe2+

7)2KI + Cl2 = 2KCl + I2
2I- - 2e = I2
Cl2 + 2e = 2Cl-

Answer 2

Oxidation-Reduction Reactions and Equations

Oxidation-reduction reactions, also known as redox reactions, involve the transfer of electrons between reactants. In these reactions, one substance loses electrons (undergoes oxidation) while another substance gains electrons (undergoes reduction). To determine if a reaction is an oxidation-reduction reaction, we need to identify the changes in oxidation states of the elements involved.

Let's go through each of the given reactions and determine if they are oxidation-reduction reactions, identify the oxidizing and reducing agents, and write the electron transfer.

1. Oxide of Carbon (IV) + Barium Hydroxide The reaction between carbon dioxide (CO2) and barium hydroxide (Ba(OH)2) can be represented by the following equation: ``` CO2 + Ba(OH)2 → BaCO3 + H2O ``` This reaction is not an oxidation-reduction reaction since there is no change in the oxidation states of the elements involved.

2. Chromium (III) Oxide + Hydrogen The reaction between chromium (III) oxide (Cr2O3) and hydrogen (H2) can be represented by the following equation: ``` Cr2O3 + 3H2 → 2Cr + 3H2O ``` This reaction is an oxidation-reduction reaction. Chromium (III) is reduced from an oxidation state of +3 to 0, while hydrogen is oxidized from an oxidation state of 0 to +1. The reducing agent is hydrogen, which donates electrons, and the oxidizing agent is chromium (III), which accepts electrons. The electron transfer can be represented as follows: ``` Cr2O3 + 3H2 → 2Cr + 3H2O [Cr(III)] + 3[H2] → 2[Cr] + 3[H2O] ```

3. Calcium + Water The reaction between#### Understanding Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between reactants. In these reactions, one substance loses electrons (oxidation) while another gains electrons (reduction). Let's analyze the given reactions and identify which ones are redox reactions, specify the oxidizing and reducing agents, and describe the electron transfer.

Analyzing the Given Reactions

1. Oxide of Carbon (IV) + Barium Hydroxide - The reaction between oxide of carbon (IV) and barium hydroxide is a neutralization reaction, not a redox reaction. It forms barium carbonate and water.

2. Chromium (III) Oxide + Hydrogen - The reaction between chromium (III) oxide and hydrogen is a redox reaction. Chromium undergoes reduction, and hydrogen undergoes oxidation.

3. Calcium + Water - The reaction between calcium and water is a redox reaction. Calcium undergoes oxidation, and water undergoes reduction.

4. Carbon Monoxide + Oxygen - The reaction between carbon monoxide and oxygen is a redox reaction. Carbon monoxide undergoes oxidation, and oxygen undergoes reduction.

5. Copper (II) Sulfate + Potassium Hydroxide - The reaction between copper (II) sulfate and potassium hydroxide is a double displacement reaction, not a redox reaction. It forms copper hydroxide and potassium sulfate.

6. Iron + Hydrochloric Acid - The reaction between iron and hydrochloric acid is a redox reaction. Iron undergoes oxidation, and hydrogen ions in the acid undergo reduction.

7. Potassium Iodide + Chlorine - The reaction between potassium iodide and chlorine is a redox reaction. Potassium iodide undergoes oxidation, and chlorine undergoes reduction.

Identifying Oxidizing and Reducing Agents

- Chromium (III) Oxide + Hydrogen - Chromium (III) oxide is the reducing agent, and hydrogen is the oxidizing agent.

- Calcium + Water - Calcium is the reducing agent, and water is the oxidizing agent.

- Carbon Monoxide + Oxygen - Carbon monoxide is the reducing agent, and oxygen is the oxidizing agent.

- Iron + Hydrochloric Acid - Iron is the reducing agent, and hydrogen ions in the acid are the oxidizing agent.

- Potassium Iodide + Chlorine - Potassium iodide is the reducing agent, and chlorine is the oxidizing agent.

Describing Electron Transfer

- Chromium (III) Oxide + Hydrogen - Chromium (III) oxide transfers electrons to hydrogen.

- Calcium + Water - Calcium transfers electrons to water.

- Carbon Monoxide + Oxygen - Carbon monoxide transfers electrons to oxygen.

- Iron + Hydrochloric Acid - Iron transfers electrons to hydrogen ions in the acid.

- Potassium Iodide + Chlorine - Potassium iodide transfers electrons to chlorine.

I hope this helps you understand the concept of oxidation-reduction reactions better! If you have further questions or need more assistance, feel free to ask.