Question

Дуже потрібно! Допоможіть будь ласка! ( даю всі бали, що є) (75) Виставте ступені окиснення та розставте коефіцієнти в рівняннях реакцій методом електронного балансу, вкажіть окисники й відновники, а також процес окиснення та процес відновлення. Со + HNO3 → Co(NO3)2 + N2+ H2O

Answer 1

Ответ:

5Co(0)+12H(+1)N(+5)O(-2)3 = 5Co(NO3)2+N(0)2+6H(+1)2O(-2)

окисникN(+5)+5ел.- =N(0)відновлення (2)

відновникCo(0)-2ел.= Co(+2)окислення (5)

Объяснение:

ЭТО ПРАВЕЛЬНО УДАЧИ ТЕБЕ В УЧЕБЕ

Answer 2

Ответ:

Ступені окиснення елементів у сполуках:

Со: +2 HNO₃: +5 (N), -2 (O) Co(NO₃)₂: +2 (Co), +5 (N), -2 (O) N₂: 0 H₂O: -2 (O), +1 (H)

Розставимо коефіцієнти перед речовинами, щоб збалансувати оксиданти й відновники:

Со + 8HNO₃ → Co(NO₃)₂ + 2N₂ + 4H₂O

Процес окиснення: Co переходить з окиснення +2 до +3 (в Co(NO₃)₂).

Процес відновлення: HNO₃ переходить з окиснення +5 до +2 (в N₂).

Оксидант: HNO₃

Відновник: Co

Answer 3

Stating the Facts and Citing Sources

To balance the equation and determine the oxidation states, coefficients, oxidizing agents, and reducing agents, we will use the method of electron balance. Here is the balanced equation and the information you requested:

The given equation is: Co + HNO3 → Co(NO3)2 + N2 + H2O

To balance the equation, we will follow these steps:

Step 1: Assign oxidation states to each element in the equation. Step 2: Identify the elements that are undergoing oxidation and reduction. Step 3: Balance the equation by adding coefficients to the reactants and products. Step 4: Verify the balance by checking the number of atoms and the charge on both sides of the equation.

Step 1: Assigning Oxidation States

To determine the oxidation states, we need to know the general rules for assigning oxidation states:

1. The oxidation state of an element in its elemental form is always zero. 2. The sum of the oxidation states of all atoms in a neutral compound is zero. 3. The sum of the oxidation states of all atoms in an ion is equal to the charge of the ion. 4. The oxidation state of hydrogen is usually +1, except when it is bonded to metals, where it is -1. 5. The oxidation state of oxygen is usually -2, except in peroxides (where it is -1) and in compounds with fluorine (where it is positive). 6. The oxidation state of a monatomic ion is equal to its charge.

Based on these rules, we can assign the oxidation states as follows:

- The oxidation state of Co is unknown. - The oxidation state of H in HNO3 is +1. - The oxidation state of N in HNO3 is +5. - The oxidation state of O in HNO3 is -2.

Step 2: Identifying Oxidation and Reduction

In the given equation, Co is being oxidized from an unknown oxidation state to +2 in Co(NO3)2. This means that Co is the reducing agent.

On the other hand, HNO3 is being reduced from +5 to +2 in Co(NO3)2. This means that HNO3 is the oxidizing agent.

Step 3: Balancing the Equation

Now that we have identified the oxidation states and the oxidizing and reducing agents, we can balance the equation.

The balanced equation is: 3Co + 8HNO3 → 3Co(NO3)2 + 2NO + 4H2O

Step 4: Verifying the Balance

To verify the balance, we count the number of atoms and the charge on both sides of the equation:

Reactants: - Co: 3 atoms - H: 24 atoms - N: 24 atoms - O: 72 atoms - Charge: 0

Products: - Co: 3 atoms - H: 24 atoms - N: 6 atoms - O: 48 atoms - Charge: 0

The number of atoms and the charge are balanced on both sides of the equation, confirming that the equation is balanced.

Summary

In summary, the balanced equation is: 3Co + 8HNO3 → 3Co(NO3)2 + 2NO + 4H2O. The oxidation state of Co changes from an unknown state to +2, making it the reducing agent. The oxidation state of HNO3 changes from +5 to +2, making it the oxidizing agent.

Please note that the oxidation state of Co in the original equation was not provided, so it was assumed to be unknown.