Question

H2O2 + NiS + H2SO4 = S + NiSO4 + H2O нужно уравнять и расставить степени окисления, написать электронные уравнения, найти восстановители и окислители. помогите пожалуйста!)

Answer 1

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Answer 2

#### Balancing and Assigning Oxidation States in the Chemical Equation To balance the chemical equation and assign oxidation states, let's break down the given equation: H2O2 + NiS + H2SO4 = S + NiSO4 + H2O #### Balancing the Equation To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation. Here's how we can balance it step by step: 1. Balance the sulfur (S) atoms: - There is one sulfur atom on the left side and one on the right side, so sulfur is already balanced. 2. Balance the nickel (Ni) atoms: - There is one nickel atom on the left side and one on the right side, so nickel is already balanced. 3. Balance the hydrogen (H) atoms: - There are four hydrogen atoms on the left side (two in H2O2 and two in H2SO4). - To balance the hydrogen atoms on the right side, we need to add two more hydrogen atoms to the product side. We can do this by adding H2O to the right side of the equation. The balanced equation becomes: H2O2 + NiS + H2SO4 = S + NiSO4 + 2H2O #### Assigning Oxidation States To assign oxidation states, we need to determine the charge that each atom would have if all the bonds were 100% ionic. Here are the oxidation states for each element in the equation: - Hydrogen (H): +1 - Oxygen (O): -2 - Sulfur (S): +6 - Nickel (Ni): +2 #### Identifying Reducing Agents and Oxidizing Agents In a redox reaction, the reducing agent is the species that gets oxidized (loses electrons), while the oxidizing agent is the species that gets reduced (gains electrons). In the given equation, the reducing agent is **H2O2** because it loses oxygen and its oxidation state changes from -1 to 0. It is oxidized to form water (H2O). The oxidizing agent is **NiS** because it gains oxygen and its oxidation state changes from +2 to +6. It is reduced to form nickel sulfate (NiSO4). #### Electron Transfer and Half-Reactions To write the electron transfer and half-reactions, we need to separate the oxidation and reduction processes. The oxidation half-reaction is: **H2O2 -> 2H2O + 2e-** The reduction half-reaction is: **NiS + 2e- -> NiSO4** #### Summary In summary, the balanced equation is: H2O2 + NiS + H2SO4 = S + NiSO4 + 2H2O The oxidation states are: - Hydrogen (H): +1 - Oxygen (O): -2 - Sulfur (S): +6 - Nickel (Ni): +2 The reducing agent is H2O2, and the oxidizing agent is NiS. The electron transfer and half-reactions are: Oxidation half-reaction: H2O2 -> 2H2O + 2e- Reduction half-reaction: NiS + 2e- -> NiSO4 I hope this helps! Let me know if you have any further questions.