Question

Отримайте цинк сульфат не менш ніж п’ятьма різними способами. Назвіть типи хімічних реакцій, рівняння яких ви написали. На прикладі однієї з реакцій розрахуйте, які маси кожного з реагентів будуть потрібні для одержання 2,5 моль цинк сульфату. Визначте серед написаних вами рівнянь окисно-відновні. Укажіть окисник і відновник.

Answer 1

Ответ:

Я сам хз

Объяснение:

Answer 2

Methods of Obtaining Zinc Sulfate

There are several methods for obtaining zinc sulfate. Here are five different ways to obtain zinc sulfate:

1. Reaction between zinc oxide and sulfuric acid: Zinc oxide reacts with sulfuric acid to produce zinc sulfate and water. The balanced chemical equation for this reaction is:

   ZnO + H2SO4 -> ZnSO4 + H2O
   

2. Reaction between zinc carbonate and sulfuric acid: Zinc carbonate reacts with sulfuric acid to produce zinc sulfate, carbon dioxide, and water. The balanced chemical equation for this reaction is:

   ZnCO3 + H2SO4 -> ZnSO4 + CO2 + H2O
   

3. Reaction between zinc metal and sulfuric acid: Zinc metal reacts with sulfuric acid to produce zinc sulfate and hydrogen gas. The balanced chemical equation for this reaction is:

   Zn + H2SO4 -> ZnSO4 + H2
   

4. Reaction between zinc hydroxide and sulfuric acid: Zinc hydroxide reacts with sulfuric acid to produce zinc sulfate and water. The balanced chemical equation for this reaction is:

   Zn(OH)2 + H2SO4 -> ZnSO4 + 2H2O
   

5. Reaction between zinc chloride and sulfuric acid: Zinc chloride reacts with sulfuric acid to produce zinc sulfate and hydrochloric acid. The balanced chemical equation for this reaction is:

   ZnCl2 + H2SO4 -> ZnSO4 + 2HCl
   

Calculation of Reactant Masses

Let's consider the first reaction between zinc oxide and sulfuric acid to calculate the masses of each reactant required to obtain 2.5 moles of zinc sulfate (ZnSO4).

The molar mass of zinc sulfate (ZnSO4) is calculated as follows: - Atomic mass of zinc (Zn) = 65.38 g/mol - Atomic mass of sulfur (S) = 32.07 g/mol - Atomic mass of oxygen (O) = 16.00 g/mol - Molar mass of zinc sulfate (ZnSO4) = (65.38 g/mol) + (32.07 g/mol) + 4 * (16.00 g/mol) = 161.38 g/mol

To obtain 2.5 moles of zinc sulfate, we can use the molar ratio between zinc oxide (ZnO) and zinc sulfate (ZnSO4) from the balanced chemical equation: - From the balanced equation: 1 mole of ZnO produces 1 mole of ZnSO4

Therefore, the mass of zinc oxide required can be calculated as follows: - Mass of zinc oxide = (2.5 moles) * (molar mass of ZnO)

Similarly, the mass of sulfuric acid required can be calculated using the molar ratio between sulfuric acid (H2SO4) and zinc sulfate (ZnSO4) from the balanced chemical equation: - From the balanced equation: 1 mole of H2SO4 produces 1 mole of ZnSO4

Therefore, the mass of sulfuric acid required can be calculated as follows: - Mass of sulfuric acid = (2.5 moles) * (molar mass of H2SO4)

Oxidation-Reduction Reactions

Among the reactions mentioned above, the reaction between zinc metal and sulfuric acid is an example of an oxidation-reduction (redox) reaction. In this reaction, zinc is oxidized to zinc ions, and hydrogen ions from sulfuric acid are reduced to hydrogen gas.

The balanced chemical equation for this redox reaction is: ``` Zn + H2SO4 -> ZnSO4 + H2 ```

In this reaction, zinc is the reducing agent (it donates electrons and gets oxidized), and hydrogen ions (H+) from sulfuric acid are the oxidizing agent (they accept electrons and get reduced).

Please let me know if there is anything else I can help you with!