"Nitrogen and Its Compounds" Important non-metallic elements in chemical production PPT (Lesson 3: Nitric acid rain and its prevention and control)

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"Nitrogen and Its Compounds" Important non-metallic elements in chemical production PPT (Lesson 3: Nitric acid rain and its prevention and control)

Part 1: Essential knowledge and foundation of literacy

1. Properties of nitric acid

1.Physical properties

2. Chemical properties

(1)Acidity:

The equation for ionization in water is _______________.

(2)Instability:

Concentrated nitric acid will decompose when exposed to light or heat. The chemical equation is _______________________________.

[Micro Thought] According to the properties of concentrated nitric acid, how should concentrated nitric acid be stored?

Tip: Concentrated nitric acid is easy to decompose when exposed to light or heat, so concentrated nitric acid should be stored in a brown reagent bottle and placed in a cool place.

【Smart Judgment】

(1) The greater the concentration of nitric acid, the stronger its oxidizing property. ()

Tips:√. It can be seen from the severity of the reaction between copper and concentrated and dilute nitric acid that the greater the concentration of nitric acid, the stronger the oxidizing property.

(2) The reaction between copper and concentrated nitric acid can only generate nitrogen dioxide gas. ()

Tip:×. The reaction between copper and concentrated nitric acid begins to generate NO2 gas, but as the nitric acid concentration decreases, NO gas will be generated.

(3) In the reaction between copper and nitric acid, nitric acid only exhibits oxidizing properties. ()

Tip:×. In the reaction between copper and nitric acid, NO2 (or NO) is generated, and copper nitrate is generated. Nitric acid exhibits both oxidizing and acidic properties.

②Exhibition of strong oxidation:

Write the following chemical equation for the reaction:

a. React with metal:

Dilute nitric acid reacts with copper: _______________________________.

Concentrated nitric acid reacts with copper: ____________________________.

b. React with non-metals:

The reaction between concentrated nitric acid and red hot C (oxidized to CO2) is ____________________________.

[Situation·Thinking] A student took out a bottle of concentrated nitric acid in the laboratory and found that the solution was yellow, which was inconsistent with the description of nitric acid in the textbook.

(1) Can you help the student explain the reason?

Tip: Concentrated nitric acid is unstable and will decompose to produce NO2 when exposed to light or heat. NO2 dissolves in concentrated nitric acid and makes the solution yellow.

(2) Can you help this student remove the yellow color of nitric acid?

Tip: Pour oxygen (or air) into the concentrated nitric acid, and the reaction 4NO2+O2+2H2O====4HNO3 will occur, eliminating the yellow color.

2. Acid rain and its prevention and control

1.Main sources, hazards and prevention of SO2 and NO2

2.Acid rain

(1) Concept: precipitation with pH<____. Normal rainwater has a pH of approximately 5.6 due to dissolved CO2.

(2) Cause: Mainly caused by ___ and ___ in the atmosphere dissolved in water.

(3)Hazards:

① Directly damages crops, destroys forests and grasslands, and acidifies soil and lakes.

②Accelerate the corrosion of buildings, bridges, industrial equipment, transportation vehicles and cables.

Nitrogen and its compounds PPT, part 2 content: key abilities and literacy formation

Knowledge point 1: The strong oxidizing property of nitric acid

[Key points to clarify doubts]

1. Laws

(1) The greater the concentration of nitric acid, the higher the reaction temperature, and the stronger its oxidizing property.

(2) The reduction product of concentrated nitric acid is NO2, and the reduction product of dilute nitric acid is NO.

(3) Reducing agents are generally oxidized to the highest valence state.

2.Performance

(1) Reaction between nitric acid and metal

①Except for a few metals such as Au and Pt, nitric acid can oxidize almost all metals, such as 3Ag+4HNO3 (dilute)====3AgNO3+NO↑+2H2O;

② The reaction between active metal and nitric acid does not generate H2, and the concentration of nitric acid is different, and the reduction products are different;

③ Concentrated nitric acid can passivate Fe and Al at room temperature and react when heated.

(2) Reaction of nitric acid and non-metals

①Reaction rule: non-metal element + concentrated nitric acid → highest valence oxide or other

Oxygen-containing acid +NO2↑+H2O;

②Example: C+4HNO3 (concentrated) CO2↑+4NO2↑+2H2O.

【Think·Discussion】

(1) When a small amount of Fe reacts with a sufficient amount of dilute nitric acid, will Fe be oxidized to +2 or +3? What about the reaction of excess Fe with dilute nitric acid?

Tip: Nitric acid is highly oxidizing and can oxidize Fe to Fe3+, so a small amount of Fe reacts with a sufficient amount of dilute nitric acid, and Fe is oxidized to +3; since Fe can react with Fe3+ to form Fe2+, excess Fe reacts with dilute nitric acid The reaction yields +2-valent iron.

Knowledge point 2: Calculations related to the reaction between nitric acid and metals

[Key points to clarify doubts]

1. The rules of reaction between nitric acid and metals

When nitric acid reacts with metal elements, part of it is reduced and part of it generates nitrate. Therefore, nitric acid exhibits both acidity and oxidation. However, H2 is generally not generated when nitric acid reacts with metals.

(1) Reaction of nitric acid and copper:

The role of nitric acid in the reaction can be represented as follows:

③Using electron conservation and atomic conservation, we can successfully solve the relationship between the quantities of Cu and HNO3 participating in the reaction and the products NO2 and NO.

2. Commonly used calculation methods for reactions between metals and nitric acid

(1) Atomic conservation method: When HNO3 reacts with metal, the HNO3 consumed by the reaction

The amount of nitrogen atoms is equal to the sum of the amount of acidic HNO3 (existing in the form of nitrate in solution) and the amount of oxidizing HNO3 (existing in the form of NOx).

(2) Electron conservation method: The amount of matter from which nitrogen atoms gain electrons in HNO3 is equal to the amount of matter from which metal loses electrons.

(3) Charge conservation: When HNO3 is excessive, the solution after the reaction (regardless of OH-) is: c( )=c(H+)+n×c(Mn+) (Mn+ represents metal ions).

【Compensation training】

1. Zinc reacts with very dilute nitric acid to produce zinc nitrate, ammonium nitrate and water. When 1 mol of zinc nitrate is generated, the amount of reduced nitric acid is ()

A. 2 molB. 1 mol

C. 0.5 molD. 0.25 mol

[Analysis] Choose D. The equation of the reaction can be expressed as 4Zn+10HNO3 (dilute)====4Zn(NO3)2 +NH4NO3+3H2O, so the reduced nitric acid is the part that is reduced to, so 1 mol of zinc nitrate is generated, correspondingly The amount of ammonium nitrate produced is 0.25 mol, so the reduced part of nitric acid is 0.25 mol.

2. A certain amount of Cu reacts with 1 mol·L-1 of dilute nitric acid. If the concentration drops by 0.2 mol·L-1, the c(H+) in the solution will drop at the same time (assuming that the volume of the solution remains unchanged before and after the reaction) ()

A.0.2 mol·L-1 B.0.4 mol·L-1

C.0.6 mol·L-1 D.0.8 mol·L-1

3.1 L of a mixture of dilute nitric acid and dilute sulfuric acid, the substance concentrations are 0.1 mol·L-1 and 0.4 mol·L-1 respectively. If enough copper powder is added to the mixed solution, the maximum mass of copper powder that can be dissolved is ()

A.2.4 g B.3.2 g C.6.4 g D.9.6 g

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Update Time: 2024-10-02

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