How can you tell the difference between sulphur dioxide and carbon dioxide?

Method 1: Inject bromine water or acidic potassium permanganate solution to fade sulfur dioxide, and carbon dioxide instead, which is the use of sulfur dioxide's reducibility;

Method 2: Sulfur dioxide is introduced into the magenta solution to fade it, and carbon dioxide is used to make it bleach.

Sulfur dioxide is reducible, carbon dioxide is not, so this is generally used to identify, but there are other methods.

1. Acidic potassium permanganate solution, sulfur dioxide can make it fade, carbon dioxide is not 5SO2 + 2KMNO4 + 2H2O = = K2SO4 + 2MNSO4 + 2H2SO4

2. Bromine water, sulfur dioxide can make it fade, carbon dioxide does not work BR2 + SO2 + 2H2O = = 2HBR + H2SO43, hydrogen sulfide aqueous solution, sulfur dioxide will produce turbidity, and carbon dioxide will have no obvious phenomenon 2H2S + SO2 = = 2H2O + 3S

4. Magenta solution, sulfur dioxide can make it fade, but carbon dioxide cannot.

Sulfur dioxide is odorous, while carbon dioxide is odorless.

ls is wrong.

First with the clarification of lime water, become turbid before the introduction of magenta, so that it fades is sulfur dioxide, and vice versa, carbon dioxide.

(1) All are acidic oxides.

It can react with alkali or alkaline oxides, for example, it can be clear lime water to become turbid.

2) Both are oxidizing.

so₂+2h₂s=3s+2h₂o

CO +C = 2CO high temperature.

3) so is reductive.

so +br +2h o=h so +2hbr(4)so bleaching.

Comparison of the properties of oxygen and carbon dioxide.

Sulfur dioxide(Chemical formula: SO) is a gas under standard conditions and at room temperature and pressureSulphur trioxide(Chemical formula: SO) is a solid under standard conditions and a liquid at room temperature and pressure.

1.Smell: pungent sulfur dioxide, odorless carbon dioxide;

2.Solubilization: Under normal circumstances, 40 volumes of SO2 can be dissolved in 1 volume of water; Only 1 volume of CO2 can be dissolved in 1 volume of water;

3.Chemistry: SO2 is easy to liquefy, while CO2 cannot be liquefied;

4.State: When two unknown gases are placed in an environment below minus 10 degrees Celsius, sulfur dioxide becomes liquid;

5.Dense: Fill two unknown gases into an equal volume container and weigh the mass, the heavy bottle contains sulfur dioxide;

6.Color: Unknown gases are mixed with hydrogen sulfide gas, and sulfur dioxide is generated from light yellow solids;

It can react with bromine water to fade bromine water; CO2 cannot react with bromine water, nor can it fade bromine water;

8.The two gases are respectively passed into the magenta solution, so that the magenta fades sulfur dioxide and carbon dioxide does not change color;

9.Iron chloride can be added, sulfur dioxide can turn yellow to green, and carbon dioxide does not change color in the solution.

1. Sulfur dioxide is reducible, but carbon dioxide is not, so this method is generally used to identify lead.

2. Acidic potassium permanganate solution, sulfur dioxide can make it fade, carbon dioxide cannot.

The reaction formula is 5SO2+2KMno4+2H2O==K2SO4+2MNSO4+2H2SO4.

3. Bromine water and sulfur dioxide can make it fade, but carbon dioxide cannot.

Reaction equation: BR2+SO2+2H2O==2HBR+H2SO4.

4. For hydrogen sulfide aqueous solution, the introduction of sulfur dioxide will produce turbidity, and the introduction of carbon dioxide will have no obvious phenomenon.

Reaction equation: 2H2S+SO==2H2O+3S.

Carbon dioxide: Physical properties: It is a colorless and odorless gas at room temperature, slightly denser than air, soluble in water, and produces carbonic acid. Chemical properties: It can make the clarified lime water (Ca(OH)) turbid.

Oxygen: Physical properties: Density in grams and liters under standard conditions (0 and atmospheric pressure 101325 Pa).

Colorless, odorless, tasteless. It has very little solubility in water. At a pressure of 101 kPa, oxygen turns into a pale blue liquid at about -180 degrees Celsius and a snowflake-like pale blue solid at about -218 degrees Celsius.

Chemical properties: The chemical properties of oxygen are relatively reactive. In addition to rare gases and small reactive metal elements such as gold, platinum and silver, most of the elements can react with oxygen, and these reactions are called oxidation reactions, and the compounds produced by the reaction (composed of two elements, one of which is the oxygen element) are called oxides.

In general, aqueous solutions of non-metallic oxides are acidic, while alkali metals or alkaline earth metal oxides are alkaline. In addition, almost all organic compounds can violently ignite carbon dioxide and water in oxygen.