I. Reaction of substances with oxygen:
(1) the reaction of simple substance with oxygen;
1. Magnesium burns in air: 2Mg+O2 ignites 2MgO.
2. Iron burns in oxygen: 3Fe+2O2 ignites Fe3O4.
3. Copper heating in air: 2Cu+O2 heating 2CuO.
4. Aluminum burns in air: 4Al+3O2 ignites 2Al2O3.
5. Combustion in hydrogen and air: 2H2+O2 ignites 2H2O.
6. Red phosphorus burns in air: 4P+5O2 ignites 2P2O5.
7. Sulfur powder burns in air: S+O2 ignites SO2.
8. Complete combustion of carbon in oxygen: C+O2 ignites CO2.
9. Incomplete combustion of carbon in oxygen: 2C+O2 ignites 2CO.
(2) the reaction of compounds with oxygen:
10. Carbon monoxide burns in oxygen: 2CO+O2 ignites 2CO2.
1 1. Methane burns in air: CH4+2O2 ignites CO2+2H2O.
12. Alcohol burns in air: C2H5OH+3O2 ignites 2CO2+3H2O.
2. Several decomposition reactions:
13. Decomposition of water under direct current: 2H2O charged 2H2 =+O2 =
14. heating basic copper carbonate: Cu2(OH)2CO3 heating 2cuo+H2O+CO2 =
15. heating potassium chlorate (containing a small amount of manganese dioxide): 2kClO3 = = = 2kCl+3o2 =
16. heating potassium permanganate: 2KMnO4 heating k2mno4+MnO2+O2 =
17. Carbonic acid is unstable and decomposed: H2CO3 === H2O+CO2↑ =
18. high temperature calcined limestone: CaCO3, high temperature CaO+CO2↑ =
Three. Several redox reactions:
19. Reduction of copper oxide by hydrogen: H2+ copper oxide heats copper +H2O.
20. Reduction of copper oxide with charcoal: 2Cu, high temperature 2Cu+CO2↑ =
2 1. Iron oxide reduction by coke: 3C+ 2Fe2O3, high temperature 4Fe+3CO2↑ =
22. Reducing Fe3O4 with coke at high temperature: 2c+Fe3O4, 3Fe+2 CO2 =
23. Reduction of copper oxide by carbon monoxide: CO+ CuO heats Cu+CO2.
24. Reduction of iron oxide by carbon monoxide: 3CO+ Fe2O3, high temperature, 2Fe+3CO2.
25. Reduction of ferroferric oxide with carbon monoxide: 4CO+ Fe3O4, high temperature 3Fe+4CO2.
4. Relationship among simple substance, oxide, acid, alkali and salt
(1) elemental metal+acid salt+hydrogen (displacement reaction)
26. Zinc and dilute sulfuric acid Zn+H2SO4 = ZnSO4+H2 Write
27. Iron and dilute sulfuric acid Fe+H2SO4 = FeSO4+H2 Write
28. magnesium and dilute sulfuric acid mg+H2SO4 = mgso4+H2 write
29. Aluminum and dilute sulfuric acid 2Al +3H2SO4 = Al2(SO4)3 +3H2↑ 3+3H2+3H2 write 3+3H2.
30. Zinc and dilute hydrochloric acid Zn+Zn+2HCl === ZnCl2+H2↑ =
3 1. Iron and dilute hydrochloric acid Fe+2 Fe+2HCl === FeCl2+H2↑ = H2 =
32. Magnesium and dilute hydrochloric acid Mg Mg+ 2HCl === MgCl2+H2↑ =
33. Aluminum and dilute hydrochloric acid 2Al+6HCl = = 2AlCl3+3H2 Write
(2) Simple metal+salt (solution)-another metal+another salt
34. The reaction between iron and copper sulfate solution: Fe+CuSO4 = = FeSO4+Cu.
35. The reaction between zinc and copper sulfate solution: Zn+CuSO4 = = ZnSO4+Cu.
36. The reaction between copper and mercury nitrate solution: Cu+Hg (NO3) 2 = = Cu (NO3) 2+Hg.
(3) Alkaline oxide+acid salt+water
37. The reaction of iron oxide with dilute hydrochloric acid: Fe2O3+6HCl === 2FeCl3+3H2O+3H2O.
38. Reaction of iron oxide with dilute sulfuric acid: Fe2O3+3H2SO4 = = Fe2 (SO4) 3+3H2O+3H2O.
39. Reaction of copper oxide with dilute hydrochloric acid: CuO+2hcl = = = CuCl2+H2O.
40. The reaction between copper oxide and dilute sulfuric acid: CuO+H2SO4 = = = CuSO4+H2O.
4 1. The reaction of magnesium oxide with dilute sulfuric acid: MgO+H2SO4 = = = MgSO4+H2O.
42. The reaction of calcium oxide with dilute hydrochloric acid: Cao+2 HCl = = = CaCl2+H2O.
(4) acidic oxide+alkaline salt+water
43. Caustic sodium will deteriorate when exposed to air: 2NaOH+CO2 ==== Na2CO3+H2O.
44. Caustic sodium absorbs sulfur dioxide gas: 2 NaOH+SO2 = = = Na2SO3+H2O.
45. Caustic sodium absorbs sulfur trioxide gas: 2NaOH+SO3 ==== Na2SO4+H2O.
46. The slaked lime deteriorates in the air: Ca (OH) 2+CO2 = = = CaCO3 ↓+H2O+H2O.
47. The slaked lime absorbs sulfur dioxide: ca (oh) 2+SO2 = = = caso3 ↓+H2O+H2O.
(5) acid+alkali-salt+water
48. Reaction of hydrochloric acid with caustic soda: HCl+NaOH = = = NaCl+H2O.
49. Reaction of hydrochloric acid and potassium hydroxide: HCl+KOH = = = KCl+H2O.
50. The reaction between hydrochloric acid and copper hydroxide: 2HCl+Cu (OH) 2 = = CuCl2+2H2O.
5 1. The reaction between hydrochloric acid and calcium hydroxide: 2hcl+Ca (OH) 2 = = CaCl2+2h2o.
52. The reaction between hydrochloric acid and iron hydroxide: 3HCl+Fe (OH) 3 = = = FeCl 3+3H2O.
53. Aluminum hydroxide for the treatment of hyperacidity: 3HCl+Al (OH) 3 = = = AlCl3+3H2O.
54. Reaction between sulfuric acid and caustic soda: H2SO4+2NaOH = = = Na2SO4+2H2O.
55. The reaction between sulfuric acid and potassium hydroxide: H2SO4+2koh = = = K2SO4+2h2o.
56. The reaction between sulfuric acid and copper hydroxide: H2SO4+Cu (OH) 2 = = CuSO4+2H2O.
57. The reaction between sulfuric acid and iron hydroxide: 3H2SO4+2Fe (OH) 3 = = Fe2 (SO4) 3+6H2O.
58. The reaction between nitric acid and caustic soda: nitric acid+sodium hydroxide = = = sodium nitrite+H2O H2O.
(6) acid+salt-another acid+,another salt
59. marble reacts with dilute hydrochloric acid: CaCO3+2hcl = = CaCl2+H2O+CO2 =
60. Sodium carbonate reacts with dilute hydrochloric acid: Na2CO3+2HCl = = 2NaCl+H2O+CO2 =
6 1. Reaction of magnesium carbonate with dilute hydrochloric acid: MgCO3+2HCl = = MgCl2+H2O+CO2 =
62. Reaction between hydrochloric acid and silver nitrate solution: HCl+AgNO3 === AgCl↓+HNO3.
63. The reaction of sulfuric acid and sodium carbonate: Na2CO3+H2SO4 = = Na2SO4+H2O+CO2 =
64. The reaction between sulfuric acid and barium chloride solution: H2SO4+bacl2 = = = baso4 ↓+2hcl.
(7) alkali+salt-another alkali+another salt
65. Sodium hydroxide and copper sulfate: 2 NaOH+CuSO4 = = Cu (OH) 2 ↓+Na2SO4.
66. Sodium hydroxide and ferric chloride: 3 NaOH+FeCl 3 = = Fe (OH) 3 ↓+3 NaCl.
67. Sodium hydroxide and magnesium chloride: 2 NaOH+MgCl2 = = mg (OH) 2 ↓+2 NaCl.
68. Sodium hydroxide and copper chloride: 2 NaOH+CuCl2 = = Cu (OH) 2 ↓+2 NaCl.
69. Calcium hydroxide and sodium carbonate: Ca (OH) 2+Na2CO3 = = CaCO3 ↓+2NaOH.
(8) salt+salt-two new salts
70. Sodium chloride solution and silver nitrate solution: NaCl+AgNO3 = = = AgCl ↓+Nano3.
7 1. sodium sulfate and barium chloride: Na2SO4+bacl2 = = = baso4 ↓+2 NaCl.
Verb (short for verb) Other reactions:
72. Carbon dioxide is soluble in water: CO2+H2O === H2CO3.
73. Quicklime is soluble in water: CaO+H2O === Ca(OH)2.
74. Sodium oxide is soluble in water: Na2O+H2O = = = 2 NaOH.
75. Sulfur trioxide is soluble in water: SO3+H2O = = = H2SO4.
76. Copper sulfate crystal is decomposed by heating: CuSO4 5H2O heats CuSO4+5H2O.
77. Anhydrous copper sulfate as desiccant: cuso 4+5H2O = = = = cuso 4·5H2O.
Computational problem
There are 4g limestone samples. Now, 40g of dilute hydrochloric acid is added in four times, and after fully reflecting each time, the quality of solid residue is weighed after filtering, drying and other operations. (After the first addition of 10g, the remaining solid mass is 3.0g; after the second addition of 10g, the remaining solid mass is 2.0g; after the third addition of 10g, the remaining solid mass is1.0g; After the fourth addition of 10g, the remaining solid mass was 0.4g).
If the quality of impurity-containing quicklime produced by calcining the above limestone raw materials is 100T, how many tons of limestone raw materials are needed?
Suppose the quality of limestone raw material is y.
CaCO3 CaO+CO2↑
100 56
y×90% ( 100-y× 10%)
100:56 = 90% y:( 100-y× 10%)
y= 165.6 t
Pig iron and steel are both ferroalloys. The carbon content of pig iron is between 2.0% and 4.3%, and that of steel is between 0.03% and 2%. Put a piece of iron alloy with the mass of 10.0g into the conical flask, and then add 100g dilute H2SO4 into the conical flask, just to completely react the iron in the iron alloy (carbon is insoluble in dilute sulfuric acid; The content of other elements in ferroalloy is very low, which can be ignored), and the volume of generated H2 is 4.00 L (the density of H2 is 0.0880g/L under this condition). Try to answer according to the calculation: (the calculation result keeps three digits)
(! ) Is this ferroalloy pig iron or steel?
(2) Solute mass fraction of the solution obtained after the reaction.
(1) solution: let the mass of iron in this ferroalloy be x.
(H2)= 4.00 0.0880g/L = 0.352g.
Fe+H2SO4====FeSO4+H2↑
56 2
X 0.352g gram
X =(56×0.352)/2 = 9.856g.
The mass fraction of carbon in this ferroalloy is (10.0g-9.856g)/10.0g×100% =1.44%.
0.03%-2.0%, and the iron alloy is steel.
(2) solution: let the mass in the solution obtained after the reaction be y.
Iron+sulfuric acid = = ferrous sulfate+H2 =
152 2
Y0.352g.
y=( 152×0.352g)/2=26.75g
The mass fraction of ferrous sulfate is:
26.75g/(100g+9.856g-0.352g) × 100%=24.4%.
8.(6 points) Solution: (1) According to the meaning of the question, let the mass of generated NaOH be X.
Na2O+H2O==2NaOH
62 80
3. 1 g x
62:80=3. 1g:x x=4g
4g/(3. 1g+m)= 16% m = 2 1.9g
How many tons of carbon dioxide are produced by calcining limestone 100t containing 80% calcium carbonate? If all the impurities in limestone enter the quicklime, how many tons of such quicklime can be obtained?
Coal is an important chemical raw material. Using coal as fuel is not only a great waste, but also because coal contains sulfur, the sulfur dioxide produced after combustion will cause air pollution. A factory uses coal as fuel and burns 4.8× 103kg of coal containing 2% sulfur every day.
(1) Try to calculate how many kilograms of sulfur dioxide the factory releases into the air every day. (The calculation result is reserved to one decimal place, the same below)
(2) The content of sulfur dioxide in the waste gas of this factory can be determined according to the following reaction: SO2+2h2o = H2SO4+2hi. Now, 500mL of waste gas samples are taken from this factory, and the iodine solution containing 4× 10-7g of iodine just completely reacts with sulfur dioxide in the waste gas. Try to calculate whether the waste gas discharged by this factory meets the national industrial waste gas emission standard (the sulfur dioxide content in the waste gas shall not exceed 0. 15mg/m3) (relative atomic mass: H- 1, O-66).
Solution: The mass of sulfur in coal burned every day: 4.8× 103× 2% = 96 ×.
The mass of SO2 produced is 96× =192×.
Let the mass of the complete reaction of SO2 with 4× 10-7g iodine be X.
SO2+2H2O+I2=H2SO4+2HI
64 254
X4×10-7g
= x= 1.0× 10-7g
∴ SO2 content in waste gas:1.0×10-7g/500ml = 0.2mg/m3 > 0.15mg/m3.
The waste gas emitted by this factory does not meet the national industrial waste gas emission standards.
When the gas flow of CO is heated by a gCuO, CuO is partially reduced, and the total mass of solid matter is called b g, while the mass of CO2 produced is called dg. It is known that the relative atomic mass of oxygen is 16, and the relative atomic mass of carbon is expressed by mathematical formula.
Analysis: let the relative atomic mass of carbon be X.
80 64 (x+32)
dg (a-b)g
(x+32)∶d= 16∶(a-b)