高中化学方程式默写(High school chemistry equation dictation)

高中化学方程式默写（

High

school

chemistry

equation

dictation

）

Write the following reaction (the chemical formula is ion

reaction to write ion equation)

1. sodium combustion in oxygen:

2. sodium and oxygen at room temperature reaction

3. sodium and water reaction

4. sodium and water reaction

6. reaction between sodium peroxide and water

The reaction between sodium peroxide and 7. carbon dioxide

8. sodium carbonate and hydrochloric acid

9. sodium bicarbonate reacts with hydrochloric acid

The reaction of 10. sodium bicarbonate and sodium hydroxide

The thermal decomposition of 11. sodium bicarbonate

12. carbon dioxide into sodium carbonate solution

13. calcium carbonate with hydrochloric acid

14. sodium bicarbonate and excess calcium hydroxide

A

small

amount

of

15.

sodium

bicarbonate

and

calcium

hydroxide

16.

sodium

hydroxide

pass

into

a

small

amount

of

carbon

dioxide

gas

Sodium hydroxide with carbon dioxide gas excess

17. calcium hydroxide solution with carbon dioxide gas excess

18. the addition of excessive calcium hydroxide

19. the addition of excessive calcium hydroxide

20. Laboratory of chlorine

21. hydrochloric acid with Potassium Permanganate

22. chlorine reacts with water

23. fluorine gas and water reaction

24. industry for bleaching powder (or bleach)

25. chlorine reacts with sodium hydroxide solution

26. chlorine and iron reaction

27. reaction of chlorine and copper

The reaction of chlorine and sodium 28.

29. reaction of chlorine and sodium bromide

30. chlorine and hydrogen iodide reaction

31. bromine reacts with potassium iodide

32. see the light decomposition of silver bromide

33.

under

high

temperature,

iron

oxide

and

carbon

monoxide

gas

reaction

34. sulfur and copper heating reaction

35. sulfur and iron heating reaction

36. hydrogen peroxide and manganese dioxide for oxygen

Destroy 37. ozone layer

38. sulfur dioxide reacts with hydrogen sulfide

39. halogenelemental solution X2 (X = Cl, Br, I) in the SO2

41. chlorine and sodium sulfite solution reaction

The reaction of 42. copper and concentrated sulfuric acid

Reaction of 43. carbon and concentrated sulfuric acid

44. sulfur dioxide three sulfur dioxide

Three sulfur dioxide reacts with water

Reaction

of

45.

hydrogen

sulfide

and

concentrated

sulfuric

acid

46. silicon reacts with sodium hydroxide solution

47. silica and carbon reaction

Reaction of 48. silica and sodium hydroxide,

49. silica and calcium carbonate reaction

50. SiO2 reacted with hydrofluoric acid

Preparation method of ammonia industry 51:

52.

in

the

discharge

conditions

of

nitrogen

and

oxygen

reaction

53. gas nitric oxide meets the air become red brown:

2 + O2 + H2O = HNO3

+ O2 + H2O = HNO3

56.P+ O2

57.P2O5+ H2O H3PO4

58.P+ Cl2 (lack of)

59.P+ Cl2 (enough)

60. reasons of ammonia dissolution in water alkaline:

3? H2O is not stable, heat decomposition:

62. be dipped in concentrated ammonia water with hydrochloric

acid

to

get

the

glass

rod

and

the

glass

rod

close

to

each

other,

resulting in a large number of white smoke:

63. the catalytic oxidation of ammonia:

64. NH4Cl crystal heating tube in the tube wall of the upper

end

of

a

white

solid

attachment,

this

process

is

the

reaction:

The thermal decomposition reaction of 4HCO3:

66. (NH4) 2SO4 and NH4NO3 solid solid reaction, respectively

with NaOH heating:

The

reaction

principle

of

67.

laboratory

production

of

ammonia:

The 68. reason is the concentrated nitric acid yellow:

69. copper and dilute nitric acid reaction,

Release

the

colorless

gas,

when

exposed

to

air,

gas

became red

brown, write the reaction in the process of occurrence:

70. charcoal and concentrated nitric acid reaction:

71. CO2 will pass into the lime water, the first white

precipitate, with CO2 to pass into the white precipitate,

disappear,

please

write

the

chemical

formula

in

the

process

of

occurrence:

72. iron oxide reduced by CO:

Use the yellow iron ore industry 73. (mostly FeS2) to produce

sulfuric acid, the main reaction:

74. NO2 gas compressed gas, found pale:

75. write the following electrolyte ionization equation:

1. CH3COOH:

The NH3 H2O?:

The H3PO4:

The Mg (OH) 2:

The ionization NaHSO4 in the molten state:

The ionization in water NaHSO4:

The alum water soluble ionization:

76.

write

the

following

the

salt

hydrolysis

reaction

equation:

1. NH4NO3:

Na2S:

The Fe2 (SO4) 3:

2CO3 dissolution in water alkaline (represented by ion

equation):

78.

alum

and

FeCl3

can

be

used

as

purifying

agent

(represented

by ion equation):

79. foam containing Al2 (SO4) 3 and NaHCO3 solution, the use

of ionic reaction equations:

In 80. NH4Cl solution was added into magnesium will produce

bubbles (represented by ion equation):

81. soda solution by adding hydrochloric acid to excess

(represented by the ion equation):

The chemical formula 82. mg and CO2 reaction:

83. laboratories from Al (OH) 3 ionic reaction equation:

The 84. AlCl3 solution into ions in the solution of NaOH

equation:

The 85. NaOH solution was added drop wise AlCl3 solution to

excess (represented by the ion equation):

2O3 dissolved in NaOH solution (expressed by ion

equation):

87. the excess CO2 into sodium aluminate solution (by ion

equation):

88. CO2 into sodium aluminate solution in excess of

(represented by the ion equation):

89. drops of hydrochloric acid sodium metaaluminate solution

to excess (represented by the ion equation):

90. nitrogen and magnesium reaction:

91. the excess iron and iron deficiency and ionic equation of

dilute nitric acid reaction:

Iron overload:

Iron deficiency:

92. heating in air FeO:

93. put the Fe2O3 into the ion equation in hydrochloric acid:

94. laboratories from Fe (OH) 2, observed a white precipitate

produced, but

precipitation immediately

turns

gray

green,

and

finally

changed

to

red

brown,

write

about

the

chemical

equation

of this process:

3 solution mixed with ammonia ion equation:

Write the following 96. aluminothermic reaction: