What is the effect of calcium hydroxide solution in the experiment of reducing copper oxide to coppe

Junior Chemistry - Carbon Reduction Copper Oxide.

1.These two anti-uphescent conditions are different, the former is heating, and the latter is high temperature.

2 The latter is a displacement reaction.

3.The experimental procedure is different, the former: carbon monoxide needs to be passed for a while.

In order to remove the air from the glass tube first and prevent the carbon monoxide from mixing with the air**, pass the carbon monoxide for a while before heating. At the end of the day, remove the alcohol lamp.

Continue to pass the carbon monoxide for a while until the glass tube has cooled. It is also important to note that the gas introduced here must be disposed of and collected with a light or a small balloon.

the latter, in connection with clarified lime water.

After the end, remove the alcohol lamp to prevent gasping and bursting the test tube, and after the end, you must wait for the glass tube to cool down before taking out the copper to prevent oxidation.

CuO+Co==CO2+Cu According to the reaction equation, 1molCuo reacts to generate 1molCu, and 80 648 x reacts to find x=

If the CO is insufficient, to remove CuO, you can add a sufficient amount of dilute hydrochloric acid, and filter it to obtain Cu after full reaction, and the reaction equation: CuO+2HCl===CuCl2+H2O

cu===64/80*8== g

Sufficient amount of sulfuric acid or hydrochloric acid, filtered.

H2SO4 +CuO==CuSO4 +H2O (or HCl 2HCl +CuO ==CuCl2 +H2O).

co+cuo=cu+co2

Therefore, to make grams of copper (moles) to mole copper oxide, that is, 4 grams.

CO2 mass =

Volume = 2(1) grams.

2) CO2 = moles.

So calcium carbonate is also molar.

Mass Score =

Because calcium hydroxide is a base, it can only react with non-metallic oxides and not with copper oxide.

Introduction: Alkali: The anions formed during ionization are all compounds of hydroxide ions.

General properties of alkali: 1. Alkali solution can interact with acid-base indicators.

The alkali solution turns blue when it encounters purple litmus solution (the phenomenon is not obvious, but there is a change), and it turns red when it encounters a colorless phenolphthalein solution (the phenomenon is obvious).

2. Alkali energy reacts with non-metallic elements

The disproportionation reaction of chlorine gas with alkali, such as:

Cl2+2NaOH = NaCl+Naclo+H2O (Br2, I2 are similar).

The disproportionation reaction of sulfur with alkalis, such as:

3s+6naoh=na2so3+2na2s+3h2o

Reaction of silicon with bases, such as:

si+2naoh+h2o=na2sio3+2h2↑

3. Alkali can react with acid to produce salt and water (this kind of reaction is usually called neutralization reaction, and this kind of reaction releases a lot of heat h=

For example, hydrated lime (calcium hydroxide) is commonly used in industry to neutralize wastewater containing excessive sulfuric acid.

ca(oh)2+h2so4=caso4+2h2o

4. The alkali solution can react with acidic oxides to generate salt and water.

For example, the most common reaction of this type is the reaction of carbon dioxide in the laboratory to test with clarified lime water, but this type of reaction is not a metathesis reaction.

co2+ca(oh)2==caco3↓+h2o

In addition, there are: 2naoh+so2==na2so3+h2o

This reaction does not conform to the exchange of components between two ionic compounds, so it is not a metathesis reaction.

5. The alkali solution (relatively strong alkali) can react with salt to generate neoalkali (relatively weak alkali) and new salt.

For example, this kind of reaction is common in the preparation of sodium hydroxide in the laboratory, and the reaction between alkali and salt has two requirements, one requires that the alkali and salt involved in the reaction be soluble in water, and the other requires that there is precipitation, gas or water in the product.

ca(oh)2+na2co3=caco3↓+2naoh

(1) Because CO gas and air may be mixed with air during heating, therefore, all the air in the glass tube should be discharged before heating, so the air in the CO discharge tube should be introduced first and then heated during operation;

Therefore, the answer is: remove the air in the glass tube to prevent heating**;

2) At a, the black copper oxide reacts with CO to form red metallic copper and produces gas carbon dioxide, so the black solid can be observed here to turn red;

So the answer is: the black solid gradually turns into a red solid; co+cuo?cu+co2；

At b, the carbon dioxide generated by the reaction of the previous device passes into the clarified lime water to generate calcium carbonate precipitation and water, so it can be observed that the clarified lime water becomes turbid;

Therefore, the answer is: lime water becomes turbid; co2+ca（oh）2=caco3↓+h2o；

At C, the unreacted CO is ignited to form carbon dioxide, and the CO burns to produce a blue flame;

Therefore, the answer is: the exhaust gas burns and emits a blue flame; 2co+o2

Ignite2co2；

Use alcohol lamps to burn toxic gas CO in the exhaust gas into carbon dioxide to prevent the exhaust gas from polluting the air;

So the answer is: eliminate pollution

Junior Chemistry - Carbon Reduction Copper Oxide.

The phenomenon is that the color of copper oxide becomes the color of copper. Up to the experimental arrangement is followed by a clarified lime water bottle. CO will not be turbid, and the verification edge will be turbid as CO2.

The application just tells you that the co is reductive, and the others are almost none.

The reaction is simple.

co+cuo=cu+co2

This is a very typical reduction reaction, maybe in ancient times there would be no electrolytic copper method, copper smelters are charcoal and copper oxide together to heat to get copper, is to use the above reaction.

It is more practical to use CO to reduce iron oxide in industry, but the high temperature is not suitable for laboratory operation, so copper is used as a substitute for teaching.

Junior Chemistry - Carbon Monoxide Reduction Copper Oxide.

1. Pass carbon oxide for a while (it is best to pass nitrogen for a while and then carbon monoxide), and collect tail gas while passing carbon monoxide.

2. Light the alcohol lamp to heat the copper oxide.

3. When the copper oxide turns from black to red, stop heating and continue to pass carbon monoxide.

4. The test tube is cooled to room temperature and the carbon monoxide can be stopped.

Junior Chemistry - Carbon Monoxide Reduction Copper Oxide.

This is a matter of reaction uniformity. In other words, some solids are exposed to carbon monoxide.

gas, reacted; Some have little contact and incomplete reactions; The letter ruler was not touched at all, and there was no response. The liquid reaction is relatively uniform. For example, ferric chloride.

Reaction with copper element: With only a little iron ion, there will be no copper left, and they will continue to react. But the reaction of the gas with the solid is likely to be uneven. That is, if there is copper, there may still be copper oxide.

If it exists, it is not necessary that all copper oxide has been reduced to slippery copper oxide.

Therefore, the possible combinations are: 1. Complete reaction, all copper element. 2. It is completely unreacted, all copper oxide.

3. The reaction is incomplete, according to the degree of reaction, copper oxide and copper each account for a part, and cuprous oxide only accounts for a small part. 4. The reaction was carried out only a little, only a small amount of cuprous oxide and copper oxide. 5. The reaction is carried out relatively slowly, most of the cuprous oxide, copper oxide and cuprous oxide are very few.

6. The reaction is carried out thoroughly, most of the copper, only a small part of oxygen-trapped cuprous spike, and almost no copper oxide.