 # The experiment requires 13.2 grams of carbon dioxide, which is prepared by the reaction of calcium carbonate and sufficient dilute hydrochloric acid. How much calcium carbonate is needed

## The experiment requires 13.2 grams of carbon dioxide, which is prepared by the reaction of calcium carbonate and sufficient dilute hydrochloric acid. How much calcium carbonate is needed

CaCO3+2HCl=CaCl2+H2O+CO2↑
44gco2 was obtained by the reaction of 100gcaco3
Now 13.2gco2 is required, so CaCO3 13.2 / 44 * 100 = 30g

### 10 grams of calcium carbonate and 100 grams of dilute hydrochloric acid react exactly. 1. How many grams of carbon dioxide gas are produced after the complete reaction? 2. What is the mass fraction of dilute hydrochloric acid

CaCO3+2HCl=CaCl2+H2O+CO2
100 73 44
10g x y
100/10g=73/x=44/y
x=7.3g y=4.4g
1. 4.4 g of carbon dioxide gas is produced after complete reaction
2. The mass fraction of dilute hydrochloric acid is 7.3g/100g * 100% = 7.3%

### Put a certain amount of calcium carbonate into 50g of dilute hydrochloric acid and the reaction is just complete Put a certain amount of calcium carbonate into 50g of a dilute hydrochloric acid, and the reaction is just complete. A total of 4.4g of carbon dioxide is collected to obtain 1. Mass fraction of solute in dilute hydrochloric acid 2. Mass fraction of solute in the solution after reaction It's better to complete the steps

If x g of hydrochloric acid is set. CaCO3 + 2HCl = CaCl2 + H2O + co273 44x 4.4 is 73 / x = 44 / 4.4, x = 7.3, then the mass fraction of hydrochloric acid in the total dilute hydrochloric acid solution is 7.3 / 50 * 100% = 14.6% (the mass fraction of dilute hydrochloric acid is 50 g, and hydrochloric acid accounts for 7.3 G!) PS: hydrochloric acid dissolved in water is dilute hydrochloric acid, which are different! As for the reaction

### How much carbon dioxide is produced by the complete reaction of marble containing 50 grams of calcium carbonate with 100 grams of dilute hydrochloric acid? What is the mass fraction of solute in this dilute hydrochloric acid Another is to put 12.5 g of limestone into 36.5 g of dilute hydrochloric acid, just complete the reaction, and release 4.4 g of carbon dioxide gas to calculate the mass fraction of CaCO 3 in limestone? Mass fraction of original dilute hydrochloric acid? Mass fraction of solute in calcium chloride solution obtained after complete reaction?

Suppose the mass of calcium carbonate in limestone is x, the mass of calcium chloride is y, and the mass of solute in dilute hydrochloric acid is Z
CaCO3 +2HCl=CaCl2+CO2↑+H2O
100 73 111 44
x z y 4.4g
x=10g y=11.1g z=7.3g
(1) The mass fraction of calcium carbonate in limestone is:
10/12.5 × 100%=80%
(2) The mass fraction of solute in dilute hydrochloric acid is:
7.3/ 36.5 × 100%═20%
(3) The mass of the solution after reaction is 10g + 36.5g-4.4g = 42.1g
The mass fraction of solute in the solution after reaction is:
11.1/42.1g × 100%=26.4%

### 12g limestone and 50g dilute hydrochloric acid just completely react to generate 4.4g carbon dioxide. Try to calculate the mass fraction of solute in dilute hydrochloric acid Help respondents give accurate answers The answer is 14.6%

From 4.4g of carbon dioxide, it can be known that there is 0.1mol of carbonic acid in total, so h is 0.2mol. Due to the complete reaction, it is obtained that HCl is 0.2mol, 0.2 times 36.5 is 7.3,7.3/50 × 100%=14.6%
CaCO3+2HCL=CaCl2+CO2↑+H2O
73 44
x 4.4g
73/x=44/4.4g
x=7.3
7.3/50 × 100%=14.6%
With this answer, there is no problem with the explanation and calculation process according to the examination requirements. The above is a simple calculation method, which is applicable to the solution of all types of scores. The following is a traditional calculation, which is only applicable to quality scores. Pick it yourself

### Preparation of CO2 gas from limestone and dilute hydrochloric acid

CaCO3 + 2HCl === CaCl2 + CO2 + H2O