 # How many grams of carbon dioxide are prepared by fully reacting 100g limestone containing 80% calcium carbonate with 100g dilute hydrochloric acid (assuming that all calcium carbonate react) 1? What is the mass fraction of the solute of the dilute hydrochloric acid

## How many grams of carbon dioxide are prepared by fully reacting 100g limestone containing 80% calcium carbonate with 100g dilute hydrochloric acid (assuming that all calcium carbonate react) 1? What is the mass fraction of the solute of the dilute hydrochloric acid

Because it is assumed that all calcium carbonate reacts, hydrochloric acid is sufficient, and the concentration does not need to be considered
CaCO3+2HCl=CaCl2+H2O+CO2
44 g CO2 per 100 g calcium carbonate
100 * 80% * (44 / 100) = 35.2G

### 10g limestone reacts exactly with 100g hydrochloric acid to produce CO2 with a mass of 2.2g. Calculate: (1) Calculate the mass fraction of CaCO3 in limestone; (2) What is the mass fraction of solute in the solution obtained after the reaction?

(1) Let the mass of calcium carbonate be x and the mass of calcium chloride be y. CaCO3 + 2HCl = CaCl2 + H2O + CO2 ↑        one hundred         one hundred and eleven        forty-four   x&nb...

### 12g limestone completely reacts with 100g dilute hydrochloric acid. The total mass of the remaining material is 107.6g. What is the mass of calcium carbonate? Dilute hydrochloric acid with a certain mass fraction, and limestone contains impurities However, the dilute hydrochloric acid reaction should not be 100. The dilute hydrochloric acid is a certain mass fraction, which is what I doubt

CaCO3 + 2HCl = CaCl2 + H2O + CO2
one hundred point four four
x.100g+12g-107.6g=4.4g
x/4.4g = 100/44
x = 10g
Participate in reflecting the quality of calcium carbonate 10g

### There are impurities in a batch of limestone. Take 4 g of this limestone sample and add 40 g of dilute hydrochloric acid with unknown solute mass fraction four times Add 10g of residual solid for the first time, 2G of residual solid for the second time, 1g of residual solid for the third time, and 0.4g of residual solid for the fourth time. Calculate the purity of the limestone sample? Find the mass fraction of solute in hydrochloric acid? Please answer quickly

When 10g of residual solid is added for the first time, it means that 10g of hydrochloric acid solution can exactly react with 1g of calcium carbonate. Similarly, the second and third times, but by the fourth time, the residual solid is only 0.4g, indicating that this 0.4g is an impurity that cannot react with hydrochloric acid. Therefore, the purity of limestone sample = (4-0.4) / 4 = 90% from the first time or the third time

### In the laboratory, limestone reacts with dilute hydrochloric acid to produce carbon dioxide   G carbon dioxide, how many grams of hydrochloric acid with 10% mass fraction of solute?

Let the mass of solute in hydrochloric acid used be X
CaCO3+2HCl=CaCl2+H2O+CO2↑
seventy-three             forty-four
x               4.4g
seventy-three
44=x
4.4g，x=7.3g
The mass of hydrochloric acid used is 7.3g ÷ 10% = 73g
Answer: 73g hydrochloric acid with 10% mass fraction of solute is required

### 25g limestone containing 20% impurities reacts exactly with 100g dilute hydrochloric acid with a certain solute mass fraction (impurities do not react with acid). Calculate the mass fraction of solute in this dilute hydrochloric acid

Let the mass of HCl consumed in the reaction of calcium carbonate and hydrochloric acid be X
The mass of calcium carbonate is (1-20%) × 25g=20g
CaCO3+2HCl=CaCl2+H2O+CO2↑
one hundred     seventy-three
20g      x
one hundred
73=20g
x
x=14.6g；
So the mass of hydrogen chloride in the reaction is 14.6g,
Mass fraction of hydrochloric acid: 14.6g
100g × 100%=14.6g
A: the mass fraction of solute in this dilute hydrochloric acid is 14.6%