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Calcium carbonate reacts with dilute hydrochloric acid according to the equation shown.
CaCO3 + 2HCl → CaCl2 + CO₂ + H₂O
10g of calcium carbonate is reacted with 100 cm³ of 1 mol/dm³ hydrochloric acid.
mole calculation is needed
The following statements are made.
1
2
3
4
1.2 dm³ of carbon dioxide is formed.
5.6g of calcium chloride is formed.
4.8 g of carbon dioxide is formed.
No calcium carbonate is left when the reaction is completed.
Which statements about the reaction are correct?
A 1 and 2
B 1 and 4
C 2 and 3
D 3 and 4

Respuesta :

4.8 g of carbon dioxide is formed and No calcium carbonate is left when the reaction is completed statements are correct.

Calculation and Explanation :

CaCO3 has a molar mass of 40+12+316.

CaCO3 has a molar mass of 100 g/mol.

CaCl2 has a molar mass of 40 + 235.5.

CaCl2 has a molar mass of 111 g/mol.

100 g of CaCO3 and 111 g of CaCl2 are produced per mole.

Assume that x g of CaCl2 is created for every 10 g of CaCO3.

Therefore,

CO2 has a molar mass of 12 + 162.

CO2 has a molar mass of 44 g.

100 g of CaCO3 yield 44 g of CO2 per mole, or one mole.

Assume 10 g of CaCO3 results in y g of CO2.

Therefore,

y = 4.8 g 4.8 g of CO2 are created, meaning that one statement is false and three are true.

So we can say that the option D is correct . When the reaction is finished, the assertions that read "4.8 g of carbon dioxide is produced" and "No calcium carbonate is left" are true.

To know more about Calcium carbonate please click here ; https://brainly.com/question/1990063

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