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The reaction between calcium carbonate [tex]$\left( CaCO_3 \right)$[/tex] and hydrochloric acid [tex]$(HCl)$[/tex] is represented by the balanced chemical equation below:

[tex]\[ CaCO_3(s) + 2HCl(aq) \rightarrow CaCl_2(aq) + CO_2(g) + H_2O(\ell) \][/tex]

50 grams of calcium carbonate reacts completely to form 0.5 moles of carbon dioxide [tex]$\left( CO_2 \right)$[/tex] at STP.

6.1 Determine the:
6.1.1 Molar mass of calcium carbonate



Answer :

GinnyAnswer
Sure, let's determine the molar mass of calcium carbonate [tex]\((CaCO_3)\)[/tex].

To solve for the molar mass, we need to sum up the atomic masses of all the atoms in the compound:

1. Identify the atomic masses:
- Calcium (Ca): 40.08 g/mol
- Carbon (C): 12.01 g/mol
- Oxygen (O): 16.00 g/mol

2. Count the number of each type of atom in the formula [tex]\(CaCO_3\)[/tex]:
- There is 1 atom of Calcium (Ca).
- There is 1 atom of Carbon (C).
- There are 3 atoms of Oxygen (O).

3. Multiply the atomic masses by the number of each type of atom in the compound and sum them up:
- Contribution from Calcium: [tex]\(1 \times 40.08 = 40.08\)[/tex] g/mol
- Contribution from Carbon: [tex]\(1 \times 12.01 = 12.01\)[/tex] g/mol
- Contribution from Oxygen: [tex]\(3 \times 16.00 = 48.00\)[/tex] g/mol

4. Add these contributions together to get the molar mass of [tex]\(CaCO_3\)[/tex]:
[tex]\[ 40.08 \text{ g/mol (from Ca)} + 12.01 \text{ g/mol (from C)} + 48.00 \text{ g/mol (from O)} = 100.09 \text{ g/mol} \][/tex]

Thus, the molar mass of calcium carbonate [tex]\((CaCO_3)\)[/tex] is 100.09 g/mol.

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