What is the number of moles of calcium chloride that can be obtained from 25g of limestone CaCO3 in the presence of excess dilute hydrochloride acid according to the following equation
CaCO3 —> CaCL2+H2O+CO2
To determine the number of moles of calcium chloride that can be obtained from 25g of limestone (CaCO3), we need to use the molar mass of CaCO3.
Molar mass of CaCO3:
= (40.08 g/mol for Ca) + (12.01 g/mol for C) + (3 x 16.00 g/mol for O)
= 100.09 g/mol
Now we need to calculate the number of moles of CaCO3 using the given mass:
Number of moles = mass / molar mass
Number of moles of CaCO3 = 25g / 100.09 g/mol
= 0.2498 moles (rounded to 4 decimal places)
From the balanced chemical equation, we can see that 1 mole of CaCO3 forms 1 mole of CaCl2. Therefore, the number of moles of CaCl2 that can be obtained from 0.2498 moles of CaCO3 is also 0.2498 moles.
To find the number of moles of calcium chloride that can be obtained from 25g of limestone (CaCO3), we need to follow these steps:
Step 1: Calculate the molar mass of CaCO3
The molar mass of calcium carbonate (CaCO3) can be found by adding up the atomic masses of each element:
Molar mass of Ca = 40.08 g/mol
Molar mass of C = 12.01 g/mol
Molar mass of O = 16.00 g/mol
Molar mass of CaCO3 = (1 × 40.08) + (1 × 12.01) + (3 × 16.00) = 100.09 g/mol
Step 2: Convert the given mass of limestone into moles
To convert grams into moles, divide the given mass of limestone by its molar mass:
Moles of CaCO3 = Mass of CaCO3 / Molar mass of CaCO3
Moles of CaCO3 = 25 g / 100.09 g/mol
Moles of CaCO3 = 0.2499 mol (approximately 0.25 mol)
Step 3: Determine the stoichiometry of the balanced equation
According to the balanced equation, the molar ratio between CaCO3 and CaCl2 is 1:1. This means that for every 1 mole of CaCO3, 1 mole of CaCl2 is produced.
Step 4: Calculate the number of moles of CaCl2 obtained
Since the stoichiometry of CaCO3 to CaCl2 is 1:1, the number of moles of CaCl2 produced is the same as the number of moles of CaCO3:
Moles of CaCl2 = Moles of CaCO3 = 0.25 mol
Therefore, the number of moles of calcium chloride that can be obtained from 25g of limestone CaCO3 is 0.25 moles.
To determine the number of moles of calcium chloride (CaCl2) that can be obtained from 25g of limestone (CaCO3), we need to follow these steps:
1. Find the molar mass of CaCO3:
- The atomic mass of calcium (Ca) is 40.08 g/mol.
- The atomic mass of carbon (C) is 12.01 g/mol.
- The atomic mass of oxygen (O) is 16.00 g/mol.
- The molar mass of CaCO3 is calculated as:
Molar mass of CaCO3 = (40.08 g/mol) + (12.01 g/mol) + (3 * 16.00 g/mol) = 100.09 g/mol.
2. Calculate the number of moles of CaCO3:
- We can use the equation:
Moles = Mass / Molar mass.
- Given that the mass of CaCO3 is 25g, we can calculate the number of moles as:
Moles of CaCO3 = 25g / 100.09 g/mol.
3. Use the stoichiometry of the balanced chemical equation to determine the number of moles of CaCl2.
- From the balanced equation, we see that 1 mole of CaCO3 produces 1 mole of CaCl2.
- Therefore, the number of moles of CaCl2 will be the same as the number of moles of CaCO3.
As a result, the number of moles of calcium chloride that can be obtained from 25g of limestone CaCO3 is calculated by dividing the mass of CaCO3 by its molar mass, which gives an answer in moles. Since the stoichiometry of the balanced equation is 1:1 between CaCO3 and CaCl2, the number of moles of CaCl2 will also be equal to the number of moles of CaCO3.