A 0.5215 gram sample of CaCO3 is dissolved in 12M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask.
How many moles of CaCO3 are used?
grams/molar mass = moles. How many moles "were used" I don't know? How many mL did you use of the 250.
Moles used = moles in flask x (mL used/250) = ??
What mass of natural gas {\rm{(CH}}_4 ) must you burn to emit 271 kJ of heat?
To calculate the number of moles of CaCO3 used, you need to use its molar mass and the mass of the sample provided. Here's how you can calculate it step by step:
1. Determine the molar mass of CaCO3:
- Calcium (Ca) has a molar mass of 40.08 g/mol.
- Carbon (C) has a molar mass of 12.01 g/mol.
- Oxygen (O) has a molar mass of 16.00 g/mol.
- So, the molar mass of CaCO3 = (1 × 40.08 g/mol) + (1 × 12.01 g/mol) + (3 × 16.00 g/mol) = 100.09 g/mol.
2. Calculate the moles of CaCO3 used:
- Given mass of CaCO3 = 0.5215 g.
- Moles of CaCO3 = mass of CaCO3 / molar mass of CaCO3.
- Moles of CaCO3 = 0.5215 g / 100.09 g/mol.
3. Calculate the moles of CaCO3 used in the experiment.
Now you can do the calculations:
Moles of CaCO3 = 0.5215 g / 100.09 g/mol = 0.005213 mol
So, 0.005213 moles of CaCO3 are used in the experiment.