416g of an anhydrous Bacl2 were obtained when 488g of hydrated salt were heated.calculate x in the formula:Bacl2.xH2O
g H2O = 488 - 416 = 72
mols BaCl2 = 416/molar mass BaCl2 = approx 2
mols H2O = 72/18 = approx 4
Reduce to lowest terms.
BaCl2.2H2O
I need help
To calculate the value of x in the formula BaCl2.xH2O, we need to determine the number of moles of water lost during the heating process.
1. Calculate the number of moles of BaCl2:
- Convert the mass of anhydrous BaCl2 to moles by dividing by its molar mass.
- The molar mass of BaCl2 is calculated as:
(Ba atomic mass) + 2*(Cl atomic mass)
= (137.33 g/mol) + 2*(35.45 g/mol)
= 208.23 g/mol
- Moles of BaCl2 = mass of BaCl2 / molar mass
= 416 g / 208.23 g/mol
≈ 2 moles of BaCl2
2. Calculate the number of moles of H2O in the hydrated salt:
- Convert the mass of hydrated salt to moles by dividing by its molar mass.
- The molar mass of H2O is calculated as:
(H atomic mass) + (2 * O atomic mass)
= 1.01 g/mol + 16.00 g/mol
= 18.01 g/mol
- Moles of H2O = mass of H2O / molar mass
= 488 g / 18.01 g/mol
≈ 27 moles of H2O
3. Determine the difference in moles between the hydrated salt and anhydrous BaCl2:
- Moles of water lost = moles of H2O in the hydrated salt - moles of BaCl2
= 27 moles - 2 moles
= 25 moles
Therefore, the value of x in the formula BaCl2.xH2O is 25. The compound is BaCl2.25H2O.
To find the value of x in the formula BaCl2.xH2O, we need to use the given information about the mass of the anhydrous BaCl2 and the mass of the hydrated salt.
1. Calculate the molar mass of BaCl2:
- Ba (Barium) has a molar mass of 137.33 g/mol
- Cl (Chlorine) has a molar mass of 35.45 g/mol (x2 since there are 2 Cl atoms)
- The molar mass of BaCl2 is therefore 137.33 + (35.45 x 2) = 208.23 g/mol
2. Calculate the number of moles of anhydrous BaCl2:
- Divide the mass of anhydrous BaCl2 (416 g) by its molar mass (208.23 g/mol):
- Moles of BaCl2 = 416 g / 208.23 g/mol = 1.998 mol
- Round this to the appropriate number of significant figures, if necessary.
3. Calculate the number of moles of water in the hydrated salt:
- Subtract the mass of anhydrous BaCl2 from the mass of the hydrated salt to find the mass of water:
- Mass of water = Mass of hydrated salt - Mass of anhydrous BaCl2
- Mass of water = 488 g - 416 g = 72 g
- Water (H2O) has a molar mass of 18.02 g/mol
- Divide the mass of water (72 g) by its molar mass (18.02 g/mol):
- Moles of water = 72 g / 18.02 g/mol = 3.998 mol
- Again, round this to the appropriate number of significant figures, if necessary.
4. Determine the ratio between moles of anhydrous BaCl2 and moles of water:
- Divide the moles of anhydrous BaCl2 by the moles of water:
- Moles of BaCl2 / Moles of water = 1.998 mol / 3.998 mol
- Simplify this ratio, if possible.
The ratio obtained from this calculation will give the value of x in the formula BaCl2.xH2O.