On heating 10grams copper sulphate crystals (CuSO4.5H2O),6.4 grams anhydrous sulphate was left .Find the value of X .
0.2mol
To find the value of X, we need to determine the number of water molecules present in the copper sulfate pentahydrate (CuSO4.5H2O) crystals.
The molar mass of copper sulfate pentahydrate can be calculated as follows:
Copper (Cu): 63.55 g/mol
Sulfur (S): 32.07 g/mol
Oxygen (O): 16.00 g/mol
Hydrogen (H): 1.01 g/mol
So, the molar mass of CuSO4.5H2O is:
(63.55 + 32.07 + (4 × 16.00) + (5 × (1.01 × 2))) = 249.72 g/mol
Now, let's calculate the total molar mass of the copper sulfate that was left after heating. This is given as 6.4 grams.
Moles = Mass / Molar Mass
Moles of copper sulfate = 6.4 g / 249.72 g/mol
Now, we know that for every 1 mole of copper sulfate, there are 5 moles of water molecules (H2O) present in the pentahydrate form. Therefore:
Moles of water = 5 × moles of copper sulfate
Now, let's calculate the mass of water (H2O) that was lost during heating using the following formula:
Mass = Molar Mass × Moles
Mass of water (H2O) = Molar Mass of H2O × Moles of water
Mass of water (H2O) = (18.02 g/mol) × (5 × moles of copper sulfate)
The initial mass of copper sulfate crystals was given as 10 grams, and the mass of water that was left was 6.4 grams. Therefore, the mass of water lost during heating is:
Mass of water lost = Initial mass of copper sulfate - Mass of copper sulfate + Mass of water
Mass of water lost = 10 g - 6.4 g + (18.02 g/mol) × (5 × moles of copper sulfate)
Now, we can equate the two expressions for the mass of water lost and solve for X:
Mass of water lost = Mass of water (H2O) lost during heating
10 g - 6.4 g + (18.02 g/mol) × (5 × moles of copper sulfate) = (18.02 g/mol) × (5 × moles of copper sulfate)
Now, we can solve the equation for X. However, please note that the equation provided might be incomplete or incorrect, so the actual value of X cannot be determined with the given information.
To find the value of X, which represents the number of moles of water in the copper sulfate formula (CuSO4.XH2O), we need to use the concept of stoichiometry.
First, we need to determine the number of moles of anhydrous (without water) copper sulfate (CuSO4) formed. The molar mass of anhydrous copper sulfate is calculated as follows:
- The atomic mass of copper (Cu) is 63.55 g/mol.
- The atomic mass of sulfur (S) is 32.07 g/mol.
- The atomic mass of oxygen (O) is 16.00 g/mol.
So the molar mass of CuSO4 is:
(1 atom of Cu x 63.55 g/mol) + (1 atom of S x 32.07 g/mol) + (4 atoms of O x 16.00 g/mol) = 159.63 g/mol.
Given that you started with 10 grams of copper sulfate crystals, we can calculate the number of moles of CuSO4 as follows:
Number of moles = mass / molar mass
Number of moles of CuSO4 = 10 g / 159.63 g/mol = 0.062739 moles.
Next, we need to determine the number of moles of anhydrous copper sulfate (CuSO4) that remained after heating. This can be calculated by subtracting the moles of anhydrous copper sulfate from the moles of copper sulfate initially present. In this case, the moles of CuSO4 left would be:
Number of moles of CuSO4 left = 0.062739 moles - X moles of H2O.
Since the molar mass of water (H2O) is 18.02 g/mol, we can calculate the mass of water in grams:
Mass of H2O = X moles of H2O x 18.02 g/mol.
Given that 6.4 grams of anhydrous copper sulfate remained after heating, we can write the following equation:
Mass of CuSO4 left = 10 g - Mass of H2O.
Substituting the known values, we have:
6.4 g = 10 g - X moles of H2O x 18.02 g/mol.
Simplifying the equation further:
6.4 g = 10 g - 18.02 X g/mol.
Rearranging the equation:
18.02 X g/mol = 10 g - 6.4 g = 3.6 g.
Now, solve for X:
X g/mol = 3.6 g / 18.02 g/mol.
Dividing and simplifying:
X = 0.1998.
Therefore, the value of X is approximately 0.20.