A student was asked to prepare a sample of copper(ii)sulphate crystals(CUSO4.5H2O) given 5g of of copper (ii)oxide (CUO) as the starting material.if 10g of dry crystals of CUSO4.5H2O were obtained,calculate the percentage yield???
Convert 5 g CuO to grams CuSO4.5H2O.
That s 5 g CuO x (molar mass CuSO4.5H2O/molar mass CuO) = ?g CuSO4.5H2O equivalent. This is the theoretical yield (TY). The actual yield (AY) from the problemn is 10g.
%yield = (AY/TY)*100 = ?
Well, well, well! It seems we have a chemistry question. Brace yourself, because I'm about to perform some math magic!
To find the percentage yield, you need to compare the actual yield (10g) with the theoretical yield, which we'll calculate. So, let's get those calculators out.
First, we need to find the molar mass of copper(II) oxide (CUO). Copper has a molar mass of 63.55 g/mol, and oxygen has a molar mass of 16.00 g/mol. Since there's only one oxygen atom in CUO, the molar mass of CUO is 63.55 + 16.00 = 79.55 g/mol.
Next, we calculate the molar mass of copper(II) sulfate pentahydrate (CuSO4.5H2O). Copper has a molar mass of 63.55 g/mol, sulfur has a molar mass of 32.07 g/mol, and oxygen has a molar mass of 16.00 g/mol. Additionally, we have 5 water molecules, and each one has a molar mass of 18.02 g/mol. So, the molar mass of CuSO4.5H2O is (63.55 + 32.07 + (16.00 * 4) + (18.02 * 5)) g/mol = 249.68 g/mol.
Now, let's calculate the theoretical yield. We know that the starting material is 5g of copper(II) oxide (CUO), and the molar mass of CUO is 79.55 g/mol. Using stoichiometry, we can find that the theoretical yield of copper(II) sulfate pentahydrate (CuSO4.5H2O) is (5g * (1 mol / 79.55 g)) * (1 mol / 1 mol) * (249.68 g / 1 mol) = 15.69 g.
Finally, we can calculate the percentage yield: (Actual Yield / Theoretical Yield) * 100 = (10g / 15.69g) * 100 = 63.77%.
Ta-da! The percentage yield is approximately 63.77%.
To calculate the percentage yield, we need to compare the actual yield (10g) with the theoretical yield. The theoretical yield is the maximum amount of product that can be obtained based on the stoichiometry of the reaction.
First, we need to determine the balanced chemical equation for the reaction:
CUO + H2SO4 → CUSO4.5H2O
From the balanced equation, we can see that 1 mole of CUO reacts with 1 mole of H2SO4 to produce 1 mole of CUSO4.5H2O.
Next, we convert the given mass of CUO into moles:
Molar mass of CUO = 63.55 g/mol (copper) + 16.00 g/mol (oxygen) = 79.55 g/mol
Number of moles of CUO = 5g / 79.55 g/mol = 0.063 moles
Since the stoichiometry of the reaction is 1:1, the number of moles of CUSO4.5H2O formed is also 0.063 moles.
Now, we calculate the theoretical yield of CUSO4.5H2O:
Molar mass of CUSO4.5H2O = 63.55 g/mol (copper) + 32.07 g/mol (sulfur) + (16.00 g/mol (oxygen) * 4) + (1.01 g/mol (hydrogen) * 10) = 249.68 g/mol
Theoretical yield = Number of moles of CUSO4.5H2O * Molar mass of CUSO4.5H2O
Theoretical yield = 0.063 moles * 249.68 g/mol = 15.73 g
Now, we can calculate the percentage yield:
Percentage yield = (Actual yield / Theoretical yield) * 100
Percentage yield = (10g / 15.73g) * 100
Percentage yield = 63.6%
Therefore, the percentage yield of the reaction is 63.6%.
To calculate the percentage yield, you need to compare the actual yield (the amount of product obtained) with the theoretical yield (the maximum amount of product that could be obtained, based on stoichiometry).
First, let's calculate the theoretical yield of copper(II) sulfate pentahydrate (CuSO4·5H2O) using the given starting material, copper(II) oxide (CuO).
1 mole of CuO yields 1 mole of CuSO4·5H2O according to the balanced equation:
CuO + H2SO4 → CuSO4·5H2O
To find the number of moles of CuO, divide the given mass (5g) by the molar mass of CuO (63.55 g/mol):
Number of moles of CuO = 5g / 63.55 g/mol = 0.079 mol
Since the stoichiometry is 1:1, the number of moles of CuSO4·5H2O will also be 0.079 mol.
Now, let's calculate the theoretical yield of CuSO4·5H2O using the molar mass of CuSO4·5H2O (249.68 g/mol):
Theoretical yield = 0.079 mol × 249.68 g/mol = 19.68 g
Next, let's calculate the percentage yield using the actual yield and the theoretical yield:
Percentage yield = (actual yield / theoretical yield) × 100
Given that the actual yield is 10g, and the theoretical yield is 19.68g, we can calculate the percentage yield:
Percentage yield = (10 g / 19.68 g) × 100 ≈ 50.81 %
Therefore, the percentage yield of copper(II) sulfate pentahydrate is approximately 50.81%.