What mass in grammes of hydrogen sulphide will be required to precipitate 15g of copper sulphide from a copper(2) tetraoxosulphate (6) solution?
Please note that if you start with CuSO4 you will produce CuS and not Cu2S.
CuSO4 + H2S ==> CuS + H2SO4
Note also that a correct IUPAC name is copper(II) sulfate.
write the equation
how many moles of Cu2S in 15g?
The equation will tell you how many moles of H2S to use; convert that back to grams.
To determine the mass of hydrogen sulphide required to precipitate 15g of copper sulphide from a copper(II) tetraoxosulphate (VI) solution, you need to consider the balanced chemical equation for the reaction between hydrogen sulphide and copper(II) tetraoxosulphate (VI):
CuSO4 + H2S -> CuS + H2SO4
By inspecting the equation, you can see that the stoichiometric ratio between CuS and H2S is 1:1. This means that for every 1 mole of CuS, we need 1 mole of H2S.
Now, let's calculate the molar mass of CuS and H2S:
- The atomic weight of Cu: 63.55 g/mol
- The atomic weight of S: 32.06 g/mol
Molar mass of CuS:
= (atomic weight of Cu) + (atomic weight of S)
= 63.55 + 32.06
= 95.61 g/mol
Molar mass of H2S:
= 2 * (atomic weight of H) + (atomic weight of S)
= 2 * 1.01 + 32.06
= 34.08 g/mol
Now, let's calculate the number of moles of CuS:
Number of moles = mass / molar mass
Number of moles = 15g / 95.61 g/mol
Number of moles ≈ 0.157 moles
Since the stoichiometric ratio between CuS and H2S is 1:1, we need the same number of moles of H2S as CuS. Therefore, you will need approximately 0.157 moles of H2S.
Finally, let's calculate the mass of H2S required:
Mass = number of moles * molar mass
Mass = 0.157 moles * 34.08 g/mol
Mass ≈ 5.35g
Therefore, approximately 5.35g of hydrogen sulphide is required to precipitate 15g of copper sulphide from a copper(II) tetraoxosulphate (VI) solution.
To determine the mass of hydrogen sulphide (H2S) required to precipitate copper sulphide (CuS) from a copper(II) tetraoxosulphate(VI) solution, we need to use the stoichiometry of the reaction between copper(II) ions and hydrogen sulphide.
The balanced chemical equation for this reaction is as follows:
CuSO4 + H2S -> CuS + H2SO4
From the equation, we can see that the mole ratio between CuSO4 and H2S is 1:1. This means that 1 mole of CuSO4 requires 1 mole of H2S to fully react.
To calculate the mass of H2S required, use the following steps:
Step 1: Calculate the molar mass of CuSO4.
The molar mass of CuSO4 is calculated by adding the atomic masses of copper (Cu), sulfur (S), and four oxygen (O) atoms.
CuSO4 = (1 * Cu atomic mass) + (1 * S atomic mass) + (4 * O atomic mass)
Step 2: Convert the given mass of CuSO4 to moles.
To convert the mass of CuSO4 to moles, divide the given mass by the molar mass calculated in Step 1.
moles of CuSO4 = mass of CuSO4 / molar mass of CuSO4
Step 3: Calculate the moles of H2S required.
Since the mole ratio between CuSO4 and H2S is 1:1, the moles of H2S required will be the same as the moles of CuSO4.
moles of H2S = moles of CuSO4
Step 4: Convert moles of H2S to mass.
To convert the moles of H2S to mass, multiply the moles of H2S by its molar mass.
mass of H2S = moles of H2S * molar mass of H2S
By following these steps, you can calculate the mass of H2S required to precipitate 15g of CuS from the copper tetraoxosulphate solution.