Complete Hydrolysis of P4S6

In the process of complete hydrolysis of P4S6, the compound P4S6 reacts with water to form phosphoric acid (H3PO4) and hydrogen sulfide (H2S). This reaction can be represented by the following balanced chemical equation:

P4S6 + 12H2O → 4H3PO4 + 6H2S

To determine the number of water molecules required for this reaction, we need to analyze the stoichiometric coefficients in the balanced equation.

Stoichiometry Analysis

1. Balanced Equation:
- The balanced equation shows the molar ratios between reactants and products.
- In this case, the stoichiometric coefficient of P4S6 is 1, indicating that 1 mole of P4S6 reacts with 12 moles of water.

2. Ratio of P4S6 to H2O:
- The stoichiometric coefficient of P4S6 is 1, while the coefficient of water is 12.
- This means that for every 1 mole of P4S6, 12 moles of water are required.

3. Molar Mass Calculation:
- To convert the moles of water to its mass, we need to know the molar mass of water.
- The molar mass of water (H2O) is calculated by adding the atomic masses of its constituents: 2(1.01 g/mol) + 16.00 g/mol = 18.02 g/mol.

Calculating the Number of Water Molecules

To calculate the number of water molecules required for the complete hydrolysis of P4S6, we need to convert the given mass of P4S6 into moles, and then use the stoichiometric ratio to determine the moles of water.

1. Assume we have a certain mass of P4S6.
2. Convert the mass of P4S6 to moles using the molar mass of P4S6.
3. Use the stoichiometric ratio of P4S6 to water (12:1) to determine the moles of water required.
4. Convert the moles of water to the number of water molecules using Avogadro's number (6.022 x 10^23 molecules/mol).

Conclusion

In the complete hydrolysis of P4S6, 12 water molecules are required for every mole of P4S6. This is determined by the stoichiometric coefficients in the balanced chemical equation.