Final answer:
To find the mass of POCl3 that can form from 25.0 g of PCl5, calculate the moles of PCl5 and use the stoichiometric ratios from the balanced equation to determine the corresponding moles, and then mass, of POCl3 produced.
Step-by-step explanation:
The question relates to a stoichiometry problem where we have to calculate how much phosphorus oxychloride (POCl3) can be formed from a given mass of phosphorus pentachloride (PCl5) when it reacts with water (H2O).
First, we need the balanced chemical equation for the reaction:
PCl5 + H2O → POCl3 + 2HCl
To solve this problem:
- Calculate the molar mass of PCl5.
- Determine the number of moles of PCl5 present in 25.0 g.
- Use the stoichiometry of the balanced equation to find the amount of POCl3 formed.
- Finally, calculate the mass of POCl3 from the moles using its molar mass.
Since the students are provided with options rather than calculating the exact amount, they can use these steps to identify which of the given options (a. 114 g, b. 125 g, c. 137 g, d. 150 g) is correct.