If P4 (white phosphorous) forms different compounds with chlorine (Cl3) depending on the amount of chlorine present (limited chlorine forms PCl3 and chlorine in excess forms PCl5) design an experiment that could be performed to verify each synthesis reaction. Include a hypothesis relating to whether PCl3 or PCl5 are formed, info about the initial masses you'd use and possible problems that might arise.
I'm sTuCk!! Please help?
I don't know how to help you. You're looking for an in-depth paper which I estimate will take at least 4-5 pages (certainly not less than 3) typed. Few of us here have that kind of time AND you get no experience doing it. If you can clue me in on what your problem is perhaps I can get you started.
Sure, I can help you design an experiment to verify the synthesis reactions of white phosphorus (P4) with chlorine (Cl2) to form PCl3 and PCl5. Here's an experimental setup along with relevant information and possible problems that may arise:
Experiment Setup:
1. Obtain a sample of white phosphorus (P4) and chlorine gas (Cl2).
2. Use a fume hood or perform the experiment in a well-ventilated area due to the toxic nature of both white phosphorus vapor and chlorine gas.
3. Take suitable safety precautions, including wearing gloves, goggles, and a lab coat.
4. Ensure you have a reliable balance to measure the masses accurately.
Experimental Procedure:
1. Determining the Formation of PCl3:
a. Take a known mass of white phosphorus (e.g., 1 gram) and place it in a reaction vessel. Record the initial mass.
b. Add a limited amount of chlorine gas (e.g., 2 moles) to the vessel, where the molar ratio of P4 to Cl2 is 1:6.
c. Observe the reaction and record any changes that occur, such as color changes or gas evolution.
d. After the reaction is complete, weigh the remaining contents to determine the final mass. Any decrease in mass suggests the formation of PCl3.
e. Compare the final mass to the initial mass to calculate the amount of PCl3 formed.
2. Determining the Formation of PCl5:
a. Take another known mass of white phosphorus (e.g., 1 gram) and place it in a separate reaction vessel. Record the initial mass.
b. Add an excess amount of chlorine gas (e.g., 10 moles) to the vessel, where the molar ratio of P4 to Cl2 is 1:6.
c. Observe the reaction and record any changes that occur, such as color changes or gas evolution.
d. After the reaction is complete, weigh the remaining contents to determine the final mass. Any decrease in mass suggests the formation of PCl5.
e. Compare the final mass to the initial mass to calculate the amount of PCl5 formed.
Hypothesis:
Given a limited amount of chlorine gas, if the initial mass of white phosphorus decreases significantly, with a molar ratio of 1:6, then it is hypothesized that PCl3 will be formed. If an excessive amount of chlorine gas is used, with the same molar ratio, then it is hypothesized that PCl5 will be formed.
Possible Problems:
1. Safety concern: Both white phosphorus and chlorine are toxic substances. Proper precautions, such as working under a fume hood and wearing appropriate safety equipment, should be taken.
2. Reactivity: White phosphorus is highly reactive and can spontaneously ignite in air. Handle it with care and avoid exposure to open flames or heat sources.
3. Contamination: Ensure that the reaction vessels and equipment are clean and free from impurities which might skew the results.
4. Incomplete reactions: The reactions may not be 100% efficient, resulting in incomplete conversion of reactants to products. This can affect the accuracy of the final mass measurements and subsequent calculations.
Remember to consult your instructor or follow specific guidelines provided by your educational institution before conducting any experiments.