a) Tetraphosphorus (P4), commonly known as white phosphorus, forms different compounds with chlorine (Cl2) depending on the amount of chlorine present. If chlorine is limited, phosphorus trichloride (PCl3) is formed. If there is an excess of chlorine, phosphorus pentachloride (PCl5) is formed.Write balanced equations for the two reactions of white phosphorous with chlorine.

b) Design an experiment that could be performed to verify each synthesis reaction. Include a hypothesis relating to whether PCl3 or PCl5 will be produced, information about the initial masses you would use, and possible problems that might arise.
c) Explain how your experiment will confirm the conservation of matter for each reaction.
d) Based on the ratio of moles of reactants in each case, predict the product of each trial of your experiment (PCl3 or PCl5) using your chosen initial masses. Explain your reasoning, and show any calculations.
e) Suppose you choose the initial masses so that both reactions produce PCl3. Explain how both of these chemical reactions obey the law of definite proportions, even though they produce different numbers of moles of the product. Justify your answer with calculations.

I need help with part b.

To follow up on Bob Pursley's response, you know the Cl2 will be the limiting reagent (unless of course you start with too much P4) but I would think you start with some amount of P4, use stoichiometry to add enough Cl2 to form PCl3 and do a separate calculation to see how much Cl2 to add for PCl5. The hypothesis should be centered around what the limiting reagent is and how that affects the yield of either PCl3 or PCl5. That should get you started.

b) To verify the synthesis reactions, you can perform the following experiment:

Experiment 1: Synthesis of Phosphorus Trichloride (PCl3)
Hypothesis: Limited chlorine will result in the formation of Phosphorus Trichloride (PCl3).

Procedure:
1. Weigh a known amount of white phosphorus (P4) and record its mass.
2. Place the white phosphorus in a reaction flask or container.
3. Slowly add chlorine gas (Cl2) to the flask in a controlled manner until all the white phosphorus has reacted.
4. Observe any changes in color, odor, or the formation of a new compound.
5. Once the reaction is complete, collect the gas formed and perform appropriate tests to confirm it is Phosphorus Trichloride (PCl3).
6. Weigh the final product and record its mass.

Possible problems that might arise:
- Managing and controlling the addition of chlorine gas can be challenging. Ensure safety precautions while handling chlorine gas.
- There may be impurities or side reactions that could affect the formation and purity of PCl3. Perform the appropriate tests to verify its identity.

Experiment 2: Synthesis of Phosphorus Pentachloride (PCl5)
Hypothesis: Excess chlorine will result in the formation of Phosphorus Pentachloride (PCl5).

Procedure:
1. Weigh another known amount of white phosphorus (P4) and record its mass.
2. Place the white phosphorus in a reaction flask or container.
3. Add an excess amount of chlorine gas (Cl2) to the flask.
4. Observe any changes in color, odor, or the formation of a new compound.
5. Once the reaction is complete, collect the gas formed and perform appropriate tests to confirm it is Phosphorus Pentachloride (PCl5).
6. Weigh the final product and record its mass.

Possible problems that might arise:
- Controlling the addition of excess chlorine gas can be challenging. Ensure safety precautions while handling chlorine gas.
- There may be impurities or side reactions that could affect the formation and purity of PCl5. Perform the appropriate tests to verify its identity.

Remember to always follow proper safety guidelines and seek guidance from a chemistry professional before conducting any experiments.

Note: The experimental details provided are general guidelines, and it is important to consult an appropriate chemistry reference for specific experimental procedures and safety precautions.

To design an experiment to verify each synthesis reaction, you can follow these steps:

a) Experiment to verify the formation of phosphorus trichloride (PCl3):
1. Start by setting up a fume hood or a well-ventilated area for safety reasons.
2. Take a small amount of white phosphorus (P4) and weigh it accurately.
3. Place the measured white phosphorus in a dry and clean test tube.
4. Gradually add a limited amount of chlorine gas (Cl2) using a gas syringe.
5. Observe the reaction that takes place inside the test tube, noting any changes in appearance or other physical characteristics.
6. Allow the reaction to proceed for a sufficient amount of time.
7. Finally, examine the test tube for the formation of a yellowish liquid, which indicates the presence of phosphorus trichloride.

Hypothesis: If limited chlorine gas (Cl2) is added to white phosphorus (P4), phosphorus trichloride (PCl3) will be produced.

Possible problems: It is important to handle white phosphorus with care as it is highly reactive. The experiment should be conducted in a well-ventilated area or under a fume hood to avoid exposure to toxic gases. Additionally, there may be a risk of the reaction becoming violent if not properly controlled.

b) Experiment to verify the formation of phosphorus pentachloride (PCl5):
1. Similar to the previous experiment, set up a fume hood or a well-ventilated area for safety.
2. Take another portion of white phosphorus (P4) and weigh it accurately.
3. Place the measured white phosphorus in a dry and clean test tube.
4. This time, add an excess amount of chlorine gas (Cl2) using a gas syringe.
5. Observe the reaction that occurs inside the test tube, noting any changes in appearance or other physical characteristics.
6. Allow the reaction to proceed for a sufficient amount of time.
7. Finally, examine the test tube for the presence of a yellow solid, which indicates the formation of phosphorus pentachloride.

Hypothesis: If an excess amount of chlorine gas (Cl2) is added to white phosphorus (P4), phosphorus pentachloride (PCl5) will be produced.

Possible problems: Similar to the previous experiment, precautions should be taken while handling white phosphorus and working in a well-ventilated area. Handling chlorine gas requires caution as it is toxic and should be used in small quantities to avoid exposure.

By performing these experiments, you can confirm the formation of PCl3 and PCl5 in each case. Additionally, the conservation of matter can be confirmed by ensuring that the mass of the reactants equals the mass of the products. This can be checked by weighing the test tube before and after the reaction. Any change in mass should be accounted for by the reaction products that form.

To design an experiment to verify each synthesis reaction, you would need to set up a controlled experiment with phosphorus and chlorine. Here is an outline for each reaction:

1. Reaction: White phosphorus reacts with limited chlorine to form phosphorus trichloride (PCl3)
Balanced Equation: P4 + 6Cl2 --> 4PCl3

Experiment for Reaction 1:
- Hypothesis: If white phosphorus is reacted with limited chlorine, phosphorus trichloride (PCl3) will be produced.
- Procedure:
1. Measure a specific and known amount of white phosphorus (e.g., 5 grams) and place it in a clean, dry reaction vessel, like a test tube.
2. Add a measured excess of chlorine gas to the reaction vessel (e.g., twice the molar amount required for the reaction).
3. Seal the reaction vessel and gently heat it in a controlled environment, such as using a water bath or heating mantle.
4. Observe any changes in the reaction mixture, such as color or gas evolution.
5. Once the reaction is complete, allow the vessel to cool down.
6. Analyze the product using appropriate methods like spectroscopy or chemical tests to confirm the presence of phosphorus trichloride (PCl3).

Potential Problems:
- The reaction vessel must be sealed tightly to prevent the escape of reactants or products.
- White phosphorus is highly toxic and pyrophoric, so proper precautions should be taken and the experiment should be carried out in a fume hood or well-ventilated area.
- The chlorine gas used should be pure and free from moisture or impurities.

2. Reaction: White phosphorus reacts with excess chlorine to form phosphorus pentachloride (PCl5)
Balanced Equation: P4 + 10Cl2 --> 4PCl5

Experiment for Reaction 2:
- Hypothesis: If white phosphorus is reacted with excess chlorine, phosphorus pentachloride (PCl5) will be produced.
- Procedure: (similar to Reaction 1)
1. Measure a specific and known amount of white phosphorus (e.g., 5 grams) and place it in a clean, dry reaction vessel.
2. Add a large excess of chlorine gas to the reaction vessel (e.g., five times the molar amount required for the reaction).
3. Seal the reaction vessel and gently heat it in a controlled environment.
4. Observe any changes in the reaction mixture.
5. Once the reaction is complete, allow the vessel to cool down.
6. Analyze the product using appropriate methods to confirm the presence of phosphorus pentachloride (PCl5).

Potential Problems:
- Similar to Reaction 1, ensure a tight seal on the reaction vessel and take precautions when handling white phosphorus and chlorine gas.
- The excess chlorine gas should be carefully calculated to avoid hazards associated with overpressure in the vessel or escape of reactants.

Now that you have designed the experiments, you can move on to explain how the conservation of matter is confirmed by each reaction (part c).