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 will be happy to critique your work. Read the statements, it tells you what the limiting reactant should be in any case.

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a) The balanced equations for the reactions are as follows:

1) When chlorine is limited:
P4 + 6Cl2 -> 4PCl3

2) When there is an excess of chlorine:
P4 + 10Cl2 -> 4PCl5

b) To verify each synthesis reaction, you could perform the following experiments:

1) To test for the formation of phosphorus trichloride (PCl3):
- Hypothesis: PCl3 will be produced.
- Obtain a known mass of white phosphorus (P4) and an excess amount of chlorine gas (Cl2).
- Place the white phosphorus in a reaction flask, and then add the chlorine gas to the flask.
- Allow the reaction to proceed at room temperature and observe any changes.
- Possible problems: Ensuring sufficient ventilation due to toxic fumes released during the reaction, ensuring safety procedures are followed.

2) To test for the formation of phosphorus pentachloride (PCl5):
- Hypothesis: PCl5 will be produced.
- Obtain a known mass of white phosphorus (P4) and a limited amount of chlorine gas (Cl2).
- Place the white phosphorus in a reaction flask, and then add the limited amount of chlorine gas to the flask.
- Allow the reaction to proceed at room temperature and observe any changes.
- Possible problems: Controlling the amount of chlorine gas used, ensuring safety procedures are followed.

c) The experiment will confirm the conservation of matter for each reaction by comparing the masses of the reactants with the masses of the products. The Law of Conservation of Matter states that matter cannot be created or destroyed, only transformed. In this case, the total mass of the reactants should be equal to the total mass of the products.

d) Based on the ratio of moles of reactants in each case, the predicted products can be determined.

1) When chlorine is limited:
- The balanced equation is P4 + 6Cl2 -> 4PCl3.
- From the equation, it can be seen that each mole of P4 reacts with 6 moles of Cl2 to produce 4 moles of PCl3.
- If the initial mass of P4 is known, the moles of P4 can be determined using its molar mass.
- The ratio of moles of PCl3 to moles of P4 is 1:1, indicating that the experiment should produce PCl3.

2) When there is an excess of chlorine:
- The balanced equation is P4 + 10Cl2 -> 4PCl5.
- From the equation, it can be seen that each mole of P4 reacts with 10 moles of Cl2 to produce 4 moles of PCl5.
- If the initial mass of P4 is known, the moles of P4 can be determined using its molar mass.
- The ratio of moles of PCl5 to moles of P4 is 1:1, indicating that the experiment should produce PCl5.

e) If the initial masses are chosen so that both reactions produce PCl3, it can be seen that the Law of Definite Proportions is still obeyed. The Law of Definite Proportions states that a compound is always composed of the same elements in the same ratio by mass.

Let's consider a hypothetical scenario where 2 grams of white phosphorus (P4) are used in both reactions:

1) When chlorine is limited:
- The balanced equation is P4 + 6Cl2 -> 4PCl3.
- The molar mass of P4 is 123.89 g/mol.
- Therefore, the moles of P4 can be calculated as: 2 g / 123.89 g/mol ≈ 0.0161 mol.
- According to the balanced equation, the moles of PCl3 produced would also be approximately 0.0161 mol.

2) When there is an excess of chlorine:
- The balanced equation is P4 + 10Cl2 -> 4PCl5.
- Following the same steps as above, the moles of PCl5 produced would also be approximately 0.0161 mol.

By using the same initial mass of white phosphorus for both reactions, the proportion of PCl3 to PCl5 remains the same, indicating that the reactions still obey the law of definite proportions.

a) The balanced equations for the two reactions of white phosphorus (P4) with chlorine (Cl2) are as follows:

1. Limited chlorine reaction: P4 + 6Cl2 → 4PCl3
2. Excess chlorine reaction: P4 + 10Cl2 → 4PCl5

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

1. Limited chlorine reaction:
- Hypothesis: If white phosphorus reacts with a limited amount of chlorine, phosphorus trichloride (PCl3) will be produced.
- Initial masses: Measure and record the mass of white phosphorus and the amount of chlorine reactant.
- Possible problems: Ensure proper safety measures are taken as both white phosphorus and chlorine are hazardous. Monitor the reaction carefully for any unforeseen side reactions or incomplete reactions.

2. Excess chlorine reaction:
- Hypothesis: If white phosphorus reacts with an excess amount of chlorine, phosphorus pentachloride (PCl5) will be produced.
- Initial masses: Measure and record the mass of white phosphorus and an excess amount of chlorine reactant.
- Possible problems: Similar to the limited chlorine reaction, ensure proper safety precautions are followed. Monitor the reaction to ensure complete conversion and avoid any contamination.

c) The experiment confirms the conservation of matter for each reaction because the total mass of the reactants should be equal to the total mass of the products. By measuring the initial masses of the reactants and collecting the mass of the products, you can compare them to ensure conservation of matter.

d) Based on the ratio of moles of reactants in each case, we can predict the product of each trial of the experiment.

1. Limited chlorine reaction:
- Refer to the balanced equation: P4 + 6Cl2 → 4PCl3
- Use the initial masses to calculate moles of reactants.
- Compare the moles of phosphorus to the moles of chlorine.
- The balanced equation shows a 1:6 ratio between phosphorus and chlorine.
- If the moles of phosphorus are less than 1/6th of the moles of chlorine, the limiting reagent is phosphorus, and the product will be PCl3.

2. Excess chlorine reaction:
- Refer to the balanced equation: P4 + 10Cl2 → 4PCl5
- Use the initial masses to calculate the moles of reactants.
- Compare the moles of phosphorus to the moles of chlorine.
- The balanced equation shows a 1:10 ratio between phosphorus and chlorine.
- If the moles of phosphorus are more than 1/10th of the moles of chlorine, the limiting reagent is chlorine, and the product will be PCl5.

e) If you choose the initial masses so that both reactions produce PCl3, it still obeys the law of definite proportions because the ratio of reactants to product is fixed. In both cases, the ratio of PCl3 to P4 is 1:1, regardless of the number of moles. The law of definite proportions states that a compound is always composed of the same elements in the same ratio by mass. Calculations based on the stoichiometry of the balanced equations will confirm this ratio.