12.39 kg sample of phosphorus reacts with 52.54 kg of chlorine to form only phos

Question

12.39 kg sample of phosphorus reacts with 52.54 kg of chlorine to form only phosphorus trichloride. In a similar process, the chlorine is introduced to the reactor as a solution in carbon tetrachloride (tetrachloromethane). The solvent does not react. What volume of a 4.5 M solution is required to deliver for the stoichiometric amount of chlorine? Water is much less expensive than carbon tettrachloride. It is less toxic and easier to recycle or purify for further use. Another chemist thinks that the process can be improved by using water instead of carbon tet as the solvent. Is this a good idea? Justify your answer! Hint: show (potential) reactions of starting materials and products

Explanation / Answer

The reaction is 2P+3Cl2---->2PCl3

atomic weight of P= 31, mole of P= 12.39*1000/31=400gmoles

From the stoichiometry, 2 moles of P reqquires 3 mole of Cl2

400moles required 400*3/2= 600 gmole of Cl2

Volume of Solution required = 600 gmoles/ 4.5 gmoles/L= 133.3 L

Chlorine dissoves in water accordingly

Cl2 + H2O -> HCl + HClO , So chlorine not only dissovles, but reacts with water to form Hypochlorous acid.

Hence HCl and HClO does not react with Phosphorous. It is not a good idea.

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