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All textbooksBrown 14th EditionCh.10 - GasesProblem 126c

Chapter 10, Problem 126c

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I21s2 + 5 F21g2¡2 IF51g2 A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (c) Draw the Lewis structure of IF5.

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Hello. Everyone in this video we're going to draw out the lewis structure for Penta chloride which is PCL five. So first things first we're gonna go ahead and calculate for the total number of valence electrons. So for phosphorus that's going to be in group 58. That means that we have five electrons or valence electrons per atom. So in our compound or molecule we have one phosphorus atom and then we have five electrons per atom. So that will give us five electrons total for phosphorus. And then for chlorine here we have five atoms of chlorine and chlorine is in group 78. So there's going to be seven valence electrons per atom. So multiplied by seven giving us total 35 for the whole molecule. Then five plus 35 is going to be 40. So there should be 40 total valence electrons in this molecule. So now choosing the central atom we're comparing phosphorus with chlorine. Well if there's more than one of another atom, usually that's the indicator that that's not going to be the central atom. So phosphorus in our case will be our central atom and of course it's connected to five different chlorine atoms. So go ahead and draw those in. Alright. And to fulfill its octet, the chlorine has to have eight total electrons on it. Right now it's shared with the phosphorus. So that's considered to then we need six more. So we'll draw out three lone pairs per chlorine atom. Now we do this we can see that each chlorine will have eight toilet trans around it and we have five chlorine to five Or yes, five times are eight valence electrons will give us a total of 40 electrons in which we have used. And so this right here is going to be our LewiS structure for our pento chloride.
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Textbook Question

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I21s2 + 5 F21g2¡2 IF51g2 A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (a) What is the partial pressure of IF5 in the flask?

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Textbook Question

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I21s2 + 5 F21g2¡2 IF51g2 A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (d) What is the total mass of reactants and products in the flask?

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Textbook Question

A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas at 28 °C and 99.06 kPa pressure. (c) Assuming that the reactions are complete, calculate the percentage by mass of magnesium carbonate in the mixture.

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