1.The iodine pentafluoride gas is prepared when iodine and fluorine react. A 5,00L container was used for reacting 10,0g of iodine and 10,0g of fluorine. When the reaction was finished the temperature is 125°C. Calculate the partial pressure of iodine pentafluoride gas and the total pressure of the final mixture. What gas law are you applying?
2006-11-12 07:20:23 · 1 answers · asked by gaby p 1 in Science & Mathematics ➔ Chemistry
To answer this question you must assume that the reaction goes to completion. The balanced reaction is:
I2 + 5F2 ---> 2IF5
The reaction starts with 0.0394 moles of I2 and 0.263 moles of F2.
Since they react in a 1:5 ratio, the iodine is the limiting reagent and there will be 0.066 moles of F2 remaining at the end of the reaction. 0.0788 moles of IF5 will be created since there are 2 moles of IF5 created from each mole of I2.
For the partial pressure of IF5, PV=nRT
P(5.00L) = (0.0788mol)(0.08206)(398K)
P = 0.515 atm
For the total pressure at the end of the reaction, there are 0.066 moles of F2 remaining and 0.0788 moles of IF5 created for a total of 0.145 moles of gas. PV=nRT
P(5.00L) = (0.145mol)(0.08206)(398K)
P = 0.947 atm
2006-11-12 07:57:44 · answer #1 · answered by Ravenwoodman 3 · 0⤊ 0⤋