Question

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2(s)+5F2(g)→2IF5(g) A 5.50 −L flask containing 11.0 g I2 is charged with 11.0 g 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?

B) What is the mole fraction of IF5 in the flask?

C) Draw the Lewis structure of IF5

D) What is the total mass of reactants and products in the flask?

Answer 1

Sall) wien recach it Id(s) +599) 21 Fs (9) Mars of I, =lig 3. Male of J2 (25) = 119/roon 2000434 mod 2253.88/mal Man of fz = 11g Mole... of F₂ = 1/8 tal = 0.21 Aloccar" og moke earl Imole of I eucact with small of f2 0'0434 mole of I record with (0.217) male of 2 - Lowe have 0.2895 mal - I i limiting secagent :: Abel og IFs formol = 2x o.ouze mal = 0.0868 mel A) Partial forester of Ifr = NIE XRT 0.08688 0.0820 Lam x398k t SSOL hoi olak - Iluks = 0.516 km] 8) Mole troet son of IFS EXIF) = MIFE MIf the bli (Initial- - 0.0968 mal Contmed) 0.0868 mel+0.0725 and 2 - 0:5417 c) wouls Structene -> Total Valence = 7+ 5*3 ) = 420 1) Mars of reactant - Mass of left f . = 6.2895 ml x 389/mal 311.00lg Mast of foroduct = Mars of Ifs = 0.8868 molx 22119 g/mol - 19.278