Question

compare real and ideal gasses

91. Hydrogen azide, HN3, decomposes on heating by the following unbalanced reaction: 10 C HN (8) - N(3) + H2() If 3.0 atm of pure HN (g) is decomposed initially, what is the fi- nal total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.

Answer 1

page:01 Answer: According to this given information, to find the following problems. Given, balanced equation for the reaction is, 24N3 19 1 -->> 3N2 (g) + Hly (g). { lеле, 2 moler of Myhroten aide decomposing. to give umoles of products. since, * The number of moles is doubled at constant volume and temperaturaalso, the poressure is doubled. SO * the total pressure in the reackon Containen is, - 2x 3.catm = 6.0 atm. * what are the partial pressure for nitrogen and Hydrogen het,

page:02 partial pressure total pressure X mole frackon * Hole fraction of Nitrogen gas ir .Mole fraction of Nitrogen gas Moles of nitrogen total moler. ? 3/4 * mole fraction of Hydrogen gas : Mole fraction of Hydrogen gas z molesof Hephrogen Total moles. Therefore, * calculate partial pressure of Nitrogen gas:- partial pressure of Nitrogen gas e total pressure X mole fraction of Nitrogen gas : Goatm x 3 = _ 18 atm 4 .. partial pressure of Nitrogen gas = uos atm.

sure o +4dyogen qui J=0 =0 page.03 * calculate pon-kial presence of hydrogen-gas; partial pressure of Hydrogen gas a total pressure x mole fraction of hydrogen gas = 60 atm x ! = batm i pontial pressure of Hychogen gas= lsalm.