Safari Edit View History Bookmarks Window Help [] 84% \" Thu Dec 78:3 Chapter 10

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Safari Edit View History Bookmarks Window Help [] 84% " Thu Dec 78:3 Chapter 10smartwor 27% 12/08/17 06 Question ( point) a See page 457 In some aquatic ecosystems, nitrate (NOs) is converted to nitrite (NO21. which then decomposes to nitrogen and reaction, consider the decomposition of ammonium nitrite NH4NO2(aq )- N2(g) + 2H20(1) 1st attempt hl See Periodic Table What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N2 gas when the ammonium nitrite in 1.40Lof 0.900 M NH&4NO2 decomposes at 25.0°C? atm 3 OF 9 QUESTIONS COMPLETED

Explanation / Answer

The reaction is NH4NO2---à N2(g)+2H2O(l)

Moles of ammoniu nitrate can be calculated from

Moles of NH4NO2= Molarity* volume

Moles of NH4NO2= 0.900*1.4=1.26

From the reaction stoichiometry

One mole of NH4NO2 gives 1 mole of N2

Moles of N2 formed = 1.26

Given T= 25 deg.c= 25+273= 298K

V= 10L, R= gas constant =0.0821 L.atm/mole.K

P= pressure = nRT/V= 1.26*0.0821*298/10=3.08 atm

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