Nitrogen dioxide is one of the many oxides of nitrogen (often form another form

Question

Nitrogen dioxide is one of the many oxides of nitrogen (often form another form of NOx, dinitrogen tetroxide A chemical engineer studying this reaction fils a 500. mL flask at 7.9 °C with 4.9 atm of nitrogen dioxide gas. He thèn raises the temperature considerably and when the mixture has come to equilibrium determines that it contains 2.7 atm of nitrogen dioxide gas The engineer then adds another 1.2 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits collectively called·N ' that are of interest to atmospheric chemistry. It can eact with ter to atm -10 I Don't Know Submit

Explanation / Answer

The reaction is 2NO2(g)<-------->N2O4(g)

let P= partial pressure of N2O4 at equilibrium, then 4.9-2P= partial pressure of NO2(g) at equilibrium

P+4.9-2P= 2.7

P= 2.2 atm

so at equilibrium, PNO2= 4.9-2*2.2= 0.5 atm and N2O4= 2.2 atm

KP= Equilibrium constant = (PN2O4)/ (PNO2)2 = 2.2/ (0.5*0.5)=8.8

when 1.2 atom of NO2 is added, PNO2= 0.5+1.2 =1.7 atm and PN2O4= 2.2 atm

Q= reaction coefficient = PN2O4/ (PNO2)2 = 2.2/ (1.7*1.7)=0.76<K, so the equilibrium shifts towards products side

let P= additional parital pressure of N2O4 due to reaction, PN2O4= 2.2+P and PNO2= 1.7-2P

K= 8.8= (2.2+P)/ (1.7-2P)2

when solved using excel, P= 0.569

So at equilibrium, PN2O4= 2.2+0.569= 2.769atm and PNO2= 1.7-2*0.569= 0.562 atm

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