Question

nixture of 5.09 mol of N2 and 30.33 g of NO is heated in a closed vessel to 2000 °C. After heating, the total pressure of the mixture at equilibrium is 3.14 atm. N,)+0,) 2no) K-0.101 at 2000 C In which direction does the reaction proceed after heating to 2000 C? The reaction is at equilibrium. The reaction proceeds toward reactants. O The reaction proceeds toward products. Calculate the equilibrium partial pressures of N2, O2, and NO at 2000 C. Number Number Number atm N, n O, atm NO atm

Answer 1

The reaction proceeds towards reactants , because there is no O2 in the begining.

          N2(g)   +   O2(g) <====> 2NO(g)

initial 5.09 mol       -          30.33/28 = 1.088 mol

change    +x            +x         -2x

equil    5.09+x         x          1.088-2x

total no of moles of gaseous mixture at equilibrium(n) = 1.088-2x+5.09+x+x

                                                       = 6.178 mol

at equilibrium,

as Dn rxn = 0

Kp = Kn = nNO^2/nN2*nO2

       0.101 = (1.088-2x)^2/((5.09+x)*x)

   x = 0.331

pNO = nNO/nTotal*pTotal

    = ((1.088-2*0.331)/6.178)*3.14

    = 0.216 atm

pO2 = (0.331/6.178)*3.14

    = 0.168 atm

pN2 = ((5.09+0.331)/6.178)*3.14

    = 2.76 atm