Question

When heated, colorless dinitrogen tetraoxide, N2O4(g), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204 (g) + 2 NO2 (g) Suppose that 2.00 mol of N204(g) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K, for this reaction at 407 K. 3.80 2.00 0.500 0.263 0.525

Answer 1

Equilibrium constant (Kc)! It is defined as lue ratio molar Concen of product ct tratiaus ct gaseous Drucucts to luct to tuct ct proceu- CH ct molar concoutrations ct gaseous react- auts to eneir powers raised to encir Stoichi- auctric Coettici euts at equilibrium, Nz Oy (9) کج 2 NO2 (9) Initial moles 2-00 24. Equilibrium moles (2.00-) Here x' is called degree of dissociation. Given, Erui librium Concentratica ct NO2 - 0.52SM, te (NO2) 0.525m =) no ctuoles ct No2 -0.525M Volume in

=) 2 a mol 0.525 M 5.00L =) 2 a M= 0.525 M لنگ 22 - (0.525) x(5.00) > 22 2.625 7) 2.625 - 1,3125 Equilibrium concentratica ct N₂ Oy (2.00-al melle 5.00 - 2-00 1.3125 M 5.00 0.1375M

5) Equilibrium constant (K) = C No2} [1204) (0.525) こ 0.1375 2-004 ~ 2.00 option B Correct