The equilibrium reaction N₂O₄(g) ⇄ 2 NO₂(g) has been thoroughly studied (Figure 15.7).

(a) If the total pressure in a flask containing NO₂ and N₂O₄ gas at 25°C is 1.50 atm and the value of K_p at this temperature is 0.148, what fraction of the N₂O₄ has dissociated to NO₂?
(b) What happens to the fraction dissociated if the volume of the container is increased so that the total equilibrium pressure falls to 1.00 atm?

Data given in figure 15.7

Transcribed Image Text:

Higher Temperature At 50 °C the equilibrium is shifted toward NO2, as indicated by the darker brown color. 2 NO₂(g) Brown gas N₂04(g) Colorless gas Cengage Learning/Marna G. Clarke X X H Lower Temperature The mixture of NO₂ and N₂O4 gas at 0°C is only slightly brown, indicating a smaller concentration of the brown gas NO₂ than at 50 °C.