Chemistry · Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of Delta G and Delta G° in chemical equilibrium
For the following equilibrium, in gaseous phase, is of the total volume when equ
For the following equilibrium, \( N_{2} O_{4} \rightleftharpoons \) \( 2 N O_{2} \) in gaseous phase, \( N O_{2} \) is \( 50 \% \) of the total volume when equilibrium is set up. Hence, percent of dissociation of \( N_{2} O_{4} \) is:
- A. 50\%
- B. 25\%
- C. \( 66.66 \% \)
- D. 33.33\%
Step-by-step solution
Let initial moles of N2O4 be 1. Let α be the degree of dissociation. At equilibrium: N2O4 = 1-α, NO2 = 2α, total moles = 1+α. Given NO2 is 50% of total volume (mole fraction = 0.5), so 2α/(1+α) = 0.5. Solving gives α = 1/3 = 33.33%.
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