Consider the equilibrium,2 NOCl(g)$\leftrightarrows$ Cl₂(g)+ 2 NO(g).When 2.000 atm NOCl is placed in a tank at 500.0 K and allowed to come to equilibrium,the equilibrium partial pressure of Cl₂ is 0.226 atm.Calculate K_p.

Question

Quizplus · Accepted Answer

The equilibrium constant can be calculated using the equilibrium partial pressures of the reactants and products:

Kp = (P(NO)² * P(Cl₂O)) / P(NOCl)²

We are given P(Cl₂O) = 0.226 atm and we can calculate the partial pressure of NO using the fact that the initial pressure of NOCl is equal to the sum of the equilibrium pressures of NOCl and NO:

P(NO) = (2.000 atm - 0.226 atm)/2 = 0.887 atm

The partial pressure of NOCl can then be calculated using the ideal gas law:

P(NOCl) = (2.000 atm - 0.887 atm)/2 = 0.556 atm

Substituting these values into the equilibrium constant expression gives:

Kp = (0.887² * 0.226) / 0.556² = 0.0193

Therefore, the correct answer is (C).

Consider the Equilibrium,2 NOCl(g) ⇆\leftrightarrows⇆ Cl2(g)+ 2 NO(g)

Consider the Equilibrium,2 NOCl(g) $\leftrightarrows$ Cl₂(g)+ 2 NO(g)