A reaction vessel is charged with 1.720 atm of N₂O₄ and 1.220 atm of NO₂ at 25 C. The equilibrium reaction is given in the equation below. N₂O₄ (g) 2 NO₂ (g)
After equilibrium is reached, the partial pressure of NO₂ is 0.555 atm. What is the value for the equilibrium constant, K c , of this reaction at 25 C?

Question

A reaction vessel is charged with 1.720 atm of N₂O₄ and 1.220 atm of NO₂ at 25 C. The equilibrium reaction is given in the equation below. N₂O₄ (g)

A reaction vessel is charged with 1.720 atm of N₂O<sub>4</sub> and 1.220 atm of NO₂ at 25 C. The equilibrium reaction is given in the equation below. N₂O<sub>4</sub> (g) 2 NO₂ (g) After equilibrium is reached, the partial pressure of NO₂ is 0.555 atm. What is the value for the equilibrium constant, K c , of this reaction at 25 C? A) K <sub>c</sub> = 0.129 B) K <sub>c</sub> = 0.150 C) K <sub>c</sub> = 0.222 D) K <sub>c</sub> = 0.270 E) K <sub>c</sub> = 6.67

2 NO₂ (g)
After equilibrium is reached, the partial pressure of NO₂ is 0.555 atm. What is the value for the equilibrium constant, K c , of this reaction at 25 C?

Quizplus · Accepted Answer

The Answer of A reaction vessel is charged with 1.720 atm of N₂O₄ and 1.220 atm of NO₂ at 25 C. The equilibrium reaction is given in the equation below. N₂O₄ (g) 2 NO₂ (g) After equilibrium is reached, the partial pressure of NO₂ is 0.555 atm. What is the value for the equilibrium constant, K c , of this reaction at 25 C?

A Reaction Vessel Is Charged with 1