For the reaction N 2 O 4 (g) ⇌ 2NO 2 (g), the value of K p is 1.7 × 10 3 at 500 K and…
Chemistry · JEE Advanced · NTA Exams — Equilibrium
For the reaction N2O4 (g) \(\text { ⇌ }\)2NO2 (g), the value of Kp is 1.7 × 103 at 500 K and 1.78 × 104 at 600 K. Which of the following is correct ?
I. The proportion of NO2 in the equilibrium mixture is increased by decreasing the pressure
II. The standard enthalpy change for the forward reaction is negative
III. units of Kp are atm
IV. At 500 K, the degree of dissociation N2O4 decreases by 50% by increasing the pressure by 100%.
The correct choice is :
I. The proportion of NO2 in the equilibrium mixture is increased by decreasing the pressure
II. The standard enthalpy change for the forward reaction is negative
III. units of Kp are atm
IV. At 500 K, the degree of dissociation N2O4 decreases by 50% by increasing the pressure by 100%.
The correct choice is :
- I, III
- I
- II, IV
- III
Answer
(A) I, III
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