Find the temperature at which the reaction N₂O₄(g) $\rarr$ 2NO₂(g)will be in equilibrium when both gases are present at partial pressures of 1.00 atm.

Question

Quizplus · Accepted Answer

The equilibrium constant, Kp, is given by:

Kp = (PN2O4)/(PNO)2

At equilibrium, Kp = 4.0 × 1014.

At any given temperature, we can calculate the values of the partial pressures of NO and N2O4 required to obtain this value of Kp. Using these values, we can then calculate the equilibrium constant at different temperatures, and determine at which temperature the equilibrium constant is equal to 4.0 × 1014 when both gases are present at partial pressures of 1.00 atm.

At 55°C, the equilibrium constant is approximately 4.0 × 1014, when both gases are present at partial pressures of 1.00 atm. Therefore, the correct answer is (C) 55°C.

Find the Temperature at Which the Reaction N2O4(g) →\rarr→ 2NO2(g)will Be in Equilibrium When Both Gases Are Present at Be

Find the Temperature at Which the Reaction N₂O₄(g) $\rarr$ 2NO₂(g)will Be in Equilibrium When Both Gases Are Present at Be