Exhibit 14-3
The following question(s) pertain to the reaction N₂(g) + 3H₂(g) $\leftrightarrows$ 2NH₃(g) at 200°C with the reaction vessel being charged in such a way that the initial partial pressures of N₂, H₂, and NH₃ are 0.200, 0.300, and 0.600 atm respectively.
Refer to Exhibit 14-3. Based on the equilibrium constant and the value of Q, will more reactants or products be formed as the system approaches equilibrium at this temperature?

Question

Exhibit 14-3
The following question(s) pertain to the reaction N₂(g) + 3H₂(g)

\leftrightarrows

2NH₃(g) at 200°C with the reaction vessel being charged in such a way that the initial partial pressures of N₂, H₂, and NH₃ are 0.200, 0.300, and 0.600 atm respectively.
Refer to Exhibit 14-3. Based on the equilibrium constant and the value of Q, will more reactants or products be formed as the system approaches equilibrium at this temperature?

Quizplus · Accepted Answer

To determine the direction of the reaction, compare the reaction quotient (Q) with the equilibrium constant (K). If Q > K, the reaction will shift towards the reactants to reach equilibrium. If Q < K, it will shift towards the products. Without the value of K, we can't calculate Q, but the question implies that Q is greater than K, indicating more reactants will be formed.

Exhibit 14-3 the Following Question(s) Pertain to the Reaction N2(g) ⇆\leftrightarrows ⇆

Exhibit 14-3
the Following Question(s) Pertain to the Reaction N₂(g) $\leftrightarrows$