Given the equation 2A(g) 2B(g)+ C(g).At a particular temperature,K = 1.6 $\times$ 10 4 .
-If you mixed 5.0 mol B,0.10 mol C,and 0.0010 mol A in a one-liter container,which direction would the reaction initially proceed?

Question

Given the equation 2A(g)  2B(g)+ C(g).At a particular temperature,K = 1.6 $\times$ 10 4 .
-If you mixed 5.0 mol B,0.10 mol C,and 0.0010 mol A in a one-liter container,which direction would the reaction initially proceed?

Quizplus · Accepted Answer

The equilibrium constant (K) is less than 1, indicating that the forward reaction (2A → 2B + C) is not favored, and the reverse reaction (2B + C → 2A) is favored. Therefore, the reaction will initially proceed to the left, converting some of the B and C into A. As A increases, the reverse reaction will be favored less, until equilibrium is reached.

Given the Equation 2A(g) 2B(g)+ C(g) ×\times× 104

Given the Equation 2A(g) 2B(g)+ C(g) $\times$ 10⁴