If the equilibrium constant for the following reaction is K_c = 1 x 10²
2 C₂H₆(g) + 7 O₂(g) 4 CO₂(g) + 6 H₂O(g)
And all the concentrations were initially 0.10 M, we can predict that the reaction

Question

If the equilibrium constant for the following reaction is K_c = 1 x 10²
2 C₂H₆(g) + 7 O₂(g)

If the equilibrium constant for the following reaction is K<sub>c</sub> = 1 x 10<sup>2</sup> 2 C<sub>2</sub>H<sub>6</sub>(g) + 7 O<sub>2</sub>(g) 4 CO<sub>2</sub>(g) + 6 H<sub>2</sub>O(g) And all the concentrations were initially 0.10 M, we can predict that the reaction A) is at equilibrium initially. B) must shift from left to right to reach equilibrium. C) must shift from right to left to reach equilibrium. D) cannot reach equilibrium. E) cannot be determined unless we have the information necessary to calculate Q<sub>c</sub> for the reaction.

4 CO₂(g) + 6 H₂O(g)
And all the concentrations were initially 0.10 M, we can predict that the reaction

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The Answer of If the equilibrium constant for the following reaction is K_c = 1 x 10² 2 C₂H₆(g) + 7 O₂(g) 4 CO₂(g) + 6 H₂O(g) And all the concentrations were initially 0.10 M, we can predict that the reaction

If the Equilibrium Constant for the Following Reaction Is Kc

If the Equilibrium Constant for the Following Reaction Is K_c