Assume an equilibrium constant K_c = 1.7 x 10^-2 for the reaction:

N₂(g) + 3 H₂(g) 2 NH₃(g)
Calculate (to a first approximation) the equilibrium concentrations of NH₃, H₂ and N₂ when 0.10 moles per liter each of N₂ and H₂ are mixed and allowed to react to equilibrium.

Question

Assume an equilibrium constant K_c = 1.7 x 10^-2 for the reaction:

N₂(g) + 3 H₂(g)

Assume an equilibrium constant K<sub>c</sub> = 1.7 x 10<sup>-2</sup> for the reaction: N<sub>2</sub>(g) + 3 H<sub>2</sub>(g) 2 NH<sub>3</sub>(g) Calculate (to a first approximation) the equilibrium concentrations of NH<sub>3</sub>, H<sub>2</sub> and N<sub>2</sub> when 0.10 moles per liter each of N<sub>2</sub> and H<sub>2</sub> are mixed and allowed to react to equilibrium.

2 NH₃(g)
Calculate (to a first approximation) the equilibrium concentrations of NH₃, H₂ and N₂ when 0.10 moles per liter each of N₂ and H₂ are mixed and allowed to react to equilibrium.

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The Answer of Assume an equilibrium constant K_c = 1.7 x 10^-2 for the reaction: N₂(g) + 3 H₂(g) 2 NH₃(g) Calculate (to a first approximation) the equilibrium concentrations of NH₃, H₂ and N₂ when 0.10 moles per liter each of N₂ and H₂ are mixed and allowed to react to equilibrium.

Assume an Equilibrium Constant Kc = 1

Assume an Equilibrium Constant K_c = 1