At a high temperature,equal concentrations of 0.160 mol/L of H₂(g) and I₂(g) are initially present in a flask.The H₂ and I₂ react according to the balanced equation below. H₂(g) + I₂(g) 2 HI(g)
When equilibrium is reached,the concentration of H₂(g) has decreased to 0.036 mol/L.What is the equilibrium constant,K_c,for the reaction?

Question

At a high temperature,equal concentrations of 0.160 mol/L of H₂(g) and I₂(g) are initially present in a flask.The H₂ and I₂ react according to the balanced equation below. H₂(g) + I₂(g)

At a high temperature,equal concentrations of 0.160 mol/L of H<sub>2</sub>(g) and I<sub>2</sub>(g) are initially present in a flask.The H<sub>2</sub> and I<sub>2</sub> react according to the balanced equation below. H<sub>2</sub>(g) + I<sub>2</sub>(g) 2 HI(g) When equilibrium is reached,the concentration of H<sub>2</sub>(g) has decreased to 0.036 mol/L.What is the equilibrium constant,K<sub>c</sub>,for the reaction? A) 3.4 B) 4.0 C) 12 D) 22 E) 48

2 HI(g)
When equilibrium is reached,the concentration of H₂(g) has decreased to 0.036 mol/L.What is the equilibrium constant,K_c,for the reaction?

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The Answer of At a high temperature,equal concentrations of 0.160 mol/L of H₂(g)and I₂(g)are initially present in a flask.The H₂ and I₂ react according to the balanced equation below. H₂(g)+ I₂(g) 2 HI(g) When equilibrium is reached,the concentration of H₂(g)has decreased to 0.036 mol/L.What is the equilibrium constant,K_c,for the reaction?

At a High Temperature,equal Concentrations of 0