# Problem: Suppose a 250. mL flask is filled with 0.60 mol of I2 and 2.0 mol HI. The following reaction becomes possible:H2(g) + I2(g) ⇌ 2 HI(g)The equilibrium constant K for this reaction is 5.23 at the temperature of the flask.Calculate the equilibrium molarity of HI. Round your answer to two decimal places.

###### FREE Expert Solution

We are being asked to calculate the concentration of HI at equilibrium:

H2(g) + I2(g) ⇌ 2 HI(g)      Kc = 5.23

When dealing with equilibrium and Kc:

Kc → equilibrium units are in molarity
Kc is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression

We're going to calculate for the final concentration of HI(g) using the following steps:

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###### Problem Details

Suppose a 250. mL flask is filled with 0.60 mol of I2 and 2.0 mol HI. The following reaction becomes possible:

H2(g) + I2(g) ⇌ 2 HI(g)

The equilibrium constant K for this reaction is 5.23 at the temperature of the flask.

Calculate the equilibrium molarity of HI. Round your answer to two decimal places.