# Consider this chemical reaction: H_2(g) + I_2(g) rightleftharpoons 2HI(g). At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0.033 M, and 0.55 M, respectively. What is the value of K_(eq) for this reaction?

Dec 1, 2016

${K}_{\text{eq}} > 50$

#### Explanation:

For the reaction:

${H}_{2} \left(g\right) + {I}_{2} \left(g\right) r i g h t \le f t h a r p \infty n s 2 H I \left(g\right)$

${K}_{\text{eq}} = {\left[H I \left(g\right)\right]}^{2} / \left(\left[{H}_{2} \left(g\right)\right] \left[{I}_{2} \left(g\right)\right]\right)$

$=$ ${\left(0.55 \cdot m o l \cdot {L}^{-} 1\right)}^{2} / \left(0.15 \cdot m o l \cdot {L}^{-} 1 \times 0.033 \cdot m o l \cdot {L}^{-} 1\right)$

$=$ ??