Patel Weber
11/26/2023 · Primary School
Use the References to access important values if needed for this question. The equilibrium constant, \( K_{\mathrm{c}} \), for the following reaction is 0.0180 at 698 K . \[ 2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \] Calculate the equilibrium concentrations of reactant and products when 0.334 moles of \( \mathrm{HI}(g) \) are introduced into a 1.00 L vessel at 698 K . \( [\mathrm{HI}]=\square \mathrm{M} \) \( \left[\mathrm{H}_{2}\right]=\square \mathrm{M} \) \( \left[\mathrm{I}_{2}\right]=\square \)
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The equilibrium concentrations are \( [\mathrm{HI}] = 0.2532 \, \text{M} \), \( [\mathrm{H}_2] = 0.0404 \, \text{M} \), and \( [\mathrm{I}_2] = 0.0404 \, \text{M} \).
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