Burns Stewart
08/14/2023 · Junior High School
The equilibrium constant, \( K_{\mathrm{c}} \), for the following reaction is 55.6 at 698 K . \[ \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g}) \] Calculate the equilibrium concentrations of reactants and product when 0.372 moles of \( \mathrm{H}_{2} \) and 0.372 moles of \( \mathrm{I}_{2} \) are introduced into a 1.00 L vessel at 698 K . \( \left[\mathrm{H}_{2}\right]=\square \mathrm{M} \) \( \left[\mathrm{I}_{2}\right]=\square \mathrm{M} \) \( [\mathrm{HI}]=\square \)
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The equilibrium concentrations are \( \left[\mathrm{H}_{2}\right] = 0.078 \, \text{M} \), \( \left[\mathrm{I}_{2}\right] = 0.078 \, \text{M} \), and \( [\mathrm{HI}] = 0.588 \, \text{M} \).
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