Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only \( \mathrm{N}_{2} \) and \( \mathrm{H}_{2} \) is reacted in a vessel at high temperature. At equilibrium, the \( 5.0 \mathrm{M} \mathrm{H}_{2} \), \( 8.0 \mathrm{M} \mathrm{N}_{2} \), and \( 4.0 \mathrm{M} \mathrm{NH}_{3} \) are present. Determine the initial concentrations of \( \mathrm{H}_{2} \) and \( \mathrm{N}_{2} \) that were present in the vessel.
\[
\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})
\]
1
Based on the given values, fill in the ICE table to determine concentrations of all reactants and products.
O. RESET