For a chemical reaction $\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}$, the equilibrium concentration of the reactant $\mathrm{C}_{2} \mathrm{H}_{4}$ is given by $0.335-x$ and the equilibrium concentration of the reactant $\mathrm{H}_{2}$ is given by $0.526-x$, where $\frac{x}{(0.335-x)(0.526-x)}=0.990$. Determine the equilibrium concentrations of each reactant.

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The Answer of For a chemical reaction $\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}$, the equilibrium concentration of the reactant $\mathrm{C}_{2} \mathrm{H}_{4}$ is given by $0.335-x$ and the equilibrium concentration of the reactant $\mathrm{H}_{2}$ is given by $0.526-x$, where $\frac{x}{(0.335-x)(0.526-x)}=0.990$. Determine the equilibrium concentrations of each reactant.

For a Chemical Reaction C2H4+H2⇌C2H6\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}C2​H4​+H2​⇌C2​H6​ , the Equilibrium Concentration of the Reactant

For a Chemical Reaction $\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}$ , the Equilibrium Concentration of the Reactant