Calculate the equilibrium constant for the following two reactions. The equilibrium concentration of each reactant and product is given in the box below the reaction. Rank the extent of each reaction at equilibrium by calculating the equilibrium constant. Note that the "extent of each reaction" refers to how much reactant is converted to product at equilibrium.

Reaction $1$:

$CO(g)+O_2(g)2C{O}_2(g)$

Equilibrium concentrations

$[CO]=1\mathrm{.}1M$

$[O_2]=1\mathrm{.}1M$

$[C{O}_2]=8\mathrm{.}3M$

Reaction $2$:

$2N_2(g)+O_2(g)2N{O}_2(g)$

Equilibrium concentrations

$[N_2]=1\mathrm{.}9M$

$[O_2]=2\mathrm{.}5M$

$[N{O}_2]=0\mathrm{.}03M$

Compare $K_c$ values to indicate which reaction proceeds to a greater extent at equilibrium.

View Available Hint$($s$)$

Reaction $2,$ with $K_c=1\mathrm{.}0{10}^4>$ Reaction $1,$ with $K_c=1\mathrm{.}8{10}^{-2}$

Reaction $1,$ with $K_c=56\mathrm{.}9>$ Reaction $2,$ with $K_c=1\mathrm{.}0{10}^{-4}$

Reaction $1,$ with $K_c=6\mathrm{.}86>$ Reaction $2,$ with $K_c=6\mathrm{.}3{10}^{-3}$

Reaction $2,$ with $K_c=56\mathrm{.}9>$ Reaction $1,$ with $K_c=1\mathrm{.}0{10}^{-4}$