For the following reaction, it is found at equilibrium at a certain temperature that the concentrations are [CO(g)] = 2.7 multiplied by 10-4 M, [O2(g)] = 1.9 multiplied by 10-3 M, and [CO2(g)] = 1.1 multiplied by 10-1 M.

K=[CO2]^2/([CO}^2 * [O2]^2 )

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To calculate the equilibrium constant (K) for the given reaction, we need to use the concentrations of the reactants and products at equilibrium as well as the balanced chemical equation.

The balanced chemical equation is:
2 CO(g) + O2(g) ⇌ 2 CO2(g)

K is calculated by dividing the concentration of the products raised to their stoichiometric coefficients by the concentration of the reactants raised to their stoichiometric coefficients.

Let's plug in the given concentrations into the equation and calculate K:

K = [CO2(g)]^2 / ([CO(g)]^2 * [O2(g)])

K = (1.1 × 10^-1 M)^2 / ((2.7 × 10^-4 M)^2 * (1.9 × 10^-3 M))

K ≈ 4.8645 × 10^5

Therefore, the equilibrium constant (K) for the reaction at this temperature is approximately 4.8645 × 10^5.