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K=[CO2]^2/([CO}^2 * [O2]^2 )
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2 CO(g) + O2(g) reverse reaction arrow 2 CO2(g)
Calculate K for the reaction at this temperature.
Is there a reason you can't do the math?
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.