Calculate the equilibrium constant for 2CH3OH(l)+3O2(g)->2CO2(g)+4H2O(l)
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To calculate the equilibrium constant for the given reaction, you need to know the concentrations of the reactants and products at equilibrium. The equilibrium constant (K) is defined as the ratio of the concentrations of the products to the concentrations of the reactants, where each concentration is raised to the power of its stoichiometric coefficient in the balanced chemical equation.
The given equation is 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l).
Let's assume that at equilibrium, the concentrations of CH3OH, O2, CO2, and H2O are [CH3OH], [O2], [CO2], and [H2O], respectively.
The equilibrium constant expression is:
K_eq = ([CO2]^2 * [H2O]^4) / ([CH3OH]^2 * [O2]^3)
Since this is a gas phase reaction, we can also express the concentrations using partial pressures, denoted as P.
K_p = (P_CO2^2 * P_H2O^4) / (P_CH3OH^2 * P_O2^3)
The concentrations or partial pressures must be in units consistent with the balanced equation. For example, if the equation is balanced using the units of moles per liter (M) for concentrations, then the concentrations must be in moles per liter. Similarly, if the equation is balanced using the units of atmospheres (atm) for partial pressures, then the partial pressures must be in atmospheres.
To calculate the equilibrium constant numerically, you need experimental data or information about the initial and equilibrium concentrations or partial pressures. With this information, substitute the values into the equilibrium constant expression and calculate the value of K.