Final answer:
To calculate the equilibrium constant K for a given reaction, one needs the equilibrium concentrations or pressures of reactants and products. Without such data, it's impossible to calculate k for the reaction COF2(g) ⇌ 1/2 CO2(g) + 1/2 CF4(g). Stoichiometry and the ideal gas law or density are used in similar calculations.
Step-by-step explanation:
The calculation of for a chemical reaction involves the stoichiometry of the reaction and the concentrations of the reactants and products at equilibrium. In practice, you would use the equilibrium concentrations of the products and reactants to calculate Kc or the equilibrium partial pressures to calculate Kp. However, since you have asked about calculating k with respect to the given reaction COF2(g) ⇌ 1/2 CO2(g) + 1/2 CF4(g), without any context of concentrations or pressures, we cannot compute a numerical value for k (the equilibrium constant). An additional clarification on the convention (k, Kc, or Kp) and data regarding the equilibrium state are necessary to proceed with the calculation.
For your reference to similar problems, in the case you provided: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l), the question asks for the volume of CO2 produced when 13.4 g of C4H10 reacts completely. Using stoichiometry, we can calculate the moles of CO2 produced and then apply the ideal gas law or the density of CO2 to find the volume in liters.