FeCO = FeOC

FeCO ⟶ FeOC

Balance the chemical equation algebraically: FeCO ⟶ FeOC Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeCO ⟶ c_2 FeOC Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, C and O: Fe: | c_1 = c_2 C: | c_1 = c_2 O: | c_1 = c_2 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeCO ⟶ FeOC

FeCO ⟶ FeOC

FeCO ⟶ FeOC

Construct the equilibrium constant, K, expression for: FeCO ⟶ FeOC Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: FeCO ⟶ FeOC Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i FeCO | 1 | -1 FeOC | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeCO | 1 | -1 | ([FeCO])^(-1) FeOC | 1 | 1 | [FeOC] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([FeCO])^(-1) [FeOC] = ([FeOC])/([FeCO])

Construct the rate of reaction expression for: FeCO ⟶ FeOC Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: FeCO ⟶ FeOC Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i FeCO | 1 | -1 FeOC | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term FeCO | 1 | -1 | -(Δ[FeCO])/(Δt) FeOC | 1 | 1 | (Δ[FeOC])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[FeCO])/(Δt) = (Δ[FeOC])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| FeCO | FeOC formula | FeCO | FeOC Hill formula | CFeO | CFeO

| FeCO | FeOC molar mass | 83.855 g/mol | 83.855 g/mol