FeH2O2 = H2FeO2

Fe(OH)_2 iron(II) hydroxide ⟶ Fe(OH)_2 iron(II) hydroxide

Balance the chemical equation algebraically: Fe(OH)_2 ⟶ Fe(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe(OH)_2 ⟶ c_2 Fe(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, H and O: Fe: | c_1 = c_2 H: | 2 c_1 = 2 c_2 O: | 2 c_1 = 2 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: | | Fe(OH)_2 ⟶ Fe(OH)_2

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iron(II) hydroxide ⟶ iron(II) hydroxide

Construct the equilibrium constant, K, expression for: Fe(OH)_2 ⟶ Fe(OH)_2 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: Fe(OH)_2 ⟶ Fe(OH)_2 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 Fe(OH)_2 | 1 | -1 Fe(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe(OH)_2 | 1 | -1 | ([Fe(OH)2])^(-1) Fe(OH)_2 | 1 | 1 | [Fe(OH)2] 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 = ([Fe(OH)2])^(-1) [Fe(OH)2] = ([Fe(OH)2])/([Fe(OH)2])

Construct the rate of reaction expression for: Fe(OH)_2 ⟶ Fe(OH)_2 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: Fe(OH)_2 ⟶ Fe(OH)_2 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 Fe(OH)_2 | 1 | -1 Fe(OH)_2 | 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 Fe(OH)_2 | 1 | -1 | -(Δ[Fe(OH)2])/(Δt) Fe(OH)_2 | 1 | 1 | (Δ[Fe(OH)2])/(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[Fe(OH)2])/(Δt) = (Δ[Fe(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron(II) hydroxide | iron(II) hydroxide formula | Fe(OH)_2 | Fe(OH)_2 Hill formula | FeH_2O_2 | FeH_2O_2 name | iron(II) hydroxide | iron(II) hydroxide IUPAC name | ferrous dihydroxide | ferrous dihydroxide

| iron(II) hydroxide | iron(II) hydroxide molar mass | 89.86 g/mol | 89.86 g/mol