Fe + H2O2 = O2 + H2Fe

Fe (iron) + H_2O_2 (hydrogen peroxide) ⟶ O_2 (oxygen) + H2Fe

Balance the chemical equation algebraically: Fe + H_2O_2 ⟶ O_2 + H2Fe Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 H_2O_2 ⟶ c_3 O_2 + c_4 H2Fe 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_4 H: | 2 c_2 = 2 c_4 O: | 2 c_2 = 2 c_3 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 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe + H_2O_2 ⟶ O_2 + H2Fe

+ ⟶ + H2Fe

iron + hydrogen peroxide ⟶ oxygen + H2Fe

Construct the equilibrium constant, K, expression for: Fe + H_2O_2 ⟶ O_2 + H2Fe 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 + H_2O_2 ⟶ O_2 + H2Fe 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 | 1 | -1 H_2O_2 | 1 | -1 O_2 | 1 | 1 H2Fe | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe | 1 | -1 | ([Fe])^(-1) H_2O_2 | 1 | -1 | ([H2O2])^(-1) O_2 | 1 | 1 | [O2] H2Fe | 1 | 1 | [H2Fe] 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])^(-1) ([H2O2])^(-1) [O2] [H2Fe] = ([O2] [H2Fe])/([Fe] [H2O2])

Construct the rate of reaction expression for: Fe + H_2O_2 ⟶ O_2 + H2Fe 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 + H_2O_2 ⟶ O_2 + H2Fe 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 | 1 | -1 H_2O_2 | 1 | -1 O_2 | 1 | 1 H2Fe | 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 | 1 | -1 | -(Δ[Fe])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) H2Fe | 1 | 1 | (Δ[H2Fe])/(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])/(Δt) = -(Δ[H2O2])/(Δt) = (Δ[O2])/(Δt) = (Δ[H2Fe])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron | hydrogen peroxide | oxygen | H2Fe formula | Fe | H_2O_2 | O_2 | H2Fe name | iron | hydrogen peroxide | oxygen | IUPAC name | iron | hydrogen peroxide | molecular oxygen |

| iron | hydrogen peroxide | oxygen | H2Fe molar mass | 55.845 g/mol | 34.014 g/mol | 31.998 g/mol | 57.861 g/mol phase | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | 1535 °C | -0.43 °C | -218 °C | boiling point | 2750 °C | 150.2 °C | -183 °C | density | 7.874 g/cm^3 | 1.44 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | solubility in water | insoluble | miscible | | surface tension | | 0.0804 N/m | 0.01347 N/m | dynamic viscosity | | 0.001249 Pa s (at 20 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless |