Mn2O2 = MnO

Mn2O2 ⟶ MnO manganese monoxide

Balance the chemical equation algebraically: Mn2O2 ⟶ MnO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Mn2O2 ⟶ c_2 MnO Set the number of atoms in the reactants equal to the number of atoms in the products for Mn and O: Mn: | 2 c_1 = c_2 O: | 2 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Mn2O2 ⟶ 2 MnO

Mn2O2 ⟶

Mn2O2 ⟶ manganese monoxide

Construct the equilibrium constant, K, expression for: Mn2O2 ⟶ MnO 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: Mn2O2 ⟶ 2 MnO 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 Mn2O2 | 1 | -1 MnO | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Mn2O2 | 1 | -1 | ([Mn2O2])^(-1) MnO | 2 | 2 | ([MnO])^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 = ([Mn2O2])^(-1) ([MnO])^2 = ([MnO])^2/([Mn2O2])

Construct the rate of reaction expression for: Mn2O2 ⟶ MnO 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: Mn2O2 ⟶ 2 MnO 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 Mn2O2 | 1 | -1 MnO | 2 | 2 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 Mn2O2 | 1 | -1 | -(Δ[Mn2O2])/(Δt) MnO | 2 | 2 | 1/2 (Δ[MnO])/(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[Mn2O2])/(Δt) = 1/2 (Δ[MnO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| Mn2O2 | manganese monoxide formula | Mn2O2 | MnO name | | manganese monoxide IUPAC name | | oxomanganese

| Mn2O2 | manganese monoxide molar mass | 141.874 g/mol | 70.937 g/mol phase | | solid (at STP) melting point | | 1840 °C density | | 5.45 g/cm^3 solubility in water | | insoluble