MnO2 + CO = MnCO3

MnO_2 manganese dioxide + CO carbon monoxide ⟶ MnCO_3 manganese carbonate

Balance the chemical equation algebraically: MnO_2 + CO ⟶ MnCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 MnO_2 + c_2 CO ⟶ c_3 MnCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Mn, O and C: Mn: | c_1 = c_3 O: | 2 c_1 + c_2 = 3 c_3 C: | c_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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | MnO_2 + CO ⟶ MnCO_3

+ ⟶

manganese dioxide + carbon monoxide ⟶ manganese carbonate

Construct the equilibrium constant, K, expression for: MnO_2 + CO ⟶ MnCO_3 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: MnO_2 + CO ⟶ MnCO_3 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 MnO_2 | 1 | -1 CO | 1 | -1 MnCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression MnO_2 | 1 | -1 | ([MnO2])^(-1) CO | 1 | -1 | ([CO])^(-1) MnCO_3 | 1 | 1 | [MnCO3] 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 = ([MnO2])^(-1) ([CO])^(-1) [MnCO3] = ([MnCO3])/([MnO2] [CO])

Construct the rate of reaction expression for: MnO_2 + CO ⟶ MnCO_3 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: MnO_2 + CO ⟶ MnCO_3 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 MnO_2 | 1 | -1 CO | 1 | -1 MnCO_3 | 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 MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) CO | 1 | -1 | -(Δ[CO])/(Δt) MnCO_3 | 1 | 1 | (Δ[MnCO3])/(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[MnO2])/(Δt) = -(Δ[CO])/(Δt) = (Δ[MnCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| manganese dioxide | carbon monoxide | manganese carbonate formula | MnO_2 | CO | MnCO_3 Hill formula | MnO_2 | CO | CMnO_3 name | manganese dioxide | carbon monoxide | manganese carbonate IUPAC name | dioxomanganese | carbon monoxide | manganous carbonate

| manganese dioxide | carbon monoxide | manganese carbonate molar mass | 86.936 g/mol | 28.01 g/mol | 114.95 g/mol phase | solid (at STP) | gas (at STP) | melting point | 535 °C | -205 °C | boiling point | | -191.5 °C | density | 5.03 g/cm^3 | 0.001145 g/cm^3 (at 25 °C) | 3.12 g/cm^3 solubility in water | insoluble | | insoluble dynamic viscosity | | 1.772×10^-5 Pa s (at 25 °C) | odor | | odorless |