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H2SO4 + MnO2 + (COOH)2 = H2O + CO2 + MnSO4

Input interpretation

H_2SO_4 sulfuric acid + MnO_2 manganese dioxide + HO_2CCO_2H oxalic acid ⟶ H_2O water + CO_2 carbon dioxide + MnSO_4 manganese(II) sulfate
H_2SO_4 sulfuric acid + MnO_2 manganese dioxide + HO_2CCO_2H oxalic acid ⟶ H_2O water + CO_2 carbon dioxide + MnSO_4 manganese(II) sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ H_2O + CO_2 + MnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 MnO_2 + c_3 HO_2CCO_2H ⟶ c_4 H_2O + c_5 CO_2 + c_6 MnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Mn and C: H: | 2 c_1 + 2 c_3 = 2 c_4 O: | 4 c_1 + 2 c_2 + 4 c_3 = c_4 + 2 c_5 + 4 c_6 S: | c_1 = c_6 Mn: | c_2 = c_6 C: | 2 c_3 = c_5 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 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ 2 H_2O + 2 CO_2 + MnSO_4
Balance the chemical equation algebraically: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ H_2O + CO_2 + MnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 MnO_2 + c_3 HO_2CCO_2H ⟶ c_4 H_2O + c_5 CO_2 + c_6 MnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Mn and C: H: | 2 c_1 + 2 c_3 = 2 c_4 O: | 4 c_1 + 2 c_2 + 4 c_3 = c_4 + 2 c_5 + 4 c_6 S: | c_1 = c_6 Mn: | c_2 = c_6 C: | 2 c_3 = c_5 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 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ 2 H_2O + 2 CO_2 + MnSO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

sulfuric acid + manganese dioxide + oxalic acid ⟶ water + carbon dioxide + manganese(II) sulfate
sulfuric acid + manganese dioxide + oxalic acid ⟶ water + carbon dioxide + manganese(II) sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ H_2O + CO_2 + MnSO_4 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: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ 2 H_2O + 2 CO_2 + MnSO_4 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 H_2SO_4 | 1 | -1 MnO_2 | 1 | -1 HO_2CCO_2H | 1 | -1 H_2O | 2 | 2 CO_2 | 2 | 2 MnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) MnO_2 | 1 | -1 | ([MnO2])^(-1) HO_2CCO_2H | 1 | -1 | ([HO2CCO2H])^(-1) H_2O | 2 | 2 | ([H2O])^2 CO_2 | 2 | 2 | ([CO2])^2 MnSO_4 | 1 | 1 | [MnSO4] 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 = ([H2SO4])^(-1) ([MnO2])^(-1) ([HO2CCO2H])^(-1) ([H2O])^2 ([CO2])^2 [MnSO4] = (([H2O])^2 ([CO2])^2 [MnSO4])/([H2SO4] [MnO2] [HO2CCO2H])
Construct the equilibrium constant, K, expression for: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ H_2O + CO_2 + MnSO_4 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: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ 2 H_2O + 2 CO_2 + MnSO_4 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 H_2SO_4 | 1 | -1 MnO_2 | 1 | -1 HO_2CCO_2H | 1 | -1 H_2O | 2 | 2 CO_2 | 2 | 2 MnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) MnO_2 | 1 | -1 | ([MnO2])^(-1) HO_2CCO_2H | 1 | -1 | ([HO2CCO2H])^(-1) H_2O | 2 | 2 | ([H2O])^2 CO_2 | 2 | 2 | ([CO2])^2 MnSO_4 | 1 | 1 | [MnSO4] 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 = ([H2SO4])^(-1) ([MnO2])^(-1) ([HO2CCO2H])^(-1) ([H2O])^2 ([CO2])^2 [MnSO4] = (([H2O])^2 ([CO2])^2 [MnSO4])/([H2SO4] [MnO2] [HO2CCO2H])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ H_2O + CO_2 + MnSO_4 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: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ 2 H_2O + 2 CO_2 + MnSO_4 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 H_2SO_4 | 1 | -1 MnO_2 | 1 | -1 HO_2CCO_2H | 1 | -1 H_2O | 2 | 2 CO_2 | 2 | 2 MnSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) HO_2CCO_2H | 1 | -1 | -(Δ[HO2CCO2H])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) MnSO_4 | 1 | 1 | (Δ[MnSO4])/(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[H2SO4])/(Δt) = -(Δ[MnO2])/(Δt) = -(Δ[HO2CCO2H])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[CO2])/(Δt) = (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ H_2O + CO_2 + MnSO_4 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: H_2SO_4 + MnO_2 + HO_2CCO_2H ⟶ 2 H_2O + 2 CO_2 + MnSO_4 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 H_2SO_4 | 1 | -1 MnO_2 | 1 | -1 HO_2CCO_2H | 1 | -1 H_2O | 2 | 2 CO_2 | 2 | 2 MnSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) HO_2CCO_2H | 1 | -1 | -(Δ[HO2CCO2H])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) MnSO_4 | 1 | 1 | (Δ[MnSO4])/(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[H2SO4])/(Δt) = -(Δ[MnO2])/(Δt) = -(Δ[HO2CCO2H])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[CO2])/(Δt) = (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | manganese dioxide | oxalic acid | water | carbon dioxide | manganese(II) sulfate formula | H_2SO_4 | MnO_2 | HO_2CCO_2H | H_2O | CO_2 | MnSO_4 Hill formula | H_2O_4S | MnO_2 | C_2H_2O_4 | H_2O | CO_2 | MnSO_4 name | sulfuric acid | manganese dioxide | oxalic acid | water | carbon dioxide | manganese(II) sulfate IUPAC name | sulfuric acid | dioxomanganese | oxalic acid | water | carbon dioxide | manganese(+2) cation sulfate
| sulfuric acid | manganese dioxide | oxalic acid | water | carbon dioxide | manganese(II) sulfate formula | H_2SO_4 | MnO_2 | HO_2CCO_2H | H_2O | CO_2 | MnSO_4 Hill formula | H_2O_4S | MnO_2 | C_2H_2O_4 | H_2O | CO_2 | MnSO_4 name | sulfuric acid | manganese dioxide | oxalic acid | water | carbon dioxide | manganese(II) sulfate IUPAC name | sulfuric acid | dioxomanganese | oxalic acid | water | carbon dioxide | manganese(+2) cation sulfate

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