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H2SO4 + FeCO3 = H2O + CO2 + S + Fe2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + FeCO_3 iron(II) carbonate ⟶ H_2O water + CO_2 carbon dioxide + S mixed sulfur + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate
H_2SO_4 sulfuric acid + FeCO_3 iron(II) carbonate ⟶ H_2O water + CO_2 carbon dioxide + S mixed sulfur + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + FeCO_3 ⟶ H_2O + CO_2 + S + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 S + c_6 Fe_2(SO_4)_3·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, C and Fe: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 12 c_6 S: | c_1 = c_5 + 3 c_6 C: | c_2 = c_4 Fe: | c_2 = 2 c_6 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 6 c_3 = 10 c_4 = 6 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 H_2SO_4 + 6 FeCO_3 ⟶ 10 H_2O + 6 CO_2 + S + 3 Fe_2(SO_4)_3·xH_2O
Balance the chemical equation algebraically: H_2SO_4 + FeCO_3 ⟶ H_2O + CO_2 + S + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 S + c_6 Fe_2(SO_4)_3·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, C and Fe: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 12 c_6 S: | c_1 = c_5 + 3 c_6 C: | c_2 = c_4 Fe: | c_2 = 2 c_6 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 6 c_3 = 10 c_4 = 6 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 H_2SO_4 + 6 FeCO_3 ⟶ 10 H_2O + 6 CO_2 + S + 3 Fe_2(SO_4)_3·xH_2O

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

sulfuric acid + iron(II) carbonate ⟶ water + carbon dioxide + mixed sulfur + iron(III) sulfate hydrate
sulfuric acid + iron(II) carbonate ⟶ water + carbon dioxide + mixed sulfur + iron(III) sulfate hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + FeCO_3 ⟶ H_2O + CO_2 + S + Fe_2(SO_4)_3·xH_2O 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: 10 H_2SO_4 + 6 FeCO_3 ⟶ 10 H_2O + 6 CO_2 + S + 3 Fe_2(SO_4)_3·xH_2O 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 | 10 | -10 FeCO_3 | 6 | -6 H_2O | 10 | 10 CO_2 | 6 | 6 S | 1 | 1 Fe_2(SO_4)_3·xH_2O | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 10 | -10 | ([H2SO4])^(-10) FeCO_3 | 6 | -6 | ([FeCO3])^(-6) H_2O | 10 | 10 | ([H2O])^10 CO_2 | 6 | 6 | ([CO2])^6 S | 1 | 1 | [S] Fe_2(SO_4)_3·xH_2O | 3 | 3 | ([Fe2(SO4)3·xH2O])^3 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])^(-10) ([FeCO3])^(-6) ([H2O])^10 ([CO2])^6 [S] ([Fe2(SO4)3·xH2O])^3 = (([H2O])^10 ([CO2])^6 [S] ([Fe2(SO4)3·xH2O])^3)/(([H2SO4])^10 ([FeCO3])^6)
Construct the equilibrium constant, K, expression for: H_2SO_4 + FeCO_3 ⟶ H_2O + CO_2 + S + Fe_2(SO_4)_3·xH_2O 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: 10 H_2SO_4 + 6 FeCO_3 ⟶ 10 H_2O + 6 CO_2 + S + 3 Fe_2(SO_4)_3·xH_2O 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 | 10 | -10 FeCO_3 | 6 | -6 H_2O | 10 | 10 CO_2 | 6 | 6 S | 1 | 1 Fe_2(SO_4)_3·xH_2O | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 10 | -10 | ([H2SO4])^(-10) FeCO_3 | 6 | -6 | ([FeCO3])^(-6) H_2O | 10 | 10 | ([H2O])^10 CO_2 | 6 | 6 | ([CO2])^6 S | 1 | 1 | [S] Fe_2(SO_4)_3·xH_2O | 3 | 3 | ([Fe2(SO4)3·xH2O])^3 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])^(-10) ([FeCO3])^(-6) ([H2O])^10 ([CO2])^6 [S] ([Fe2(SO4)3·xH2O])^3 = (([H2O])^10 ([CO2])^6 [S] ([Fe2(SO4)3·xH2O])^3)/(([H2SO4])^10 ([FeCO3])^6)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + FeCO_3 ⟶ H_2O + CO_2 + S + Fe_2(SO_4)_3·xH_2O 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: 10 H_2SO_4 + 6 FeCO_3 ⟶ 10 H_2O + 6 CO_2 + S + 3 Fe_2(SO_4)_3·xH_2O 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 | 10 | -10 FeCO_3 | 6 | -6 H_2O | 10 | 10 CO_2 | 6 | 6 S | 1 | 1 Fe_2(SO_4)_3·xH_2O | 3 | 3 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 | 10 | -10 | -1/10 (Δ[H2SO4])/(Δt) FeCO_3 | 6 | -6 | -1/6 (Δ[FeCO3])/(Δt) H_2O | 10 | 10 | 1/10 (Δ[H2O])/(Δt) CO_2 | 6 | 6 | 1/6 (Δ[CO2])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Fe_2(SO_4)_3·xH_2O | 3 | 3 | 1/3 (Δ[Fe2(SO4)3·xH2O])/(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 = -1/10 (Δ[H2SO4])/(Δt) = -1/6 (Δ[FeCO3])/(Δt) = 1/10 (Δ[H2O])/(Δt) = 1/6 (Δ[CO2])/(Δt) = (Δ[S])/(Δt) = 1/3 (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + FeCO_3 ⟶ H_2O + CO_2 + S + Fe_2(SO_4)_3·xH_2O 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: 10 H_2SO_4 + 6 FeCO_3 ⟶ 10 H_2O + 6 CO_2 + S + 3 Fe_2(SO_4)_3·xH_2O 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 | 10 | -10 FeCO_3 | 6 | -6 H_2O | 10 | 10 CO_2 | 6 | 6 S | 1 | 1 Fe_2(SO_4)_3·xH_2O | 3 | 3 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 | 10 | -10 | -1/10 (Δ[H2SO4])/(Δt) FeCO_3 | 6 | -6 | -1/6 (Δ[FeCO3])/(Δt) H_2O | 10 | 10 | 1/10 (Δ[H2O])/(Δt) CO_2 | 6 | 6 | 1/6 (Δ[CO2])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Fe_2(SO_4)_3·xH_2O | 3 | 3 | 1/3 (Δ[Fe2(SO4)3·xH2O])/(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 = -1/10 (Δ[H2SO4])/(Δt) = -1/6 (Δ[FeCO3])/(Δt) = 1/10 (Δ[H2O])/(Δt) = 1/6 (Δ[CO2])/(Δt) = (Δ[S])/(Δt) = 1/3 (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | iron(II) carbonate | water | carbon dioxide | mixed sulfur | iron(III) sulfate hydrate formula | H_2SO_4 | FeCO_3 | H_2O | CO_2 | S | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | CFeO_3 | H_2O | CO_2 | S | Fe_2O_12S_3 name | sulfuric acid | iron(II) carbonate | water | carbon dioxide | mixed sulfur | iron(III) sulfate hydrate IUPAC name | sulfuric acid | ferrous carbonate | water | carbon dioxide | sulfur | diferric trisulfate
| sulfuric acid | iron(II) carbonate | water | carbon dioxide | mixed sulfur | iron(III) sulfate hydrate formula | H_2SO_4 | FeCO_3 | H_2O | CO_2 | S | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | CFeO_3 | H_2O | CO_2 | S | Fe_2O_12S_3 name | sulfuric acid | iron(II) carbonate | water | carbon dioxide | mixed sulfur | iron(III) sulfate hydrate IUPAC name | sulfuric acid | ferrous carbonate | water | carbon dioxide | sulfur | diferric trisulfate

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