Search

H2SO4 + FeCl2 = H2O + SO2 + FeCl3 + Fe2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + FeCl_2 iron(II) chloride ⟶ H_2O water + SO_2 sulfur dioxide + FeCl_3 iron(III) chloride + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate
H_2SO_4 sulfuric acid + FeCl_2 iron(II) chloride ⟶ H_2O water + SO_2 sulfur dioxide + FeCl_3 iron(III) chloride + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + FeCl_2 ⟶ H_2O + SO_2 + FeCl_3 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeCl_2 ⟶ c_3 H_2O + c_4 SO_2 + c_5 FeCl_3 + 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, Cl and Fe: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = c_3 + 2 c_4 + 12 c_6 S: | c_1 = c_4 + 3 c_6 Cl: | 2 c_2 = 3 c_5 Fe: | c_2 = c_5 + 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 6 c_4 = 3 c_5 = 4 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 H_2SO_4 + 6 FeCl_2 ⟶ 6 H_2O + 3 SO_2 + 4 FeCl_3 + Fe_2(SO_4)_3·xH_2O
Balance the chemical equation algebraically: H_2SO_4 + FeCl_2 ⟶ H_2O + SO_2 + FeCl_3 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeCl_2 ⟶ c_3 H_2O + c_4 SO_2 + c_5 FeCl_3 + 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, Cl and Fe: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = c_3 + 2 c_4 + 12 c_6 S: | c_1 = c_4 + 3 c_6 Cl: | 2 c_2 = 3 c_5 Fe: | c_2 = c_5 + 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 6 c_4 = 3 c_5 = 4 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 H_2SO_4 + 6 FeCl_2 ⟶ 6 H_2O + 3 SO_2 + 4 FeCl_3 + Fe_2(SO_4)_3·xH_2O

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

sulfuric acid + iron(II) chloride ⟶ water + sulfur dioxide + iron(III) chloride + iron(III) sulfate hydrate
sulfuric acid + iron(II) chloride ⟶ water + sulfur dioxide + iron(III) chloride + iron(III) sulfate hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + FeCl_2 ⟶ H_2O + SO_2 + FeCl_3 + 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: 6 H_2SO_4 + 6 FeCl_2 ⟶ 6 H_2O + 3 SO_2 + 4 FeCl_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 | 6 | -6 FeCl_2 | 6 | -6 H_2O | 6 | 6 SO_2 | 3 | 3 FeCl_3 | 4 | 4 Fe_2(SO_4)_3·xH_2O | 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 | 6 | -6 | ([H2SO4])^(-6) FeCl_2 | 6 | -6 | ([FeCl2])^(-6) H_2O | 6 | 6 | ([H2O])^6 SO_2 | 3 | 3 | ([SO2])^3 FeCl_3 | 4 | 4 | ([FeCl3])^4 Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] 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])^(-6) ([FeCl2])^(-6) ([H2O])^6 ([SO2])^3 ([FeCl3])^4 [Fe2(SO4)3·xH2O] = (([H2O])^6 ([SO2])^3 ([FeCl3])^4 [Fe2(SO4)3·xH2O])/(([H2SO4])^6 ([FeCl2])^6)
Construct the equilibrium constant, K, expression for: H_2SO_4 + FeCl_2 ⟶ H_2O + SO_2 + FeCl_3 + 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: 6 H_2SO_4 + 6 FeCl_2 ⟶ 6 H_2O + 3 SO_2 + 4 FeCl_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 | 6 | -6 FeCl_2 | 6 | -6 H_2O | 6 | 6 SO_2 | 3 | 3 FeCl_3 | 4 | 4 Fe_2(SO_4)_3·xH_2O | 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 | 6 | -6 | ([H2SO4])^(-6) FeCl_2 | 6 | -6 | ([FeCl2])^(-6) H_2O | 6 | 6 | ([H2O])^6 SO_2 | 3 | 3 | ([SO2])^3 FeCl_3 | 4 | 4 | ([FeCl3])^4 Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] 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])^(-6) ([FeCl2])^(-6) ([H2O])^6 ([SO2])^3 ([FeCl3])^4 [Fe2(SO4)3·xH2O] = (([H2O])^6 ([SO2])^3 ([FeCl3])^4 [Fe2(SO4)3·xH2O])/(([H2SO4])^6 ([FeCl2])^6)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + FeCl_2 ⟶ H_2O + SO_2 + FeCl_3 + 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: 6 H_2SO_4 + 6 FeCl_2 ⟶ 6 H_2O + 3 SO_2 + 4 FeCl_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 | 6 | -6 FeCl_2 | 6 | -6 H_2O | 6 | 6 SO_2 | 3 | 3 FeCl_3 | 4 | 4 Fe_2(SO_4)_3·xH_2O | 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 | 6 | -6 | -1/6 (Δ[H2SO4])/(Δt) FeCl_2 | 6 | -6 | -1/6 (Δ[FeCl2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) SO_2 | 3 | 3 | 1/3 (Δ[SO2])/(Δt) FeCl_3 | 4 | 4 | 1/4 (Δ[FeCl3])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (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 = -1/6 (Δ[H2SO4])/(Δt) = -1/6 (Δ[FeCl2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/3 (Δ[SO2])/(Δt) = 1/4 (Δ[FeCl3])/(Δt) = (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 + FeCl_2 ⟶ H_2O + SO_2 + FeCl_3 + 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: 6 H_2SO_4 + 6 FeCl_2 ⟶ 6 H_2O + 3 SO_2 + 4 FeCl_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 | 6 | -6 FeCl_2 | 6 | -6 H_2O | 6 | 6 SO_2 | 3 | 3 FeCl_3 | 4 | 4 Fe_2(SO_4)_3·xH_2O | 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 | 6 | -6 | -1/6 (Δ[H2SO4])/(Δt) FeCl_2 | 6 | -6 | -1/6 (Δ[FeCl2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) SO_2 | 3 | 3 | 1/3 (Δ[SO2])/(Δt) FeCl_3 | 4 | 4 | 1/4 (Δ[FeCl3])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (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 = -1/6 (Δ[H2SO4])/(Δt) = -1/6 (Δ[FeCl2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/3 (Δ[SO2])/(Δt) = 1/4 (Δ[FeCl3])/(Δt) = (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) chloride | water | sulfur dioxide | iron(III) chloride | iron(III) sulfate hydrate formula | H_2SO_4 | FeCl_2 | H_2O | SO_2 | FeCl_3 | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | Cl_2Fe | H_2O | O_2S | Cl_3Fe | Fe_2O_12S_3 name | sulfuric acid | iron(II) chloride | water | sulfur dioxide | iron(III) chloride | iron(III) sulfate hydrate IUPAC name | sulfuric acid | dichloroiron | water | sulfur dioxide | trichloroiron | diferric trisulfate
| sulfuric acid | iron(II) chloride | water | sulfur dioxide | iron(III) chloride | iron(III) sulfate hydrate formula | H_2SO_4 | FeCl_2 | H_2O | SO_2 | FeCl_3 | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | Cl_2Fe | H_2O | O_2S | Cl_3Fe | Fe_2O_12S_3 name | sulfuric acid | iron(II) chloride | water | sulfur dioxide | iron(III) chloride | iron(III) sulfate hydrate IUPAC name | sulfuric acid | dichloroiron | water | sulfur dioxide | trichloroiron | diferric trisulfate

Random Queries

alternate names of cobalt(II) cation vs lead(II) cation
color of calcium vs sulfur
chemical types of propadiene vs dioxybenzone
alternate names of gallium(I) cation
ion class of chromium(III) cation vs palladium(I) cation
atomic mass of period 1 elements
alternate names of manganate anion
CID choline glycerophosphate
formula of tin(II) cation vs stannite anion
atomic spectrum of tantalum