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FeCl2 + Ba(OH)2 = BaCl2 + Fe(OH)2

Input interpretation

FeCl_2 iron(II) chloride + Ba(OH)_2 barium hydroxide ⟶ BaCl_2 barium chloride + Fe(OH)_2 iron(II) hydroxide
FeCl_2 iron(II) chloride + Ba(OH)_2 barium hydroxide ⟶ BaCl_2 barium chloride + Fe(OH)_2 iron(II) hydroxide

Balanced equation

Balance the chemical equation algebraically: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeCl_2 + c_2 Ba(OH)_2 ⟶ c_3 BaCl_2 + c_4 Fe(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Fe, Ba, H and O: Cl: | 2 c_1 = 2 c_3 Fe: | c_1 = c_4 Ba: | c_2 = c_3 H: | 2 c_2 = 2 c_4 O: | 2 c_2 = 2 c_4 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2
Balance the chemical equation algebraically: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeCl_2 + c_2 Ba(OH)_2 ⟶ c_3 BaCl_2 + c_4 Fe(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Fe, Ba, H and O: Cl: | 2 c_1 = 2 c_3 Fe: | c_1 = c_4 Ba: | c_2 = c_3 H: | 2 c_2 = 2 c_4 O: | 2 c_2 = 2 c_4 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2

Structures

+ ⟶ +
+ ⟶ +

Names

iron(II) chloride + barium hydroxide ⟶ barium chloride + iron(II) hydroxide
iron(II) chloride + barium hydroxide ⟶ barium chloride + iron(II) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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 FeCl_2 | 1 | -1 Ba(OH)_2 | 1 | -1 BaCl_2 | 1 | 1 Fe(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeCl_2 | 1 | -1 | ([FeCl2])^(-1) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) BaCl_2 | 1 | 1 | [BaCl2] Fe(OH)_2 | 1 | 1 | [Fe(OH)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 = ([FeCl2])^(-1) ([Ba(OH)2])^(-1) [BaCl2] [Fe(OH)2] = ([BaCl2] [Fe(OH)2])/([FeCl2] [Ba(OH)2])
Construct the equilibrium constant, K, expression for: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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 FeCl_2 | 1 | -1 Ba(OH)_2 | 1 | -1 BaCl_2 | 1 | 1 Fe(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeCl_2 | 1 | -1 | ([FeCl2])^(-1) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) BaCl_2 | 1 | 1 | [BaCl2] Fe(OH)_2 | 1 | 1 | [Fe(OH)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 = ([FeCl2])^(-1) ([Ba(OH)2])^(-1) [BaCl2] [Fe(OH)2] = ([BaCl2] [Fe(OH)2])/([FeCl2] [Ba(OH)2])

Rate of reaction

Construct the rate of reaction expression for: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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 FeCl_2 | 1 | -1 Ba(OH)_2 | 1 | -1 BaCl_2 | 1 | 1 Fe(OH)_2 | 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 FeCl_2 | 1 | -1 | -(Δ[FeCl2])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) BaCl_2 | 1 | 1 | (Δ[BaCl2])/(Δt) Fe(OH)_2 | 1 | 1 | (Δ[Fe(OH)2])/(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[FeCl2])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = (Δ[BaCl2])/(Δt) = (Δ[Fe(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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: FeCl_2 + Ba(OH)_2 ⟶ BaCl_2 + Fe(OH)_2 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 FeCl_2 | 1 | -1 Ba(OH)_2 | 1 | -1 BaCl_2 | 1 | 1 Fe(OH)_2 | 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 FeCl_2 | 1 | -1 | -(Δ[FeCl2])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) BaCl_2 | 1 | 1 | (Δ[BaCl2])/(Δt) Fe(OH)_2 | 1 | 1 | (Δ[Fe(OH)2])/(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[FeCl2])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = (Δ[BaCl2])/(Δt) = (Δ[Fe(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iron(II) chloride | barium hydroxide | barium chloride | iron(II) hydroxide formula | FeCl_2 | Ba(OH)_2 | BaCl_2 | Fe(OH)_2 Hill formula | Cl_2Fe | BaH_2O_2 | BaCl_2 | FeH_2O_2 name | iron(II) chloride | barium hydroxide | barium chloride | iron(II) hydroxide IUPAC name | dichloroiron | barium(+2) cation dihydroxide | barium(+2) cation dichloride | ferrous dihydroxide
| iron(II) chloride | barium hydroxide | barium chloride | iron(II) hydroxide formula | FeCl_2 | Ba(OH)_2 | BaCl_2 | Fe(OH)_2 Hill formula | Cl_2Fe | BaH_2O_2 | BaCl_2 | FeH_2O_2 name | iron(II) chloride | barium hydroxide | barium chloride | iron(II) hydroxide IUPAC name | dichloroiron | barium(+2) cation dihydroxide | barium(+2) cation dichloride | ferrous dihydroxide

Substance properties

| iron(II) chloride | barium hydroxide | barium chloride | iron(II) hydroxide molar mass | 126.7 g/mol | 171.34 g/mol | 208.2 g/mol | 89.86 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 677 °C | 300 °C | 963 °C | density | 3.16 g/cm^3 | 2.2 g/cm^3 | 3.856 g/cm^3 | odor | | | odorless |
| iron(II) chloride | barium hydroxide | barium chloride | iron(II) hydroxide molar mass | 126.7 g/mol | 171.34 g/mol | 208.2 g/mol | 89.86 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 677 °C | 300 °C | 963 °C | density | 3.16 g/cm^3 | 2.2 g/cm^3 | 3.856 g/cm^3 | odor | | | odorless |

Units

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