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Ca(OH)2 + FeCl3 = CaCl2 + Fe(OH)3

Input interpretation

Ca(OH)_2 calcium hydroxide + FeCl_3 iron(III) chloride ⟶ CaCl_2 calcium chloride + Fe(OH)_3 iron(III) hydroxide
Ca(OH)_2 calcium hydroxide + FeCl_3 iron(III) chloride ⟶ CaCl_2 calcium chloride + Fe(OH)_3 iron(III) hydroxide

Balanced equation

Balance the chemical equation algebraically: Ca(OH)_2 + FeCl_3 ⟶ CaCl_2 + Fe(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(OH)_2 + c_2 FeCl_3 ⟶ c_3 CaCl_2 + c_4 Fe(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, O, Cl and Fe: Ca: | c_1 = c_3 H: | 2 c_1 = 3 c_4 O: | 2 c_1 = 3 c_4 Cl: | 3 c_2 = 2 c_3 Fe: | c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 1 c_3 = 3/2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Ca(OH)_2 + 2 FeCl_3 ⟶ 3 CaCl_2 + 2 Fe(OH)_3
Balance the chemical equation algebraically: Ca(OH)_2 + FeCl_3 ⟶ CaCl_2 + Fe(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(OH)_2 + c_2 FeCl_3 ⟶ c_3 CaCl_2 + c_4 Fe(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, O, Cl and Fe: Ca: | c_1 = c_3 H: | 2 c_1 = 3 c_4 O: | 2 c_1 = 3 c_4 Cl: | 3 c_2 = 2 c_3 Fe: | c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 1 c_3 = 3/2 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Ca(OH)_2 + 2 FeCl_3 ⟶ 3 CaCl_2 + 2 Fe(OH)_3

Structures

+ ⟶ +
+ ⟶ +

Names

calcium hydroxide + iron(III) chloride ⟶ calcium chloride + iron(III) hydroxide
calcium hydroxide + iron(III) chloride ⟶ calcium chloride + iron(III) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: Ca(OH)_2 + FeCl_3 ⟶ CaCl_2 + Fe(OH)_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: 3 Ca(OH)_2 + 2 FeCl_3 ⟶ 3 CaCl_2 + 2 Fe(OH)_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 Ca(OH)_2 | 3 | -3 FeCl_3 | 2 | -2 CaCl_2 | 3 | 3 Fe(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(OH)_2 | 3 | -3 | ([Ca(OH)2])^(-3) FeCl_3 | 2 | -2 | ([FeCl3])^(-2) CaCl_2 | 3 | 3 | ([CaCl2])^3 Fe(OH)_3 | 2 | 2 | ([Fe(OH)3])^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 = ([Ca(OH)2])^(-3) ([FeCl3])^(-2) ([CaCl2])^3 ([Fe(OH)3])^2 = (([CaCl2])^3 ([Fe(OH)3])^2)/(([Ca(OH)2])^3 ([FeCl3])^2)
Construct the equilibrium constant, K, expression for: Ca(OH)_2 + FeCl_3 ⟶ CaCl_2 + Fe(OH)_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: 3 Ca(OH)_2 + 2 FeCl_3 ⟶ 3 CaCl_2 + 2 Fe(OH)_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 Ca(OH)_2 | 3 | -3 FeCl_3 | 2 | -2 CaCl_2 | 3 | 3 Fe(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(OH)_2 | 3 | -3 | ([Ca(OH)2])^(-3) FeCl_3 | 2 | -2 | ([FeCl3])^(-2) CaCl_2 | 3 | 3 | ([CaCl2])^3 Fe(OH)_3 | 2 | 2 | ([Fe(OH)3])^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 = ([Ca(OH)2])^(-3) ([FeCl3])^(-2) ([CaCl2])^3 ([Fe(OH)3])^2 = (([CaCl2])^3 ([Fe(OH)3])^2)/(([Ca(OH)2])^3 ([FeCl3])^2)

Rate of reaction

Construct the rate of reaction expression for: Ca(OH)_2 + FeCl_3 ⟶ CaCl_2 + Fe(OH)_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: 3 Ca(OH)_2 + 2 FeCl_3 ⟶ 3 CaCl_2 + 2 Fe(OH)_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 Ca(OH)_2 | 3 | -3 FeCl_3 | 2 | -2 CaCl_2 | 3 | 3 Fe(OH)_3 | 2 | 2 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 Ca(OH)_2 | 3 | -3 | -1/3 (Δ[Ca(OH)2])/(Δt) FeCl_3 | 2 | -2 | -1/2 (Δ[FeCl3])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(Δt) Fe(OH)_3 | 2 | 2 | 1/2 (Δ[Fe(OH)3])/(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 = -1/3 (Δ[Ca(OH)2])/(Δt) = -1/2 (Δ[FeCl3])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) = 1/2 (Δ[Fe(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Ca(OH)_2 + FeCl_3 ⟶ CaCl_2 + Fe(OH)_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: 3 Ca(OH)_2 + 2 FeCl_3 ⟶ 3 CaCl_2 + 2 Fe(OH)_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 Ca(OH)_2 | 3 | -3 FeCl_3 | 2 | -2 CaCl_2 | 3 | 3 Fe(OH)_3 | 2 | 2 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 Ca(OH)_2 | 3 | -3 | -1/3 (Δ[Ca(OH)2])/(Δt) FeCl_3 | 2 | -2 | -1/2 (Δ[FeCl3])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(Δt) Fe(OH)_3 | 2 | 2 | 1/2 (Δ[Fe(OH)3])/(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 = -1/3 (Δ[Ca(OH)2])/(Δt) = -1/2 (Δ[FeCl3])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) = 1/2 (Δ[Fe(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| calcium hydroxide | iron(III) chloride | calcium chloride | iron(III) hydroxide formula | Ca(OH)_2 | FeCl_3 | CaCl_2 | Fe(OH)_3 Hill formula | CaH_2O_2 | Cl_3Fe | CaCl_2 | FeH_3O_3 name | calcium hydroxide | iron(III) chloride | calcium chloride | iron(III) hydroxide IUPAC name | calcium dihydroxide | trichloroiron | calcium dichloride | ferric trihydroxide
| calcium hydroxide | iron(III) chloride | calcium chloride | iron(III) hydroxide formula | Ca(OH)_2 | FeCl_3 | CaCl_2 | Fe(OH)_3 Hill formula | CaH_2O_2 | Cl_3Fe | CaCl_2 | FeH_3O_3 name | calcium hydroxide | iron(III) chloride | calcium chloride | iron(III) hydroxide IUPAC name | calcium dihydroxide | trichloroiron | calcium dichloride | ferric trihydroxide

Substance properties

| calcium hydroxide | iron(III) chloride | calcium chloride | iron(III) hydroxide molar mass | 74.092 g/mol | 162.2 g/mol | 111 g/mol | 106.87 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 550 °C | 304 °C | 772 °C | density | 2.24 g/cm^3 | | 2.15 g/cm^3 | solubility in water | slightly soluble | | soluble | odor | odorless | | |
| calcium hydroxide | iron(III) chloride | calcium chloride | iron(III) hydroxide molar mass | 74.092 g/mol | 162.2 g/mol | 111 g/mol | 106.87 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 550 °C | 304 °C | 772 °C | density | 2.24 g/cm^3 | | 2.15 g/cm^3 | solubility in water | slightly soluble | | soluble | odor | odorless | | |

Units

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