Input interpretation
![HI hydrogen iodide + Fe(OH)_3 iron(III) hydroxide ⟶ H_2O water + FeI3](../image_source/0231ff5325d444d7a898017b01658677.png)
HI hydrogen iodide + Fe(OH)_3 iron(III) hydroxide ⟶ H_2O water + FeI3
Balanced equation
![Balance the chemical equation algebraically: HI + Fe(OH)_3 ⟶ H_2O + FeI3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HI + c_2 Fe(OH)_3 ⟶ c_3 H_2O + c_4 FeI3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, I, Fe and O: H: | c_1 + 3 c_2 = 2 c_3 I: | c_1 = 3 c_4 Fe: | c_2 = c_4 O: | 3 c_2 = c_3 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 c_2 = 1 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 HI + Fe(OH)_3 ⟶ 3 H_2O + FeI3](../image_source/6ad372c21c50d72a49e83c7d78f44f09.png)
Balance the chemical equation algebraically: HI + Fe(OH)_3 ⟶ H_2O + FeI3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HI + c_2 Fe(OH)_3 ⟶ c_3 H_2O + c_4 FeI3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, I, Fe and O: H: | c_1 + 3 c_2 = 2 c_3 I: | c_1 = 3 c_4 Fe: | c_2 = c_4 O: | 3 c_2 = c_3 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 c_2 = 1 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 HI + Fe(OH)_3 ⟶ 3 H_2O + FeI3
Structures
![+ ⟶ + FeI3](../image_source/b911418a8109b327df7f61b62481777b.png)
+ ⟶ + FeI3
Names
![hydrogen iodide + iron(III) hydroxide ⟶ water + FeI3](../image_source/7a7605255512c56083281f2324d45ced.png)
hydrogen iodide + iron(III) hydroxide ⟶ water + FeI3
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HI + Fe(OH)_3 ⟶ H_2O + FeI3 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 HI + Fe(OH)_3 ⟶ 3 H_2O + FeI3 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 HI | 3 | -3 Fe(OH)_3 | 1 | -1 H_2O | 3 | 3 FeI3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HI | 3 | -3 | ([HI])^(-3) Fe(OH)_3 | 1 | -1 | ([Fe(OH)3])^(-1) H_2O | 3 | 3 | ([H2O])^3 FeI3 | 1 | 1 | [FeI3] 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 = ([HI])^(-3) ([Fe(OH)3])^(-1) ([H2O])^3 [FeI3] = (([H2O])^3 [FeI3])/(([HI])^3 [Fe(OH)3])](../image_source/0dffac45c0679719342ae415dd184b3e.png)
Construct the equilibrium constant, K, expression for: HI + Fe(OH)_3 ⟶ H_2O + FeI3 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 HI + Fe(OH)_3 ⟶ 3 H_2O + FeI3 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 HI | 3 | -3 Fe(OH)_3 | 1 | -1 H_2O | 3 | 3 FeI3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HI | 3 | -3 | ([HI])^(-3) Fe(OH)_3 | 1 | -1 | ([Fe(OH)3])^(-1) H_2O | 3 | 3 | ([H2O])^3 FeI3 | 1 | 1 | [FeI3] 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 = ([HI])^(-3) ([Fe(OH)3])^(-1) ([H2O])^3 [FeI3] = (([H2O])^3 [FeI3])/(([HI])^3 [Fe(OH)3])
Rate of reaction
![Construct the rate of reaction expression for: HI + Fe(OH)_3 ⟶ H_2O + FeI3 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 HI + Fe(OH)_3 ⟶ 3 H_2O + FeI3 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 HI | 3 | -3 Fe(OH)_3 | 1 | -1 H_2O | 3 | 3 FeI3 | 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 HI | 3 | -3 | -1/3 (Δ[HI])/(Δt) Fe(OH)_3 | 1 | -1 | -(Δ[Fe(OH)3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) FeI3 | 1 | 1 | (Δ[FeI3])/(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[HI])/(Δt) = -(Δ[Fe(OH)3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[FeI3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/68c51221ad659a34d6266aedec33090a.png)
Construct the rate of reaction expression for: HI + Fe(OH)_3 ⟶ H_2O + FeI3 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 HI + Fe(OH)_3 ⟶ 3 H_2O + FeI3 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 HI | 3 | -3 Fe(OH)_3 | 1 | -1 H_2O | 3 | 3 FeI3 | 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 HI | 3 | -3 | -1/3 (Δ[HI])/(Δt) Fe(OH)_3 | 1 | -1 | -(Δ[Fe(OH)3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) FeI3 | 1 | 1 | (Δ[FeI3])/(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[HI])/(Δt) = -(Δ[Fe(OH)3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[FeI3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| hydrogen iodide | iron(III) hydroxide | water | FeI3 formula | HI | Fe(OH)_3 | H_2O | FeI3 Hill formula | HI | FeH_3O_3 | H_2O | FeI3 name | hydrogen iodide | iron(III) hydroxide | water | IUPAC name | hydrogen iodide | ferric trihydroxide | water |](../image_source/ff8217b58640e49a7ead74437e57fb27.png)
| hydrogen iodide | iron(III) hydroxide | water | FeI3 formula | HI | Fe(OH)_3 | H_2O | FeI3 Hill formula | HI | FeH_3O_3 | H_2O | FeI3 name | hydrogen iodide | iron(III) hydroxide | water | IUPAC name | hydrogen iodide | ferric trihydroxide | water |
Substance properties
![| hydrogen iodide | iron(III) hydroxide | water | FeI3 molar mass | 127.912 g/mol | 106.87 g/mol | 18.015 g/mol | 436.558 g/mol phase | gas (at STP) | | liquid (at STP) | melting point | -50.76 °C | | 0 °C | boiling point | -35.55 °C | | 99.9839 °C | density | 0.005228 g/cm^3 (at 25 °C) | | 1 g/cm^3 | solubility in water | very soluble | | | surface tension | | | 0.0728 N/m | dynamic viscosity | 0.001321 Pa s (at -39 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |](../image_source/e96f80898d87bcf96174ab519f1d7316.png)
| hydrogen iodide | iron(III) hydroxide | water | FeI3 molar mass | 127.912 g/mol | 106.87 g/mol | 18.015 g/mol | 436.558 g/mol phase | gas (at STP) | | liquid (at STP) | melting point | -50.76 °C | | 0 °C | boiling point | -35.55 °C | | 99.9839 °C | density | 0.005228 g/cm^3 (at 25 °C) | | 1 g/cm^3 | solubility in water | very soluble | | | surface tension | | | 0.0728 N/m | dynamic viscosity | 0.001321 Pa s (at -39 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |
Units