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Fe(NO3)3 + NH4OH = Fe(OH)3 + NH4NO3

Input interpretation

Fe(NO_3)_3 ferric nitrate + NH_4OH ammonium hydroxide ⟶ Fe(OH)_3 iron(III) hydroxide + NH_4NO_3 ammonium nitrate
Fe(NO_3)_3 ferric nitrate + NH_4OH ammonium hydroxide ⟶ Fe(OH)_3 iron(III) hydroxide + NH_4NO_3 ammonium nitrate

Balanced equation

Balance the chemical equation algebraically: Fe(NO_3)_3 + NH_4OH ⟶ Fe(OH)_3 + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe(NO_3)_3 + c_2 NH_4OH ⟶ c_3 Fe(OH)_3 + c_4 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, N, O and H: Fe: | c_1 = c_3 N: | 3 c_1 + c_2 = 2 c_4 O: | 9 c_1 + c_2 = 3 c_3 + 3 c_4 H: | 5 c_2 = 3 c_3 + 4 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 = 3 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe(NO_3)_3 + 3 NH_4OH ⟶ Fe(OH)_3 + 3 NH_4NO_3
Balance the chemical equation algebraically: Fe(NO_3)_3 + NH_4OH ⟶ Fe(OH)_3 + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe(NO_3)_3 + c_2 NH_4OH ⟶ c_3 Fe(OH)_3 + c_4 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, N, O and H: Fe: | c_1 = c_3 N: | 3 c_1 + c_2 = 2 c_4 O: | 9 c_1 + c_2 = 3 c_3 + 3 c_4 H: | 5 c_2 = 3 c_3 + 4 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 = 3 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe(NO_3)_3 + 3 NH_4OH ⟶ Fe(OH)_3 + 3 NH_4NO_3

Structures

+ ⟶ +
+ ⟶ +

Names

ferric nitrate + ammonium hydroxide ⟶ iron(III) hydroxide + ammonium nitrate
ferric nitrate + ammonium hydroxide ⟶ iron(III) hydroxide + ammonium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Fe(NO_3)_3 + NH_4OH ⟶ Fe(OH)_3 + NH_4NO_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: Fe(NO_3)_3 + 3 NH_4OH ⟶ Fe(OH)_3 + 3 NH_4NO_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 Fe(NO_3)_3 | 1 | -1 NH_4OH | 3 | -3 Fe(OH)_3 | 1 | 1 NH_4NO_3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe(NO_3)_3 | 1 | -1 | ([Fe(NO3)3])^(-1) NH_4OH | 3 | -3 | ([NH4OH])^(-3) Fe(OH)_3 | 1 | 1 | [Fe(OH)3] NH_4NO_3 | 3 | 3 | ([NH4NO3])^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 = ([Fe(NO3)3])^(-1) ([NH4OH])^(-3) [Fe(OH)3] ([NH4NO3])^3 = ([Fe(OH)3] ([NH4NO3])^3)/([Fe(NO3)3] ([NH4OH])^3)
Construct the equilibrium constant, K, expression for: Fe(NO_3)_3 + NH_4OH ⟶ Fe(OH)_3 + NH_4NO_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: Fe(NO_3)_3 + 3 NH_4OH ⟶ Fe(OH)_3 + 3 NH_4NO_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 Fe(NO_3)_3 | 1 | -1 NH_4OH | 3 | -3 Fe(OH)_3 | 1 | 1 NH_4NO_3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe(NO_3)_3 | 1 | -1 | ([Fe(NO3)3])^(-1) NH_4OH | 3 | -3 | ([NH4OH])^(-3) Fe(OH)_3 | 1 | 1 | [Fe(OH)3] NH_4NO_3 | 3 | 3 | ([NH4NO3])^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 = ([Fe(NO3)3])^(-1) ([NH4OH])^(-3) [Fe(OH)3] ([NH4NO3])^3 = ([Fe(OH)3] ([NH4NO3])^3)/([Fe(NO3)3] ([NH4OH])^3)

Rate of reaction

Construct the rate of reaction expression for: Fe(NO_3)_3 + NH_4OH ⟶ Fe(OH)_3 + NH_4NO_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: Fe(NO_3)_3 + 3 NH_4OH ⟶ Fe(OH)_3 + 3 NH_4NO_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 Fe(NO_3)_3 | 1 | -1 NH_4OH | 3 | -3 Fe(OH)_3 | 1 | 1 NH_4NO_3 | 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 Fe(NO_3)_3 | 1 | -1 | -(Δ[Fe(NO3)3])/(Δt) NH_4OH | 3 | -3 | -1/3 (Δ[NH4OH])/(Δt) Fe(OH)_3 | 1 | 1 | (Δ[Fe(OH)3])/(Δt) NH_4NO_3 | 3 | 3 | 1/3 (Δ[NH4NO3])/(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[Fe(NO3)3])/(Δt) = -1/3 (Δ[NH4OH])/(Δt) = (Δ[Fe(OH)3])/(Δt) = 1/3 (Δ[NH4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Fe(NO_3)_3 + NH_4OH ⟶ Fe(OH)_3 + NH_4NO_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: Fe(NO_3)_3 + 3 NH_4OH ⟶ Fe(OH)_3 + 3 NH_4NO_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 Fe(NO_3)_3 | 1 | -1 NH_4OH | 3 | -3 Fe(OH)_3 | 1 | 1 NH_4NO_3 | 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 Fe(NO_3)_3 | 1 | -1 | -(Δ[Fe(NO3)3])/(Δt) NH_4OH | 3 | -3 | -1/3 (Δ[NH4OH])/(Δt) Fe(OH)_3 | 1 | 1 | (Δ[Fe(OH)3])/(Δt) NH_4NO_3 | 3 | 3 | 1/3 (Δ[NH4NO3])/(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[Fe(NO3)3])/(Δt) = -1/3 (Δ[NH4OH])/(Δt) = (Δ[Fe(OH)3])/(Δt) = 1/3 (Δ[NH4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| ferric nitrate | ammonium hydroxide | iron(III) hydroxide | ammonium nitrate formula | Fe(NO_3)_3 | NH_4OH | Fe(OH)_3 | NH_4NO_3 Hill formula | FeN_3O_9 | H_5NO | FeH_3O_3 | H_4N_2O_3 name | ferric nitrate | ammonium hydroxide | iron(III) hydroxide | ammonium nitrate IUPAC name | iron(+3) cation trinitrate | ammonium hydroxide | ferric trihydroxide |
| ferric nitrate | ammonium hydroxide | iron(III) hydroxide | ammonium nitrate formula | Fe(NO_3)_3 | NH_4OH | Fe(OH)_3 | NH_4NO_3 Hill formula | FeN_3O_9 | H_5NO | FeH_3O_3 | H_4N_2O_3 name | ferric nitrate | ammonium hydroxide | iron(III) hydroxide | ammonium nitrate IUPAC name | iron(+3) cation trinitrate | ammonium hydroxide | ferric trihydroxide |

Substance properties

| ferric nitrate | ammonium hydroxide | iron(III) hydroxide | ammonium nitrate molar mass | 241.86 g/mol | 35.046 g/mol | 106.87 g/mol | 80.04 g/mol phase | solid (at STP) | aqueous (at STP) | | solid (at STP) melting point | 35 °C | -57.5 °C | | 169 °C boiling point | | 36 °C | | 210 °C density | 1.7 g/cm^3 | 0.9 g/cm^3 | | 1.73 g/cm^3 solubility in water | very soluble | very soluble | | odor | | | | odorless
| ferric nitrate | ammonium hydroxide | iron(III) hydroxide | ammonium nitrate molar mass | 241.86 g/mol | 35.046 g/mol | 106.87 g/mol | 80.04 g/mol phase | solid (at STP) | aqueous (at STP) | | solid (at STP) melting point | 35 °C | -57.5 °C | | 169 °C boiling point | | 36 °C | | 210 °C density | 1.7 g/cm^3 | 0.9 g/cm^3 | | 1.73 g/cm^3 solubility in water | very soluble | very soluble | | odor | | | | odorless

Units

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