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H2O + NH3 + Fe(NO3)3 = Fe(OH)3 + NH4NO3

Input interpretation

H_2O water + NH_3 ammonia + Fe(NO_3)_3 ferric nitrate ⟶ Fe(OH)_3 iron(III) hydroxide + NH_4NO_3 ammonium nitrate
H_2O water + NH_3 ammonia + Fe(NO_3)_3 ferric nitrate ⟶ Fe(OH)_3 iron(III) hydroxide + NH_4NO_3 ammonium nitrate

Balanced equation

Balance the chemical equation algebraically: H_2O + NH_3 + Fe(NO_3)_3 ⟶ Fe(OH)_3 + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NH_3 + c_3 Fe(NO_3)_3 ⟶ c_4 Fe(OH)_3 + c_5 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and Fe: H: | 2 c_1 + 3 c_2 = 3 c_4 + 4 c_5 O: | c_1 + 9 c_3 = 3 c_4 + 3 c_5 N: | c_2 + 3 c_3 = 2 c_5 Fe: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 3 c_3 = 1 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + 3 NH_3 + Fe(NO_3)_3 ⟶ Fe(OH)_3 + 3 NH_4NO_3
Balance the chemical equation algebraically: H_2O + NH_3 + Fe(NO_3)_3 ⟶ Fe(OH)_3 + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NH_3 + c_3 Fe(NO_3)_3 ⟶ c_4 Fe(OH)_3 + c_5 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and Fe: H: | 2 c_1 + 3 c_2 = 3 c_4 + 4 c_5 O: | c_1 + 9 c_3 = 3 c_4 + 3 c_5 N: | c_2 + 3 c_3 = 2 c_5 Fe: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 3 c_3 = 1 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + 3 NH_3 + Fe(NO_3)_3 ⟶ Fe(OH)_3 + 3 NH_4NO_3

Structures

+ + ⟶ +
+ + ⟶ +

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + NH_3 + Fe(NO_3)_3 ⟶ 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: 3 H_2O + 3 NH_3 + Fe(NO_3)_3 ⟶ 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 H_2O | 3 | -3 NH_3 | 3 | -3 Fe(NO_3)_3 | 1 | -1 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 H_2O | 3 | -3 | ([H2O])^(-3) NH_3 | 3 | -3 | ([NH3])^(-3) Fe(NO_3)_3 | 1 | -1 | ([Fe(NO3)3])^(-1) 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 = ([H2O])^(-3) ([NH3])^(-3) ([Fe(NO3)3])^(-1) [Fe(OH)3] ([NH4NO3])^3 = ([Fe(OH)3] ([NH4NO3])^3)/(([H2O])^3 ([NH3])^3 [Fe(NO3)3])
Construct the equilibrium constant, K, expression for: H_2O + NH_3 + Fe(NO_3)_3 ⟶ 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: 3 H_2O + 3 NH_3 + Fe(NO_3)_3 ⟶ 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 H_2O | 3 | -3 NH_3 | 3 | -3 Fe(NO_3)_3 | 1 | -1 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 H_2O | 3 | -3 | ([H2O])^(-3) NH_3 | 3 | -3 | ([NH3])^(-3) Fe(NO_3)_3 | 1 | -1 | ([Fe(NO3)3])^(-1) 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 = ([H2O])^(-3) ([NH3])^(-3) ([Fe(NO3)3])^(-1) [Fe(OH)3] ([NH4NO3])^3 = ([Fe(OH)3] ([NH4NO3])^3)/(([H2O])^3 ([NH3])^3 [Fe(NO3)3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + NH_3 + Fe(NO_3)_3 ⟶ 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: 3 H_2O + 3 NH_3 + Fe(NO_3)_3 ⟶ 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 H_2O | 3 | -3 NH_3 | 3 | -3 Fe(NO_3)_3 | 1 | -1 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 H_2O | 3 | -3 | -1/3 (Δ[H2O])/(Δt) NH_3 | 3 | -3 | -1/3 (Δ[NH3])/(Δt) Fe(NO_3)_3 | 1 | -1 | -(Δ[Fe(NO3)3])/(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 = -1/3 (Δ[H2O])/(Δt) = -1/3 (Δ[NH3])/(Δt) = -(Δ[Fe(NO3)3])/(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: H_2O + NH_3 + Fe(NO_3)_3 ⟶ 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: 3 H_2O + 3 NH_3 + Fe(NO_3)_3 ⟶ 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 H_2O | 3 | -3 NH_3 | 3 | -3 Fe(NO_3)_3 | 1 | -1 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 H_2O | 3 | -3 | -1/3 (Δ[H2O])/(Δt) NH_3 | 3 | -3 | -1/3 (Δ[NH3])/(Δt) Fe(NO_3)_3 | 1 | -1 | -(Δ[Fe(NO3)3])/(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 = -1/3 (Δ[H2O])/(Δt) = -1/3 (Δ[NH3])/(Δt) = -(Δ[Fe(NO3)3])/(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

| water | ammonia | ferric nitrate | iron(III) hydroxide | ammonium nitrate formula | H_2O | NH_3 | Fe(NO_3)_3 | Fe(OH)_3 | NH_4NO_3 Hill formula | H_2O | H_3N | FeN_3O_9 | FeH_3O_3 | H_4N_2O_3 name | water | ammonia | ferric nitrate | iron(III) hydroxide | ammonium nitrate IUPAC name | water | ammonia | iron(+3) cation trinitrate | ferric trihydroxide |
| water | ammonia | ferric nitrate | iron(III) hydroxide | ammonium nitrate formula | H_2O | NH_3 | Fe(NO_3)_3 | Fe(OH)_3 | NH_4NO_3 Hill formula | H_2O | H_3N | FeN_3O_9 | FeH_3O_3 | H_4N_2O_3 name | water | ammonia | ferric nitrate | iron(III) hydroxide | ammonium nitrate IUPAC name | water | ammonia | iron(+3) cation trinitrate | ferric trihydroxide |

Substance properties

| water | ammonia | ferric nitrate | iron(III) hydroxide | ammonium nitrate molar mass | 18.015 g/mol | 17.031 g/mol | 241.86 g/mol | 106.87 g/mol | 80.04 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | | solid (at STP) melting point | 0 °C | -77.73 °C | 35 °C | | 169 °C boiling point | 99.9839 °C | -33.33 °C | | | 210 °C density | 1 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | 1.7 g/cm^3 | | 1.73 g/cm^3 solubility in water | | | very soluble | | surface tension | 0.0728 N/m | 0.0234 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.009×10^-5 Pa s (at 25 °C) | | | odor | odorless | | | | odorless
| water | ammonia | ferric nitrate | iron(III) hydroxide | ammonium nitrate molar mass | 18.015 g/mol | 17.031 g/mol | 241.86 g/mol | 106.87 g/mol | 80.04 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | | solid (at STP) melting point | 0 °C | -77.73 °C | 35 °C | | 169 °C boiling point | 99.9839 °C | -33.33 °C | | | 210 °C density | 1 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | 1.7 g/cm^3 | | 1.73 g/cm^3 solubility in water | | | very soluble | | surface tension | 0.0728 N/m | 0.0234 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.009×10^-5 Pa s (at 25 °C) | | | odor | odorless | | | | odorless

Units

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