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Fe2(SO4)3 + NH2OH = H2O + H2SO4 + FeSO4 + N2O

Input interpretation

Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + NH_2OH hydroxylamine ⟶ H_2O water + H_2SO_4 sulfuric acid + FeSO_4 duretter + N_2O nitrous oxide
Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + NH_2OH hydroxylamine ⟶ H_2O water + H_2SO_4 sulfuric acid + FeSO_4 duretter + N_2O nitrous oxide

Balanced equation

Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + NH_2OH ⟶ H_2O + H_2SO_4 + FeSO_4 + N_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 NH_2OH ⟶ c_3 H_2O + c_4 H_2SO_4 + c_5 FeSO_4 + c_6 N_2O Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, H and N: Fe: | 2 c_1 = c_5 O: | 12 c_1 + c_2 = c_3 + 4 c_4 + 4 c_5 + c_6 S: | 3 c_1 = c_4 + c_5 H: | 3 c_2 = 2 c_3 + 2 c_4 N: | c_2 = 2 c_6 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 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 4 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Fe_2(SO_4)_3·xH_2O + 2 NH_2OH ⟶ H_2O + 2 H_2SO_4 + 4 FeSO_4 + N_2O
Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + NH_2OH ⟶ H_2O + H_2SO_4 + FeSO_4 + N_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 NH_2OH ⟶ c_3 H_2O + c_4 H_2SO_4 + c_5 FeSO_4 + c_6 N_2O Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, H and N: Fe: | 2 c_1 = c_5 O: | 12 c_1 + c_2 = c_3 + 4 c_4 + 4 c_5 + c_6 S: | 3 c_1 = c_4 + c_5 H: | 3 c_2 = 2 c_3 + 2 c_4 N: | c_2 = 2 c_6 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 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 4 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Fe_2(SO_4)_3·xH_2O + 2 NH_2OH ⟶ H_2O + 2 H_2SO_4 + 4 FeSO_4 + N_2O

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

iron(III) sulfate hydrate + hydroxylamine ⟶ water + sulfuric acid + duretter + nitrous oxide
iron(III) sulfate hydrate + hydroxylamine ⟶ water + sulfuric acid + duretter + nitrous oxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + NH_2OH ⟶ H_2O + H_2SO_4 + FeSO_4 + N_2O 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: 2 Fe_2(SO_4)_3·xH_2O + 2 NH_2OH ⟶ H_2O + 2 H_2SO_4 + 4 FeSO_4 + N_2O 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_2(SO_4)_3·xH_2O | 2 | -2 NH_2OH | 2 | -2 H_2O | 1 | 1 H_2SO_4 | 2 | 2 FeSO_4 | 4 | 4 N_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe_2(SO_4)_3·xH_2O | 2 | -2 | ([Fe2(SO4)3·xH2O])^(-2) NH_2OH | 2 | -2 | ([NH2OH])^(-2) H_2O | 1 | 1 | [H2O] H_2SO_4 | 2 | 2 | ([H2SO4])^2 FeSO_4 | 4 | 4 | ([FeSO4])^4 N_2O | 1 | 1 | [N2O] 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 = ([Fe2(SO4)3·xH2O])^(-2) ([NH2OH])^(-2) [H2O] ([H2SO4])^2 ([FeSO4])^4 [N2O] = ([H2O] ([H2SO4])^2 ([FeSO4])^4 [N2O])/(([Fe2(SO4)3·xH2O])^2 ([NH2OH])^2)
Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + NH_2OH ⟶ H_2O + H_2SO_4 + FeSO_4 + N_2O 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: 2 Fe_2(SO_4)_3·xH_2O + 2 NH_2OH ⟶ H_2O + 2 H_2SO_4 + 4 FeSO_4 + N_2O 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_2(SO_4)_3·xH_2O | 2 | -2 NH_2OH | 2 | -2 H_2O | 1 | 1 H_2SO_4 | 2 | 2 FeSO_4 | 4 | 4 N_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe_2(SO_4)_3·xH_2O | 2 | -2 | ([Fe2(SO4)3·xH2O])^(-2) NH_2OH | 2 | -2 | ([NH2OH])^(-2) H_2O | 1 | 1 | [H2O] H_2SO_4 | 2 | 2 | ([H2SO4])^2 FeSO_4 | 4 | 4 | ([FeSO4])^4 N_2O | 1 | 1 | [N2O] 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 = ([Fe2(SO4)3·xH2O])^(-2) ([NH2OH])^(-2) [H2O] ([H2SO4])^2 ([FeSO4])^4 [N2O] = ([H2O] ([H2SO4])^2 ([FeSO4])^4 [N2O])/(([Fe2(SO4)3·xH2O])^2 ([NH2OH])^2)

Rate of reaction

Construct the rate of reaction expression for: Fe_2(SO_4)_3·xH_2O + NH_2OH ⟶ H_2O + H_2SO_4 + FeSO_4 + N_2O 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: 2 Fe_2(SO_4)_3·xH_2O + 2 NH_2OH ⟶ H_2O + 2 H_2SO_4 + 4 FeSO_4 + N_2O 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_2(SO_4)_3·xH_2O | 2 | -2 NH_2OH | 2 | -2 H_2O | 1 | 1 H_2SO_4 | 2 | 2 FeSO_4 | 4 | 4 N_2O | 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 Fe_2(SO_4)_3·xH_2O | 2 | -2 | -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) NH_2OH | 2 | -2 | -1/2 (Δ[NH2OH])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) FeSO_4 | 4 | 4 | 1/4 (Δ[FeSO4])/(Δt) N_2O | 1 | 1 | (Δ[N2O])/(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 = -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) = -1/2 (Δ[NH2OH])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = 1/4 (Δ[FeSO4])/(Δt) = (Δ[N2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Fe_2(SO_4)_3·xH_2O + NH_2OH ⟶ H_2O + H_2SO_4 + FeSO_4 + N_2O 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: 2 Fe_2(SO_4)_3·xH_2O + 2 NH_2OH ⟶ H_2O + 2 H_2SO_4 + 4 FeSO_4 + N_2O 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_2(SO_4)_3·xH_2O | 2 | -2 NH_2OH | 2 | -2 H_2O | 1 | 1 H_2SO_4 | 2 | 2 FeSO_4 | 4 | 4 N_2O | 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 Fe_2(SO_4)_3·xH_2O | 2 | -2 | -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) NH_2OH | 2 | -2 | -1/2 (Δ[NH2OH])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) FeSO_4 | 4 | 4 | 1/4 (Δ[FeSO4])/(Δt) N_2O | 1 | 1 | (Δ[N2O])/(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 = -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) = -1/2 (Δ[NH2OH])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = 1/4 (Δ[FeSO4])/(Δt) = (Δ[N2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iron(III) sulfate hydrate | hydroxylamine | water | sulfuric acid | duretter | nitrous oxide formula | Fe_2(SO_4)_3·xH_2O | NH_2OH | H_2O | H_2SO_4 | FeSO_4 | N_2O Hill formula | Fe_2O_12S_3 | H_3NO | H_2O | H_2O_4S | FeO_4S | N_2O name | iron(III) sulfate hydrate | hydroxylamine | water | sulfuric acid | duretter | nitrous oxide IUPAC name | diferric trisulfate | hydroxylamine | water | sulfuric acid | iron(+2) cation sulfate | nitrous oxide
| iron(III) sulfate hydrate | hydroxylamine | water | sulfuric acid | duretter | nitrous oxide formula | Fe_2(SO_4)_3·xH_2O | NH_2OH | H_2O | H_2SO_4 | FeSO_4 | N_2O Hill formula | Fe_2O_12S_3 | H_3NO | H_2O | H_2O_4S | FeO_4S | N_2O name | iron(III) sulfate hydrate | hydroxylamine | water | sulfuric acid | duretter | nitrous oxide IUPAC name | diferric trisulfate | hydroxylamine | water | sulfuric acid | iron(+2) cation sulfate | nitrous oxide

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