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H2SO4 + FeSO4 + NaNO2 = H2O + NO + Na2SO4 + Fe2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + FeSO_4 duretter + NaNO_2 sodium nitrite ⟶ H_2O water + NO nitric oxide + Na_2SO_4 sodium sulfate + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate
H_2SO_4 sulfuric acid + FeSO_4 duretter + NaNO_2 sodium nitrite ⟶ H_2O water + NO nitric oxide + Na_2SO_4 sodium sulfate + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + FeSO_4 + NaNO_2 ⟶ H_2O + NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeSO_4 + c_3 NaNO_2 ⟶ c_4 H_2O + c_5 NO + c_6 Na_2SO_4 + c_7 Fe_2(SO_4)_3·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Fe, N and Na: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 4 c_2 + 2 c_3 = c_4 + c_5 + 4 c_6 + 12 c_7 S: | c_1 + c_2 = c_6 + 3 c_7 Fe: | c_2 = 2 c_7 N: | c_3 = c_5 Na: | c_3 = 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 FeSO_4 + 2 NaNO_2 ⟶ 2 H_2O + 2 NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_2O
Balance the chemical equation algebraically: H_2SO_4 + FeSO_4 + NaNO_2 ⟶ H_2O + NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeSO_4 + c_3 NaNO_2 ⟶ c_4 H_2O + c_5 NO + c_6 Na_2SO_4 + c_7 Fe_2(SO_4)_3·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Fe, N and Na: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 4 c_2 + 2 c_3 = c_4 + c_5 + 4 c_6 + 12 c_7 S: | c_1 + c_2 = c_6 + 3 c_7 Fe: | c_2 = 2 c_7 N: | c_3 = c_5 Na: | c_3 = 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 FeSO_4 + 2 NaNO_2 ⟶ 2 H_2O + 2 NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_2O

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + duretter + sodium nitrite ⟶ water + nitric oxide + sodium sulfate + iron(III) sulfate hydrate
sulfuric acid + duretter + sodium nitrite ⟶ water + nitric oxide + sodium sulfate + iron(III) sulfate hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + FeSO_4 + NaNO_2 ⟶ H_2O + NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 + 2 FeSO_4 + 2 NaNO_2 ⟶ 2 H_2O + 2 NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 | 2 | -2 FeSO_4 | 2 | -2 NaNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 Na_2SO_4 | 1 | 1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) FeSO_4 | 2 | -2 | ([FeSO4])^(-2) NaNO_2 | 2 | -2 | ([NaNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO | 2 | 2 | ([NO])^2 Na_2SO_4 | 1 | 1 | [Na2SO4] Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] 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 = ([H2SO4])^(-2) ([FeSO4])^(-2) ([NaNO2])^(-2) ([H2O])^2 ([NO])^2 [Na2SO4] [Fe2(SO4)3·xH2O] = (([H2O])^2 ([NO])^2 [Na2SO4] [Fe2(SO4)3·xH2O])/(([H2SO4])^2 ([FeSO4])^2 ([NaNO2])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + FeSO_4 + NaNO_2 ⟶ H_2O + NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 + 2 FeSO_4 + 2 NaNO_2 ⟶ 2 H_2O + 2 NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 | 2 | -2 FeSO_4 | 2 | -2 NaNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 Na_2SO_4 | 1 | 1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) FeSO_4 | 2 | -2 | ([FeSO4])^(-2) NaNO_2 | 2 | -2 | ([NaNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO | 2 | 2 | ([NO])^2 Na_2SO_4 | 1 | 1 | [Na2SO4] Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] 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 = ([H2SO4])^(-2) ([FeSO4])^(-2) ([NaNO2])^(-2) ([H2O])^2 ([NO])^2 [Na2SO4] [Fe2(SO4)3·xH2O] = (([H2O])^2 ([NO])^2 [Na2SO4] [Fe2(SO4)3·xH2O])/(([H2SO4])^2 ([FeSO4])^2 ([NaNO2])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + FeSO_4 + NaNO_2 ⟶ H_2O + NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 + 2 FeSO_4 + 2 NaNO_2 ⟶ 2 H_2O + 2 NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 | 2 | -2 FeSO_4 | 2 | -2 NaNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 Na_2SO_4 | 1 | 1 Fe_2(SO_4)_3·xH_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 H_2SO_4 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) NaNO_2 | 2 | -2 | -1/2 (Δ[NaNO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (Δ[Fe2(SO4)3·xH2O])/(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[H2SO4])/(Δt) = -1/2 (Δ[FeSO4])/(Δt) = -1/2 (Δ[NaNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[Na2SO4])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + FeSO_4 + NaNO_2 ⟶ H_2O + NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 + 2 FeSO_4 + 2 NaNO_2 ⟶ 2 H_2O + 2 NO + Na_2SO_4 + Fe_2(SO_4)_3·xH_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 H_2SO_4 | 2 | -2 FeSO_4 | 2 | -2 NaNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 Na_2SO_4 | 1 | 1 Fe_2(SO_4)_3·xH_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 H_2SO_4 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) NaNO_2 | 2 | -2 | -1/2 (Δ[NaNO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (Δ[Fe2(SO4)3·xH2O])/(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[H2SO4])/(Δt) = -1/2 (Δ[FeSO4])/(Δt) = -1/2 (Δ[NaNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[Na2SO4])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | duretter | sodium nitrite | water | nitric oxide | sodium sulfate | iron(III) sulfate hydrate formula | H_2SO_4 | FeSO_4 | NaNO_2 | H_2O | NO | Na_2SO_4 | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | FeO_4S | NNaO_2 | H_2O | NO | Na_2O_4S | Fe_2O_12S_3 name | sulfuric acid | duretter | sodium nitrite | water | nitric oxide | sodium sulfate | iron(III) sulfate hydrate IUPAC name | sulfuric acid | iron(+2) cation sulfate | sodium nitrite | water | nitric oxide | disodium sulfate | diferric trisulfate
| sulfuric acid | duretter | sodium nitrite | water | nitric oxide | sodium sulfate | iron(III) sulfate hydrate formula | H_2SO_4 | FeSO_4 | NaNO_2 | H_2O | NO | Na_2SO_4 | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | FeO_4S | NNaO_2 | H_2O | NO | Na_2O_4S | Fe_2O_12S_3 name | sulfuric acid | duretter | sodium nitrite | water | nitric oxide | sodium sulfate | iron(III) sulfate hydrate IUPAC name | sulfuric acid | iron(+2) cation sulfate | sodium nitrite | water | nitric oxide | disodium sulfate | diferric trisulfate

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