Search

HNO3 + Fe3O4 = H2O + NO2 + Fe(NO3)3

Input interpretation

HNO_3 nitric acid + FeO·Fe_2O_3 iron(II, III) oxide ⟶ H_2O water + NO_2 nitrogen dioxide + Fe(NO_3)_3 ferric nitrate
HNO_3 nitric acid + FeO·Fe_2O_3 iron(II, III) oxide ⟶ H_2O water + NO_2 nitrogen dioxide + Fe(NO_3)_3 ferric nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_3 + FeO·Fe_2O_3 ⟶ H_2O + NO_2 + Fe(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 FeO·Fe_2O_3 ⟶ c_3 H_2O + c_4 NO_2 + c_5 Fe(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Fe: H: | c_1 = 2 c_3 N: | c_1 = c_4 + 3 c_5 O: | 3 c_1 + 4 c_2 = c_3 + 2 c_4 + 9 c_5 Fe: | 3 c_2 = c_5 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 = 10 c_2 = 1 c_3 = 5 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HNO_3 + FeO·Fe_2O_3 ⟶ 5 H_2O + NO_2 + 3 Fe(NO_3)_3
Balance the chemical equation algebraically: HNO_3 + FeO·Fe_2O_3 ⟶ H_2O + NO_2 + Fe(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 FeO·Fe_2O_3 ⟶ c_3 H_2O + c_4 NO_2 + c_5 Fe(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Fe: H: | c_1 = 2 c_3 N: | c_1 = c_4 + 3 c_5 O: | 3 c_1 + 4 c_2 = c_3 + 2 c_4 + 9 c_5 Fe: | 3 c_2 = c_5 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 = 10 c_2 = 1 c_3 = 5 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HNO_3 + FeO·Fe_2O_3 ⟶ 5 H_2O + NO_2 + 3 Fe(NO_3)_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

nitric acid + iron(II, III) oxide ⟶ water + nitrogen dioxide + ferric nitrate
nitric acid + iron(II, III) oxide ⟶ water + nitrogen dioxide + ferric nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + FeO·Fe_2O_3 ⟶ H_2O + NO_2 + Fe(NO_3)_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: 10 HNO_3 + FeO·Fe_2O_3 ⟶ 5 H_2O + NO_2 + 3 Fe(NO_3)_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 HNO_3 | 10 | -10 FeO·Fe_2O_3 | 1 | -1 H_2O | 5 | 5 NO_2 | 1 | 1 Fe(NO_3)_3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 10 | -10 | ([HNO3])^(-10) FeO·Fe_2O_3 | 1 | -1 | ([FeO·Fe2O3])^(-1) H_2O | 5 | 5 | ([H2O])^5 NO_2 | 1 | 1 | [NO2] Fe(NO_3)_3 | 3 | 3 | ([Fe(NO3)3])^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 = ([HNO3])^(-10) ([FeO·Fe2O3])^(-1) ([H2O])^5 [NO2] ([Fe(NO3)3])^3 = (([H2O])^5 [NO2] ([Fe(NO3)3])^3)/(([HNO3])^10 [FeO·Fe2O3])
Construct the equilibrium constant, K, expression for: HNO_3 + FeO·Fe_2O_3 ⟶ H_2O + NO_2 + Fe(NO_3)_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: 10 HNO_3 + FeO·Fe_2O_3 ⟶ 5 H_2O + NO_2 + 3 Fe(NO_3)_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 HNO_3 | 10 | -10 FeO·Fe_2O_3 | 1 | -1 H_2O | 5 | 5 NO_2 | 1 | 1 Fe(NO_3)_3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 10 | -10 | ([HNO3])^(-10) FeO·Fe_2O_3 | 1 | -1 | ([FeO·Fe2O3])^(-1) H_2O | 5 | 5 | ([H2O])^5 NO_2 | 1 | 1 | [NO2] Fe(NO_3)_3 | 3 | 3 | ([Fe(NO3)3])^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 = ([HNO3])^(-10) ([FeO·Fe2O3])^(-1) ([H2O])^5 [NO2] ([Fe(NO3)3])^3 = (([H2O])^5 [NO2] ([Fe(NO3)3])^3)/(([HNO3])^10 [FeO·Fe2O3])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + FeO·Fe_2O_3 ⟶ H_2O + NO_2 + Fe(NO_3)_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: 10 HNO_3 + FeO·Fe_2O_3 ⟶ 5 H_2O + NO_2 + 3 Fe(NO_3)_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 HNO_3 | 10 | -10 FeO·Fe_2O_3 | 1 | -1 H_2O | 5 | 5 NO_2 | 1 | 1 Fe(NO_3)_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 HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) FeO·Fe_2O_3 | 1 | -1 | -(Δ[FeO·Fe2O3])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) NO_2 | 1 | 1 | (Δ[NO2])/(Δt) Fe(NO_3)_3 | 3 | 3 | 1/3 (Δ[Fe(NO3)3])/(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 = -1/10 (Δ[HNO3])/(Δt) = -(Δ[FeO·Fe2O3])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[NO2])/(Δt) = 1/3 (Δ[Fe(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + FeO·Fe_2O_3 ⟶ H_2O + NO_2 + Fe(NO_3)_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: 10 HNO_3 + FeO·Fe_2O_3 ⟶ 5 H_2O + NO_2 + 3 Fe(NO_3)_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 HNO_3 | 10 | -10 FeO·Fe_2O_3 | 1 | -1 H_2O | 5 | 5 NO_2 | 1 | 1 Fe(NO_3)_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 HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) FeO·Fe_2O_3 | 1 | -1 | -(Δ[FeO·Fe2O3])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) NO_2 | 1 | 1 | (Δ[NO2])/(Δt) Fe(NO_3)_3 | 3 | 3 | 1/3 (Δ[Fe(NO3)3])/(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 = -1/10 (Δ[HNO3])/(Δt) = -(Δ[FeO·Fe2O3])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[NO2])/(Δt) = 1/3 (Δ[Fe(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | iron(II, III) oxide | water | nitrogen dioxide | ferric nitrate formula | HNO_3 | FeO·Fe_2O_3 | H_2O | NO_2 | Fe(NO_3)_3 Hill formula | HNO_3 | Fe_3O_4 | H_2O | NO_2 | FeN_3O_9 name | nitric acid | iron(II, III) oxide | water | nitrogen dioxide | ferric nitrate IUPAC name | nitric acid | | water | Nitrogen dioxide | iron(+3) cation trinitrate
| nitric acid | iron(II, III) oxide | water | nitrogen dioxide | ferric nitrate formula | HNO_3 | FeO·Fe_2O_3 | H_2O | NO_2 | Fe(NO_3)_3 Hill formula | HNO_3 | Fe_3O_4 | H_2O | NO_2 | FeN_3O_9 name | nitric acid | iron(II, III) oxide | water | nitrogen dioxide | ferric nitrate IUPAC name | nitric acid | | water | Nitrogen dioxide | iron(+3) cation trinitrate

Random Queries

alternate names of osmium(VI) cation vs mercury(II) cation
KClO3 + KNO2 = KCl + KNO3
CAS number of sodium bromide vs potassium chloride
CAS number of strontium oxide vs ironate
formula of perchloric acid
formula of sodium persulfate
molar mass of zinc formate dihydrate vs hexaamminecobalt(III) nitrate
melting point of octane vs hexacosane
HNO3 + Fe = H2O + NO2 + Fe2O3
scandium vs titanium vs manganese vs vanadium