Search

H2SO4 + FeSO4 + NNO3 = H2O + NO + Fe2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + FeSO_4 duretter + N_2O_3 nitrogen trioxide ⟶ H_2O water + NO nitric oxide + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate
H_2SO_4 sulfuric acid + FeSO_4 duretter + N_2O_3 nitrogen trioxide ⟶ H_2O water + NO nitric oxide + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + FeSO_4 + N_2O_3 ⟶ H_2O + NO + 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 N_2O_3 ⟶ c_4 H_2O + c_5 NO + c_6 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 and N: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 4 c_2 + 3 c_3 = c_4 + c_5 + 12 c_6 S: | c_1 + c_2 = 3 c_6 Fe: | c_2 = 2 c_6 N: | 2 c_3 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 FeSO_4 + N_2O_3 ⟶ H_2O + 2 NO + Fe_2(SO_4)_3·xH_2O
Balance the chemical equation algebraically: H_2SO_4 + FeSO_4 + N_2O_3 ⟶ H_2O + NO + 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 N_2O_3 ⟶ c_4 H_2O + c_5 NO + c_6 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 and N: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 4 c_2 + 3 c_3 = c_4 + c_5 + 12 c_6 S: | c_1 + c_2 = 3 c_6 Fe: | c_2 = 2 c_6 N: | 2 c_3 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 FeSO_4 + N_2O_3 ⟶ H_2O + 2 NO + Fe_2(SO_4)_3·xH_2O

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

sulfuric acid + duretter + nitrogen trioxide ⟶ water + nitric oxide + iron(III) sulfate hydrate
sulfuric acid + duretter + nitrogen trioxide ⟶ water + nitric oxide + iron(III) sulfate hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + FeSO_4 + N_2O_3 ⟶ H_2O + NO + 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: H_2SO_4 + 2 FeSO_4 + N_2O_3 ⟶ H_2O + 2 NO + 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 | 1 | -1 FeSO_4 | 2 | -2 N_2O_3 | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 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 | 1 | -1 | ([H2SO4])^(-1) FeSO_4 | 2 | -2 | ([FeSO4])^(-2) N_2O_3 | 1 | -1 | ([N2O3])^(-1) H_2O | 1 | 1 | [H2O] NO | 2 | 2 | ([NO])^2 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])^(-1) ([FeSO4])^(-2) ([N2O3])^(-1) [H2O] ([NO])^2 [Fe2(SO4)3·xH2O] = ([H2O] ([NO])^2 [Fe2(SO4)3·xH2O])/([H2SO4] ([FeSO4])^2 [N2O3])
Construct the equilibrium constant, K, expression for: H_2SO_4 + FeSO_4 + N_2O_3 ⟶ H_2O + NO + 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: H_2SO_4 + 2 FeSO_4 + N_2O_3 ⟶ H_2O + 2 NO + 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 | 1 | -1 FeSO_4 | 2 | -2 N_2O_3 | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 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 | 1 | -1 | ([H2SO4])^(-1) FeSO_4 | 2 | -2 | ([FeSO4])^(-2) N_2O_3 | 1 | -1 | ([N2O3])^(-1) H_2O | 1 | 1 | [H2O] NO | 2 | 2 | ([NO])^2 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])^(-1) ([FeSO4])^(-2) ([N2O3])^(-1) [H2O] ([NO])^2 [Fe2(SO4)3·xH2O] = ([H2O] ([NO])^2 [Fe2(SO4)3·xH2O])/([H2SO4] ([FeSO4])^2 [N2O3])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + FeSO_4 + N_2O_3 ⟶ H_2O + NO + 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: H_2SO_4 + 2 FeSO_4 + N_2O_3 ⟶ H_2O + 2 NO + 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 | 1 | -1 FeSO_4 | 2 | -2 N_2O_3 | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) N_2O_3 | 1 | -1 | -(Δ[N2O3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(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 = -(Δ[H2SO4])/(Δt) = -1/2 (Δ[FeSO4])/(Δt) = -(Δ[N2O3])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(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 + N_2O_3 ⟶ H_2O + NO + 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: H_2SO_4 + 2 FeSO_4 + N_2O_3 ⟶ H_2O + 2 NO + 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 | 1 | -1 FeSO_4 | 2 | -2 N_2O_3 | 1 | -1 H_2O | 1 | 1 NO | 2 | 2 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) N_2O_3 | 1 | -1 | -(Δ[N2O3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(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 = -(Δ[H2SO4])/(Δt) = -1/2 (Δ[FeSO4])/(Δt) = -(Δ[N2O3])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(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 | nitrogen trioxide | water | nitric oxide | iron(III) sulfate hydrate formula | H_2SO_4 | FeSO_4 | N_2O_3 | H_2O | NO | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | FeO_4S | N_2O_3 | H_2O | NO | Fe_2O_12S_3 name | sulfuric acid | duretter | nitrogen trioxide | water | nitric oxide | iron(III) sulfate hydrate IUPAC name | sulfuric acid | iron(+2) cation sulfate | nitramide | water | nitric oxide | diferric trisulfate
| sulfuric acid | duretter | nitrogen trioxide | water | nitric oxide | iron(III) sulfate hydrate formula | H_2SO_4 | FeSO_4 | N_2O_3 | H_2O | NO | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | FeO_4S | N_2O_3 | H_2O | NO | Fe_2O_12S_3 name | sulfuric acid | duretter | nitrogen trioxide | water | nitric oxide | iron(III) sulfate hydrate IUPAC name | sulfuric acid | iron(+2) cation sulfate | nitramide | water | nitric oxide | diferric trisulfate

Random Queries

names of columbite group
first ionization energies of alkali metals
formula of hexaiodostannate(IV) anion vs fluoride anion
ion class of ferrate anion vs sulfite anion
freezing point of lime vs gadolinium(III) bromide hydrate
add tritanopia color blindness filter to a picture of an awaruite
CuSO4 + Ba(OH)2 = Cu(OH)2 + BaSO4
O2 + FeS = Fe2O3 + SO3
ion class of hydrogen cation vs palladium(II) cation
colorize components image chromdravite