Search

H2O + HNO3 + As2S3 = H2SO4 + NO + H3AsO3

Input interpretation

H_2O water + HNO_3 nitric acid + As_2S_3 arsenic(III) sulfide ⟶ H_2SO_4 sulfuric acid + NO nitric oxide + As(OH)_3 arsenious acid
H_2O water + HNO_3 nitric acid + As_2S_3 arsenic(III) sulfide ⟶ H_2SO_4 sulfuric acid + NO nitric oxide + As(OH)_3 arsenious acid

Balanced equation

Balance the chemical equation algebraically: H_2O + HNO_3 + As_2S_3 ⟶ H_2SO_4 + NO + As(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 As_2S_3 ⟶ c_4 H_2SO_4 + c_5 NO + c_6 As(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N, As and S: H: | 2 c_1 + c_2 = 2 c_4 + 3 c_6 O: | c_1 + 3 c_2 = 4 c_4 + c_5 + 3 c_6 N: | c_2 = c_5 As: | 2 c_3 = c_6 S: | 3 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 = 2 c_2 = 8 c_3 = 1 c_4 = 3 c_5 = 8 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 8 HNO_3 + As_2S_3 ⟶ 3 H_2SO_4 + 8 NO + 2 As(OH)_3
Balance the chemical equation algebraically: H_2O + HNO_3 + As_2S_3 ⟶ H_2SO_4 + NO + As(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 As_2S_3 ⟶ c_4 H_2SO_4 + c_5 NO + c_6 As(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N, As and S: H: | 2 c_1 + c_2 = 2 c_4 + 3 c_6 O: | c_1 + 3 c_2 = 4 c_4 + c_5 + 3 c_6 N: | c_2 = c_5 As: | 2 c_3 = c_6 S: | 3 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 = 2 c_2 = 8 c_3 = 1 c_4 = 3 c_5 = 8 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 8 HNO_3 + As_2S_3 ⟶ 3 H_2SO_4 + 8 NO + 2 As(OH)_3

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + nitric acid + arsenic(III) sulfide ⟶ sulfuric acid + nitric oxide + arsenious acid
water + nitric acid + arsenic(III) sulfide ⟶ sulfuric acid + nitric oxide + arsenious acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + As_2S_3 ⟶ H_2SO_4 + NO + As(OH)_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: 2 H_2O + 8 HNO_3 + As_2S_3 ⟶ 3 H_2SO_4 + 8 NO + 2 As(OH)_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 | 2 | -2 HNO_3 | 8 | -8 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 NO | 8 | 8 As(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) HNO_3 | 8 | -8 | ([HNO3])^(-8) As_2S_3 | 1 | -1 | ([As2S3])^(-1) H_2SO_4 | 3 | 3 | ([H2SO4])^3 NO | 8 | 8 | ([NO])^8 As(OH)_3 | 2 | 2 | ([As(OH)3])^2 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])^(-2) ([HNO3])^(-8) ([As2S3])^(-1) ([H2SO4])^3 ([NO])^8 ([As(OH)3])^2 = (([H2SO4])^3 ([NO])^8 ([As(OH)3])^2)/(([H2O])^2 ([HNO3])^8 [As2S3])
Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + As_2S_3 ⟶ H_2SO_4 + NO + As(OH)_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: 2 H_2O + 8 HNO_3 + As_2S_3 ⟶ 3 H_2SO_4 + 8 NO + 2 As(OH)_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 | 2 | -2 HNO_3 | 8 | -8 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 NO | 8 | 8 As(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) HNO_3 | 8 | -8 | ([HNO3])^(-8) As_2S_3 | 1 | -1 | ([As2S3])^(-1) H_2SO_4 | 3 | 3 | ([H2SO4])^3 NO | 8 | 8 | ([NO])^8 As(OH)_3 | 2 | 2 | ([As(OH)3])^2 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])^(-2) ([HNO3])^(-8) ([As2S3])^(-1) ([H2SO4])^3 ([NO])^8 ([As(OH)3])^2 = (([H2SO4])^3 ([NO])^8 ([As(OH)3])^2)/(([H2O])^2 ([HNO3])^8 [As2S3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + HNO_3 + As_2S_3 ⟶ H_2SO_4 + NO + As(OH)_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: 2 H_2O + 8 HNO_3 + As_2S_3 ⟶ 3 H_2SO_4 + 8 NO + 2 As(OH)_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 | 2 | -2 HNO_3 | 8 | -8 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 NO | 8 | 8 As(OH)_3 | 2 | 2 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 | 2 | -2 | -1/2 (Δ[H2O])/(Δt) HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) As_2S_3 | 1 | -1 | -(Δ[As2S3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) NO | 8 | 8 | 1/8 (Δ[NO])/(Δt) As(OH)_3 | 2 | 2 | 1/2 (Δ[As(OH)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 = -1/2 (Δ[H2O])/(Δt) = -1/8 (Δ[HNO3])/(Δt) = -(Δ[As2S3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = 1/8 (Δ[NO])/(Δt) = 1/2 (Δ[As(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + HNO_3 + As_2S_3 ⟶ H_2SO_4 + NO + As(OH)_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: 2 H_2O + 8 HNO_3 + As_2S_3 ⟶ 3 H_2SO_4 + 8 NO + 2 As(OH)_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 | 2 | -2 HNO_3 | 8 | -8 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 NO | 8 | 8 As(OH)_3 | 2 | 2 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 | 2 | -2 | -1/2 (Δ[H2O])/(Δt) HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) As_2S_3 | 1 | -1 | -(Δ[As2S3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) NO | 8 | 8 | 1/8 (Δ[NO])/(Δt) As(OH)_3 | 2 | 2 | 1/2 (Δ[As(OH)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 = -1/2 (Δ[H2O])/(Δt) = -1/8 (Δ[HNO3])/(Δt) = -(Δ[As2S3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = 1/8 (Δ[NO])/(Δt) = 1/2 (Δ[As(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | nitric acid | arsenic(III) sulfide | sulfuric acid | nitric oxide | arsenious acid formula | H_2O | HNO_3 | As_2S_3 | H_2SO_4 | NO | As(OH)_3 Hill formula | H_2O | HNO_3 | As_2S_3 | H_2O_4S | NO | AsH_3O_3 name | water | nitric acid | arsenic(III) sulfide | sulfuric acid | nitric oxide | arsenious acid IUPAC name | water | nitric acid | | sulfuric acid | nitric oxide | arsorous acid
| water | nitric acid | arsenic(III) sulfide | sulfuric acid | nitric oxide | arsenious acid formula | H_2O | HNO_3 | As_2S_3 | H_2SO_4 | NO | As(OH)_3 Hill formula | H_2O | HNO_3 | As_2S_3 | H_2O_4S | NO | AsH_3O_3 name | water | nitric acid | arsenic(III) sulfide | sulfuric acid | nitric oxide | arsenious acid IUPAC name | water | nitric acid | | sulfuric acid | nitric oxide | arsorous acid

Random Queries

formula of ammonium hexabromoplatinate
alternate names of 1,3-butanediol dimethacrylate vs ethylene glycol monobutyl ether acetate
alternate names of D-gamma-tocopherol
CAS number of cobalt dichloride vs praseodymium(III) sulfate
CAS number of zinc dichromate
coordination numbers of aluminum cation
name of bismuth silicate tetrasodium
molar mass of chlorine pentafluoride
ionic conductivity of alkali metal ions
NFPA health rating of lithium bromide