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H2O + HNO3 + As2Se3 = NO + H3AsO4 + H2SeO4

Input interpretation

H_2O water + HNO_3 nitric acid + As_2Se_3 arsenic(III) selenide ⟶ NO nitric oxide + H_3AsO_4 arsenic acid, solid + H_2SeO_4 selenic acid
H_2O water + HNO_3 nitric acid + As_2Se_3 arsenic(III) selenide ⟶ NO nitric oxide + H_3AsO_4 arsenic acid, solid + H_2SeO_4 selenic acid

Balanced equation

Balance the chemical equation algebraically: H_2O + HNO_3 + As_2Se_3 ⟶ NO + H_3AsO_4 + H_2SeO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 As_2Se_3 ⟶ c_4 NO + c_5 H_3AsO_4 + c_6 H_2SeO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N, As and Se: H: | 2 c_1 + c_2 = 3 c_5 + 2 c_6 O: | c_1 + 3 c_2 = c_4 + 4 c_5 + 4 c_6 N: | c_2 = c_4 As: | 2 c_3 = c_5 Se: | 3 c_3 = 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 = 4/3 c_2 = 28/3 c_3 = 1 c_4 = 28/3 c_5 = 2 c_6 = 3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 4 c_2 = 28 c_3 = 3 c_4 = 28 c_5 = 6 c_6 = 9 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 28 HNO_3 + 3 As_2Se_3 ⟶ 28 NO + 6 H_3AsO_4 + 9 H_2SeO_4
Balance the chemical equation algebraically: H_2O + HNO_3 + As_2Se_3 ⟶ NO + H_3AsO_4 + H_2SeO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 As_2Se_3 ⟶ c_4 NO + c_5 H_3AsO_4 + c_6 H_2SeO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N, As and Se: H: | 2 c_1 + c_2 = 3 c_5 + 2 c_6 O: | c_1 + 3 c_2 = c_4 + 4 c_5 + 4 c_6 N: | c_2 = c_4 As: | 2 c_3 = c_5 Se: | 3 c_3 = 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 = 4/3 c_2 = 28/3 c_3 = 1 c_4 = 28/3 c_5 = 2 c_6 = 3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 4 c_2 = 28 c_3 = 3 c_4 = 28 c_5 = 6 c_6 = 9 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 28 HNO_3 + 3 As_2Se_3 ⟶ 28 NO + 6 H_3AsO_4 + 9 H_2SeO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + nitric acid + arsenic(III) selenide ⟶ nitric oxide + arsenic acid, solid + selenic acid
water + nitric acid + arsenic(III) selenide ⟶ nitric oxide + arsenic acid, solid + selenic acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + As_2Se_3 ⟶ NO + H_3AsO_4 + H_2SeO_4 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: 4 H_2O + 28 HNO_3 + 3 As_2Se_3 ⟶ 28 NO + 6 H_3AsO_4 + 9 H_2SeO_4 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 | 4 | -4 HNO_3 | 28 | -28 As_2Se_3 | 3 | -3 NO | 28 | 28 H_3AsO_4 | 6 | 6 H_2SeO_4 | 9 | 9 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) HNO_3 | 28 | -28 | ([HNO3])^(-28) As_2Se_3 | 3 | -3 | ([As2Se3])^(-3) NO | 28 | 28 | ([NO])^28 H_3AsO_4 | 6 | 6 | ([H3AsO4])^6 H_2SeO_4 | 9 | 9 | ([H2SeO4])^9 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])^(-4) ([HNO3])^(-28) ([As2Se3])^(-3) ([NO])^28 ([H3AsO4])^6 ([H2SeO4])^9 = (([NO])^28 ([H3AsO4])^6 ([H2SeO4])^9)/(([H2O])^4 ([HNO3])^28 ([As2Se3])^3)
Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + As_2Se_3 ⟶ NO + H_3AsO_4 + H_2SeO_4 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: 4 H_2O + 28 HNO_3 + 3 As_2Se_3 ⟶ 28 NO + 6 H_3AsO_4 + 9 H_2SeO_4 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 | 4 | -4 HNO_3 | 28 | -28 As_2Se_3 | 3 | -3 NO | 28 | 28 H_3AsO_4 | 6 | 6 H_2SeO_4 | 9 | 9 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) HNO_3 | 28 | -28 | ([HNO3])^(-28) As_2Se_3 | 3 | -3 | ([As2Se3])^(-3) NO | 28 | 28 | ([NO])^28 H_3AsO_4 | 6 | 6 | ([H3AsO4])^6 H_2SeO_4 | 9 | 9 | ([H2SeO4])^9 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])^(-4) ([HNO3])^(-28) ([As2Se3])^(-3) ([NO])^28 ([H3AsO4])^6 ([H2SeO4])^9 = (([NO])^28 ([H3AsO4])^6 ([H2SeO4])^9)/(([H2O])^4 ([HNO3])^28 ([As2Se3])^3)

Rate of reaction

Construct the rate of reaction expression for: H_2O + HNO_3 + As_2Se_3 ⟶ NO + H_3AsO_4 + H_2SeO_4 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: 4 H_2O + 28 HNO_3 + 3 As_2Se_3 ⟶ 28 NO + 6 H_3AsO_4 + 9 H_2SeO_4 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 | 4 | -4 HNO_3 | 28 | -28 As_2Se_3 | 3 | -3 NO | 28 | 28 H_3AsO_4 | 6 | 6 H_2SeO_4 | 9 | 9 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 | 4 | -4 | -1/4 (Δ[H2O])/(Δt) HNO_3 | 28 | -28 | -1/28 (Δ[HNO3])/(Δt) As_2Se_3 | 3 | -3 | -1/3 (Δ[As2Se3])/(Δt) NO | 28 | 28 | 1/28 (Δ[NO])/(Δt) H_3AsO_4 | 6 | 6 | 1/6 (Δ[H3AsO4])/(Δt) H_2SeO_4 | 9 | 9 | 1/9 (Δ[H2SeO4])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/28 (Δ[HNO3])/(Δt) = -1/3 (Δ[As2Se3])/(Δt) = 1/28 (Δ[NO])/(Δt) = 1/6 (Δ[H3AsO4])/(Δt) = 1/9 (Δ[H2SeO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + HNO_3 + As_2Se_3 ⟶ NO + H_3AsO_4 + H_2SeO_4 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: 4 H_2O + 28 HNO_3 + 3 As_2Se_3 ⟶ 28 NO + 6 H_3AsO_4 + 9 H_2SeO_4 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 | 4 | -4 HNO_3 | 28 | -28 As_2Se_3 | 3 | -3 NO | 28 | 28 H_3AsO_4 | 6 | 6 H_2SeO_4 | 9 | 9 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 | 4 | -4 | -1/4 (Δ[H2O])/(Δt) HNO_3 | 28 | -28 | -1/28 (Δ[HNO3])/(Δt) As_2Se_3 | 3 | -3 | -1/3 (Δ[As2Se3])/(Δt) NO | 28 | 28 | 1/28 (Δ[NO])/(Δt) H_3AsO_4 | 6 | 6 | 1/6 (Δ[H3AsO4])/(Δt) H_2SeO_4 | 9 | 9 | 1/9 (Δ[H2SeO4])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/28 (Δ[HNO3])/(Δt) = -1/3 (Δ[As2Se3])/(Δt) = 1/28 (Δ[NO])/(Δt) = 1/6 (Δ[H3AsO4])/(Δt) = 1/9 (Δ[H2SeO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | nitric acid | arsenic(III) selenide | nitric oxide | arsenic acid, solid | selenic acid formula | H_2O | HNO_3 | As_2Se_3 | NO | H_3AsO_4 | H_2SeO_4 Hill formula | H_2O | HNO_3 | As_2Se_3 | NO | AsH_3O_4 | H_2O_4Se name | water | nitric acid | arsenic(III) selenide | nitric oxide | arsenic acid, solid | selenic acid IUPAC name | water | nitric acid | | nitric oxide | arsoric acid | selenic acid
| water | nitric acid | arsenic(III) selenide | nitric oxide | arsenic acid, solid | selenic acid formula | H_2O | HNO_3 | As_2Se_3 | NO | H_3AsO_4 | H_2SeO_4 Hill formula | H_2O | HNO_3 | As_2Se_3 | NO | AsH_3O_4 | H_2O_4Se name | water | nitric acid | arsenic(III) selenide | nitric oxide | arsenic acid, solid | selenic acid IUPAC name | water | nitric acid | | nitric oxide | arsoric acid | selenic acid

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