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HNO3 + Bi2S3 = H2O + S + NO + Bi(NO3)3

Input interpretation

HNO_3 (nitric acid) + Bi_2S_3 (bismuth sulfide) ⟶ H_2O (water) + S (mixed sulfur) + NO (nitric oxide) + Bi(NO3)3
HNO_3 (nitric acid) + Bi_2S_3 (bismuth sulfide) ⟶ H_2O (water) + S (mixed sulfur) + NO (nitric oxide) + Bi(NO3)3

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Bi_2S_3 ⟶ H_2O + S + NO + Bi(NO3)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Bi_2S_3 ⟶ c_3 H_2O + c_4 S + c_5 NO + c_6 Bi(NO3)3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Bi and S: H: | c_1 = 2 c_3 N: | c_1 = c_5 + 3 c_6 O: | 3 c_1 = c_3 + c_5 + 9 c_6 Bi: | 2 c_2 = c_6 S: | 3 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 4 c_4 = 3 c_5 = 2 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + Bi_2S_3 ⟶ 4 H_2O + 3 S + 2 NO + 2 Bi(NO3)3
Balance the chemical equation algebraically: HNO_3 + Bi_2S_3 ⟶ H_2O + S + NO + Bi(NO3)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Bi_2S_3 ⟶ c_3 H_2O + c_4 S + c_5 NO + c_6 Bi(NO3)3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Bi and S: H: | c_1 = 2 c_3 N: | c_1 = c_5 + 3 c_6 O: | 3 c_1 = c_3 + c_5 + 9 c_6 Bi: | 2 c_2 = c_6 S: | 3 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 4 c_4 = 3 c_5 = 2 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + Bi_2S_3 ⟶ 4 H_2O + 3 S + 2 NO + 2 Bi(NO3)3

Structures

+ ⟶ + + + Bi(NO3)3
+ ⟶ + + + Bi(NO3)3

Names

nitric acid + bismuth sulfide ⟶ water + mixed sulfur + nitric oxide + Bi(NO3)3
nitric acid + bismuth sulfide ⟶ water + mixed sulfur + nitric oxide + Bi(NO3)3

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Bi_2S_3 ⟶ H_2O + S + NO + Bi(NO3)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: 8 HNO_3 + Bi_2S_3 ⟶ 4 H_2O + 3 S + 2 NO + 2 Bi(NO3)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 | 8 | -8 Bi_2S_3 | 1 | -1 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 Bi(NO3)3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 8 | -8 | ([HNO3])^(-8) Bi_2S_3 | 1 | -1 | ([Bi2S3])^(-1) H_2O | 4 | 4 | ([H2O])^4 S | 3 | 3 | ([S])^3 NO | 2 | 2 | ([NO])^2 Bi(NO3)3 | 2 | 2 | ([Bi(NO3)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 = ([HNO3])^(-8) ([Bi2S3])^(-1) ([H2O])^4 ([S])^3 ([NO])^2 ([Bi(NO3)3])^2 = (([H2O])^4 ([S])^3 ([NO])^2 ([Bi(NO3)3])^2)/(([HNO3])^8 [Bi2S3])
Construct the equilibrium constant, K, expression for: HNO_3 + Bi_2S_3 ⟶ H_2O + S + NO + Bi(NO3)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: 8 HNO_3 + Bi_2S_3 ⟶ 4 H_2O + 3 S + 2 NO + 2 Bi(NO3)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 | 8 | -8 Bi_2S_3 | 1 | -1 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 Bi(NO3)3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 8 | -8 | ([HNO3])^(-8) Bi_2S_3 | 1 | -1 | ([Bi2S3])^(-1) H_2O | 4 | 4 | ([H2O])^4 S | 3 | 3 | ([S])^3 NO | 2 | 2 | ([NO])^2 Bi(NO3)3 | 2 | 2 | ([Bi(NO3)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 = ([HNO3])^(-8) ([Bi2S3])^(-1) ([H2O])^4 ([S])^3 ([NO])^2 ([Bi(NO3)3])^2 = (([H2O])^4 ([S])^3 ([NO])^2 ([Bi(NO3)3])^2)/(([HNO3])^8 [Bi2S3])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Bi_2S_3 ⟶ H_2O + S + NO + Bi(NO3)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: 8 HNO_3 + Bi_2S_3 ⟶ 4 H_2O + 3 S + 2 NO + 2 Bi(NO3)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 | 8 | -8 Bi_2S_3 | 1 | -1 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 Bi(NO3)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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) Bi_2S_3 | 1 | -1 | -(Δ[Bi2S3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) S | 3 | 3 | 1/3 (Δ[S])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) Bi(NO3)3 | 2 | 2 | 1/2 (Δ[Bi(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 = -1/8 (Δ[HNO3])/(Δt) = -(Δ[Bi2S3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/2 (Δ[Bi(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Bi_2S_3 ⟶ H_2O + S + NO + Bi(NO3)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: 8 HNO_3 + Bi_2S_3 ⟶ 4 H_2O + 3 S + 2 NO + 2 Bi(NO3)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 | 8 | -8 Bi_2S_3 | 1 | -1 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 Bi(NO3)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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) Bi_2S_3 | 1 | -1 | -(Δ[Bi2S3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) S | 3 | 3 | 1/3 (Δ[S])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) Bi(NO3)3 | 2 | 2 | 1/2 (Δ[Bi(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 = -1/8 (Δ[HNO3])/(Δt) = -(Δ[Bi2S3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/2 (Δ[Bi(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | bismuth sulfide | water | mixed sulfur | nitric oxide | Bi(NO3)3 formula | HNO_3 | Bi_2S_3 | H_2O | S | NO | Bi(NO3)3 Hill formula | HNO_3 | Bi_2S_3 | H_2O | S | NO | BiN3O9 name | nitric acid | bismuth sulfide | water | mixed sulfur | nitric oxide | IUPAC name | nitric acid | thioxo-(thioxobismuthanylthio)bismuthane | water | sulfur | nitric oxide |
| nitric acid | bismuth sulfide | water | mixed sulfur | nitric oxide | Bi(NO3)3 formula | HNO_3 | Bi_2S_3 | H_2O | S | NO | Bi(NO3)3 Hill formula | HNO_3 | Bi_2S_3 | H_2O | S | NO | BiN3O9 name | nitric acid | bismuth sulfide | water | mixed sulfur | nitric oxide | IUPAC name | nitric acid | thioxo-(thioxobismuthanylthio)bismuthane | water | sulfur | nitric oxide |

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