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HNO3 + SnS = H2O + H2SO4 + NO2 + H2SnO2

Input interpretation

HNO_3 nitric acid + SnS tin(II) sulfide ⟶ H_2O water + H_2SO_4 sulfuric acid + NO_2 nitrogen dioxide + Sn(OH)_2 tin(II) hydroxide
HNO_3 nitric acid + SnS tin(II) sulfide ⟶ H_2O water + H_2SO_4 sulfuric acid + NO_2 nitrogen dioxide + Sn(OH)_2 tin(II) hydroxide

Balanced equation

Balance the chemical equation algebraically: HNO_3 + SnS ⟶ H_2O + H_2SO_4 + NO_2 + Sn(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 SnS ⟶ c_3 H_2O + c_4 H_2SO_4 + c_5 NO_2 + c_6 Sn(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, S and Sn: H: | c_1 = 2 c_3 + 2 c_4 + 2 c_6 N: | c_1 = c_5 O: | 3 c_1 = c_3 + 4 c_4 + 2 c_5 + 2 c_6 S: | c_2 = c_4 Sn: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 8 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + SnS ⟶ 2 H_2O + H_2SO_4 + 8 NO_2 + Sn(OH)_2
Balance the chemical equation algebraically: HNO_3 + SnS ⟶ H_2O + H_2SO_4 + NO_2 + Sn(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 SnS ⟶ c_3 H_2O + c_4 H_2SO_4 + c_5 NO_2 + c_6 Sn(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, S and Sn: H: | c_1 = 2 c_3 + 2 c_4 + 2 c_6 N: | c_1 = c_5 O: | 3 c_1 = c_3 + 4 c_4 + 2 c_5 + 2 c_6 S: | c_2 = c_4 Sn: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 8 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + SnS ⟶ 2 H_2O + H_2SO_4 + 8 NO_2 + Sn(OH)_2

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

nitric acid + tin(II) sulfide ⟶ water + sulfuric acid + nitrogen dioxide + tin(II) hydroxide
nitric acid + tin(II) sulfide ⟶ water + sulfuric acid + nitrogen dioxide + tin(II) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + SnS ⟶ H_2O + H_2SO_4 + NO_2 + Sn(OH)_2 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 + SnS ⟶ 2 H_2O + H_2SO_4 + 8 NO_2 + Sn(OH)_2 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 SnS | 1 | -1 H_2O | 2 | 2 H_2SO_4 | 1 | 1 NO_2 | 8 | 8 Sn(OH)_2 | 1 | 1 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) SnS | 1 | -1 | ([SnS])^(-1) H_2O | 2 | 2 | ([H2O])^2 H_2SO_4 | 1 | 1 | [H2SO4] NO_2 | 8 | 8 | ([NO2])^8 Sn(OH)_2 | 1 | 1 | [Sn(OH)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) ([SnS])^(-1) ([H2O])^2 [H2SO4] ([NO2])^8 [Sn(OH)2] = (([H2O])^2 [H2SO4] ([NO2])^8 [Sn(OH)2])/(([HNO3])^8 [SnS])
Construct the equilibrium constant, K, expression for: HNO_3 + SnS ⟶ H_2O + H_2SO_4 + NO_2 + Sn(OH)_2 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 + SnS ⟶ 2 H_2O + H_2SO_4 + 8 NO_2 + Sn(OH)_2 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 SnS | 1 | -1 H_2O | 2 | 2 H_2SO_4 | 1 | 1 NO_2 | 8 | 8 Sn(OH)_2 | 1 | 1 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) SnS | 1 | -1 | ([SnS])^(-1) H_2O | 2 | 2 | ([H2O])^2 H_2SO_4 | 1 | 1 | [H2SO4] NO_2 | 8 | 8 | ([NO2])^8 Sn(OH)_2 | 1 | 1 | [Sn(OH)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) ([SnS])^(-1) ([H2O])^2 [H2SO4] ([NO2])^8 [Sn(OH)2] = (([H2O])^2 [H2SO4] ([NO2])^8 [Sn(OH)2])/(([HNO3])^8 [SnS])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + SnS ⟶ H_2O + H_2SO_4 + NO_2 + Sn(OH)_2 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 + SnS ⟶ 2 H_2O + H_2SO_4 + 8 NO_2 + Sn(OH)_2 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 SnS | 1 | -1 H_2O | 2 | 2 H_2SO_4 | 1 | 1 NO_2 | 8 | 8 Sn(OH)_2 | 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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) SnS | 1 | -1 | -(Δ[SnS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) NO_2 | 8 | 8 | 1/8 (Δ[NO2])/(Δt) Sn(OH)_2 | 1 | 1 | (Δ[Sn(OH)2])/(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[SnS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[H2SO4])/(Δt) = 1/8 (Δ[NO2])/(Δt) = (Δ[Sn(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + SnS ⟶ H_2O + H_2SO_4 + NO_2 + Sn(OH)_2 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 + SnS ⟶ 2 H_2O + H_2SO_4 + 8 NO_2 + Sn(OH)_2 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 SnS | 1 | -1 H_2O | 2 | 2 H_2SO_4 | 1 | 1 NO_2 | 8 | 8 Sn(OH)_2 | 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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) SnS | 1 | -1 | -(Δ[SnS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) NO_2 | 8 | 8 | 1/8 (Δ[NO2])/(Δt) Sn(OH)_2 | 1 | 1 | (Δ[Sn(OH)2])/(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[SnS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[H2SO4])/(Δt) = 1/8 (Δ[NO2])/(Δt) = (Δ[Sn(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | tin(II) sulfide | water | sulfuric acid | nitrogen dioxide | tin(II) hydroxide formula | HNO_3 | SnS | H_2O | H_2SO_4 | NO_2 | Sn(OH)_2 Hill formula | HNO_3 | SSn | H_2O | H_2O_4S | NO_2 | H_2O_2Sn name | nitric acid | tin(II) sulfide | water | sulfuric acid | nitrogen dioxide | tin(II) hydroxide IUPAC name | nitric acid | thioxotin | water | sulfuric acid | Nitrogen dioxide | stannous dihydroxide
| nitric acid | tin(II) sulfide | water | sulfuric acid | nitrogen dioxide | tin(II) hydroxide formula | HNO_3 | SnS | H_2O | H_2SO_4 | NO_2 | Sn(OH)_2 Hill formula | HNO_3 | SSn | H_2O | H_2O_4S | NO_2 | H_2O_2Sn name | nitric acid | tin(II) sulfide | water | sulfuric acid | nitrogen dioxide | tin(II) hydroxide IUPAC name | nitric acid | thioxotin | water | sulfuric acid | Nitrogen dioxide | stannous dihydroxide

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