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HNO3 + Sn = H2O + NO + NO2 + H2SnO3

Input interpretation

HNO_3 nitric acid + Sn white tin ⟶ H_2O water + NO nitric oxide + NO_2 nitrogen dioxide + H2SnO3
HNO_3 nitric acid + Sn white tin ⟶ H_2O water + NO nitric oxide + NO_2 nitrogen dioxide + H2SnO3

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Sn ⟶ H_2O + NO + NO_2 + H2SnO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Sn ⟶ c_3 H_2O + c_4 NO + c_5 NO_2 + c_6 H2SnO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Sn: H: | c_1 = 2 c_3 + 2 c_6 N: | c_1 = c_4 + c_5 O: | 3 c_1 = c_3 + c_4 + 2 c_5 + 3 c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1/2 - 1 c_3 = 1 c_4 = c_1/2 - 2 c_5 = c_1/2 + 2 c_6 = c_1/2 - 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 8 and solve for the remaining coefficients: c_1 = 8 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 6 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + 3 Sn ⟶ H_2O + 2 NO + 6 NO_2 + 3 H2SnO3
Balance the chemical equation algebraically: HNO_3 + Sn ⟶ H_2O + NO + NO_2 + H2SnO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Sn ⟶ c_3 H_2O + c_4 NO + c_5 NO_2 + c_6 H2SnO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Sn: H: | c_1 = 2 c_3 + 2 c_6 N: | c_1 = c_4 + c_5 O: | 3 c_1 = c_3 + c_4 + 2 c_5 + 3 c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1/2 - 1 c_3 = 1 c_4 = c_1/2 - 2 c_5 = c_1/2 + 2 c_6 = c_1/2 - 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 8 and solve for the remaining coefficients: c_1 = 8 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 6 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + 3 Sn ⟶ H_2O + 2 NO + 6 NO_2 + 3 H2SnO3

Structures

+ ⟶ + + + H2SnO3
+ ⟶ + + + H2SnO3

Names

nitric acid + white tin ⟶ water + nitric oxide + nitrogen dioxide + H2SnO3
nitric acid + white tin ⟶ water + nitric oxide + nitrogen dioxide + H2SnO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Sn ⟶ H_2O + NO + NO_2 + H2SnO3 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 + 3 Sn ⟶ H_2O + 2 NO + 6 NO_2 + 3 H2SnO3 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 Sn | 3 | -3 H_2O | 1 | 1 NO | 2 | 2 NO_2 | 6 | 6 H2SnO3 | 3 | 3 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) Sn | 3 | -3 | ([Sn])^(-3) H_2O | 1 | 1 | [H2O] NO | 2 | 2 | ([NO])^2 NO_2 | 6 | 6 | ([NO2])^6 H2SnO3 | 3 | 3 | ([H2SnO3])^3 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) ([Sn])^(-3) [H2O] ([NO])^2 ([NO2])^6 ([H2SnO3])^3 = ([H2O] ([NO])^2 ([NO2])^6 ([H2SnO3])^3)/(([HNO3])^8 ([Sn])^3)
Construct the equilibrium constant, K, expression for: HNO_3 + Sn ⟶ H_2O + NO + NO_2 + H2SnO3 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 + 3 Sn ⟶ H_2O + 2 NO + 6 NO_2 + 3 H2SnO3 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 Sn | 3 | -3 H_2O | 1 | 1 NO | 2 | 2 NO_2 | 6 | 6 H2SnO3 | 3 | 3 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) Sn | 3 | -3 | ([Sn])^(-3) H_2O | 1 | 1 | [H2O] NO | 2 | 2 | ([NO])^2 NO_2 | 6 | 6 | ([NO2])^6 H2SnO3 | 3 | 3 | ([H2SnO3])^3 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) ([Sn])^(-3) [H2O] ([NO])^2 ([NO2])^6 ([H2SnO3])^3 = ([H2O] ([NO])^2 ([NO2])^6 ([H2SnO3])^3)/(([HNO3])^8 ([Sn])^3)

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Sn ⟶ H_2O + NO + NO_2 + H2SnO3 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 + 3 Sn ⟶ H_2O + 2 NO + 6 NO_2 + 3 H2SnO3 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 Sn | 3 | -3 H_2O | 1 | 1 NO | 2 | 2 NO_2 | 6 | 6 H2SnO3 | 3 | 3 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) Sn | 3 | -3 | -1/3 (Δ[Sn])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) NO_2 | 6 | 6 | 1/6 (Δ[NO2])/(Δt) H2SnO3 | 3 | 3 | 1/3 (Δ[H2SnO3])/(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) = -1/3 (Δ[Sn])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/6 (Δ[NO2])/(Δt) = 1/3 (Δ[H2SnO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Sn ⟶ H_2O + NO + NO_2 + H2SnO3 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 + 3 Sn ⟶ H_2O + 2 NO + 6 NO_2 + 3 H2SnO3 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 Sn | 3 | -3 H_2O | 1 | 1 NO | 2 | 2 NO_2 | 6 | 6 H2SnO3 | 3 | 3 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) Sn | 3 | -3 | -1/3 (Δ[Sn])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) NO_2 | 6 | 6 | 1/6 (Δ[NO2])/(Δt) H2SnO3 | 3 | 3 | 1/3 (Δ[H2SnO3])/(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) = -1/3 (Δ[Sn])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/6 (Δ[NO2])/(Δt) = 1/3 (Δ[H2SnO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | white tin | water | nitric oxide | nitrogen dioxide | H2SnO3 formula | HNO_3 | Sn | H_2O | NO | NO_2 | H2SnO3 Hill formula | HNO_3 | Sn | H_2O | NO | NO_2 | H2O3Sn name | nitric acid | white tin | water | nitric oxide | nitrogen dioxide | IUPAC name | nitric acid | tin | water | nitric oxide | Nitrogen dioxide |
| nitric acid | white tin | water | nitric oxide | nitrogen dioxide | H2SnO3 formula | HNO_3 | Sn | H_2O | NO | NO_2 | H2SnO3 Hill formula | HNO_3 | Sn | H_2O | NO | NO_2 | H2O3Sn name | nitric acid | white tin | water | nitric oxide | nitrogen dioxide | IUPAC name | nitric acid | tin | water | nitric oxide | Nitrogen dioxide |

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