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HCl + SnCl2 + HNO2 = H2O + NO + SnCl4

Input interpretation

HCl hydrogen chloride + SnCl_2 stannous chloride + HNO_2 nitrous acid ⟶ H_2O water + NO nitric oxide + SnCl_4 stannic chloride
HCl hydrogen chloride + SnCl_2 stannous chloride + HNO_2 nitrous acid ⟶ H_2O water + NO nitric oxide + SnCl_4 stannic chloride

Balanced equation

Balance the chemical equation algebraically: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 SnCl_2 + c_3 HNO_2 ⟶ c_4 H_2O + c_5 NO + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Sn, N and O: Cl: | c_1 + 2 c_2 = 4 c_6 H: | c_1 + c_3 = 2 c_4 Sn: | c_2 = c_6 N: | c_3 = c_5 O: | 2 c_3 = c_4 + c_5 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 = 2 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4
Balance the chemical equation algebraically: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 SnCl_2 + c_3 HNO_2 ⟶ c_4 H_2O + c_5 NO + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Sn, N and O: Cl: | c_1 + 2 c_2 = 4 c_6 H: | c_1 + c_3 = 2 c_4 Sn: | c_2 = c_6 N: | c_3 = c_5 O: | 2 c_3 = c_4 + c_5 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 = 2 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

hydrogen chloride + stannous chloride + nitrous acid ⟶ water + nitric oxide + stannic chloride
hydrogen chloride + stannous chloride + nitrous acid ⟶ water + nitric oxide + stannic chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_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: 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) SnCl_2 | 1 | -1 | ([SnCl2])^(-1) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO | 2 | 2 | ([NO])^2 SnCl_4 | 1 | 1 | [SnCl4] 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 = ([HCl])^(-2) ([SnCl2])^(-1) ([HNO2])^(-2) ([H2O])^2 ([NO])^2 [SnCl4] = (([H2O])^2 ([NO])^2 [SnCl4])/(([HCl])^2 [SnCl2] ([HNO2])^2)
Construct the equilibrium constant, K, expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_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: 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) SnCl_2 | 1 | -1 | ([SnCl2])^(-1) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO | 2 | 2 | ([NO])^2 SnCl_4 | 1 | 1 | [SnCl4] 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 = ([HCl])^(-2) ([SnCl2])^(-1) ([HNO2])^(-2) ([H2O])^2 ([NO])^2 [SnCl4] = (([H2O])^2 ([NO])^2 [SnCl4])/(([HCl])^2 [SnCl2] ([HNO2])^2)

Rate of reaction

Construct the rate of reaction expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_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: 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(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[HCl])/(Δt) = -(Δ[SnCl2])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_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: 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(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[HCl])/(Δt) = -(Δ[SnCl2])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride formula | HCl | SnCl_2 | HNO_2 | H_2O | NO | SnCl_4 Hill formula | ClH | Cl_2Sn | HNO_2 | H_2O | NO | Cl_4Sn name | hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride IUPAC name | hydrogen chloride | dichlorotin | nitrous acid | water | nitric oxide | tetrachlorostannane
| hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride formula | HCl | SnCl_2 | HNO_2 | H_2O | NO | SnCl_4 Hill formula | ClH | Cl_2Sn | HNO_2 | H_2O | NO | Cl_4Sn name | hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride IUPAC name | hydrogen chloride | dichlorotin | nitrous acid | water | nitric oxide | tetrachlorostannane

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