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HCl + HNO3 + SnCl2 = H2O + N2O + SnCl4

Input interpretation

HCl hydrogen chloride + HNO_3 nitric acid + SnCl_2 stannous chloride ⟶ H_2O water + N_2O nitrous oxide + SnCl_4 stannic chloride
HCl hydrogen chloride + HNO_3 nitric acid + SnCl_2 stannous chloride ⟶ H_2O water + N_2O nitrous oxide + SnCl_4 stannic chloride

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + SnCl_2 ⟶ H_2O + N_2O + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 N_2O + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and Sn: Cl: | c_1 + 2 c_3 = 4 c_6 H: | c_1 + c_2 = 2 c_4 N: | c_2 = 2 c_5 O: | 3 c_2 = c_4 + c_5 Sn: | 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 2 c_3 = 4 c_4 = 5 c_5 = 1 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HCl + 2 HNO_3 + 4 SnCl_2 ⟶ 5 H_2O + N_2O + 4 SnCl_4
Balance the chemical equation algebraically: HCl + HNO_3 + SnCl_2 ⟶ H_2O + N_2O + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 N_2O + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and Sn: Cl: | c_1 + 2 c_3 = 4 c_6 H: | c_1 + c_2 = 2 c_4 N: | c_2 = 2 c_5 O: | 3 c_2 = c_4 + c_5 Sn: | 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 2 c_3 = 4 c_4 = 5 c_5 = 1 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HCl + 2 HNO_3 + 4 SnCl_2 ⟶ 5 H_2O + N_2O + 4 SnCl_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + SnCl_2 ⟶ H_2O + N_2O + 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: 8 HCl + 2 HNO_3 + 4 SnCl_2 ⟶ 5 H_2O + N_2O + 4 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 | 8 | -8 HNO_3 | 2 | -2 SnCl_2 | 4 | -4 H_2O | 5 | 5 N_2O | 1 | 1 SnCl_4 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 8 | -8 | ([HCl])^(-8) HNO_3 | 2 | -2 | ([HNO3])^(-2) SnCl_2 | 4 | -4 | ([SnCl2])^(-4) H_2O | 5 | 5 | ([H2O])^5 N_2O | 1 | 1 | [N2O] SnCl_4 | 4 | 4 | ([SnCl4])^4 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])^(-8) ([HNO3])^(-2) ([SnCl2])^(-4) ([H2O])^5 [N2O] ([SnCl4])^4 = (([H2O])^5 [N2O] ([SnCl4])^4)/(([HCl])^8 ([HNO3])^2 ([SnCl2])^4)
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + SnCl_2 ⟶ H_2O + N_2O + 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: 8 HCl + 2 HNO_3 + 4 SnCl_2 ⟶ 5 H_2O + N_2O + 4 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 | 8 | -8 HNO_3 | 2 | -2 SnCl_2 | 4 | -4 H_2O | 5 | 5 N_2O | 1 | 1 SnCl_4 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 8 | -8 | ([HCl])^(-8) HNO_3 | 2 | -2 | ([HNO3])^(-2) SnCl_2 | 4 | -4 | ([SnCl2])^(-4) H_2O | 5 | 5 | ([H2O])^5 N_2O | 1 | 1 | [N2O] SnCl_4 | 4 | 4 | ([SnCl4])^4 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])^(-8) ([HNO3])^(-2) ([SnCl2])^(-4) ([H2O])^5 [N2O] ([SnCl4])^4 = (([H2O])^5 [N2O] ([SnCl4])^4)/(([HCl])^8 ([HNO3])^2 ([SnCl2])^4)

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + SnCl_2 ⟶ H_2O + N_2O + 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: 8 HCl + 2 HNO_3 + 4 SnCl_2 ⟶ 5 H_2O + N_2O + 4 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 | 8 | -8 HNO_3 | 2 | -2 SnCl_2 | 4 | -4 H_2O | 5 | 5 N_2O | 1 | 1 SnCl_4 | 4 | 4 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 | 8 | -8 | -1/8 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) SnCl_2 | 4 | -4 | -1/4 (Δ[SnCl2])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) N_2O | 1 | 1 | (Δ[N2O])/(Δt) SnCl_4 | 4 | 4 | 1/4 (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 = -1/8 (Δ[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/4 (Δ[SnCl2])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[N2O])/(Δt) = 1/4 (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 + SnCl_2 ⟶ H_2O + N_2O + 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: 8 HCl + 2 HNO_3 + 4 SnCl_2 ⟶ 5 H_2O + N_2O + 4 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 | 8 | -8 HNO_3 | 2 | -2 SnCl_2 | 4 | -4 H_2O | 5 | 5 N_2O | 1 | 1 SnCl_4 | 4 | 4 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 | 8 | -8 | -1/8 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) SnCl_2 | 4 | -4 | -1/4 (Δ[SnCl2])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) N_2O | 1 | 1 | (Δ[N2O])/(Δt) SnCl_4 | 4 | 4 | 1/4 (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 = -1/8 (Δ[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/4 (Δ[SnCl2])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[N2O])/(Δt) = 1/4 (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | stannous chloride | water | nitrous oxide | stannic chloride formula | HCl | HNO_3 | SnCl_2 | H_2O | N_2O | SnCl_4 Hill formula | ClH | HNO_3 | Cl_2Sn | H_2O | N_2O | Cl_4Sn name | hydrogen chloride | nitric acid | stannous chloride | water | nitrous oxide | stannic chloride IUPAC name | hydrogen chloride | nitric acid | dichlorotin | water | nitrous oxide | tetrachlorostannane
| hydrogen chloride | nitric acid | stannous chloride | water | nitrous oxide | stannic chloride formula | HCl | HNO_3 | SnCl_2 | H_2O | N_2O | SnCl_4 Hill formula | ClH | HNO_3 | Cl_2Sn | H_2O | N_2O | Cl_4Sn name | hydrogen chloride | nitric acid | stannous chloride | water | nitrous oxide | stannic chloride IUPAC name | hydrogen chloride | nitric acid | dichlorotin | water | nitrous oxide | tetrachlorostannane

Substance properties

| hydrogen chloride | nitric acid | stannous chloride | water | nitrous oxide | stannic chloride molar mass | 36.46 g/mol | 63.012 g/mol | 189.6 g/mol | 18.015 g/mol | 44.013 g/mol | 260.5 g/mol phase | gas (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | -114.17 °C | -41.6 °C | 246 °C | 0 °C | -91 °C | -33 °C boiling point | -85 °C | 83 °C | 652 °C | 99.9839 °C | -88 °C | 114 °C density | 0.00149 g/cm^3 (at 25 °C) | 1.5129 g/cm^3 | 3.354 g/cm^3 | 1 g/cm^3 | 0.001799 g/cm^3 (at 25 °C) | 2.226 g/cm^3 solubility in water | miscible | miscible | | | | soluble surface tension | | | | 0.0728 N/m | 0.00175 N/m | dynamic viscosity | | 7.6×10^-4 Pa s (at 25 °C) | 7 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | 5.8×10^-4 Pa s (at 60 °C) odor | | | odorless | odorless | |
| hydrogen chloride | nitric acid | stannous chloride | water | nitrous oxide | stannic chloride molar mass | 36.46 g/mol | 63.012 g/mol | 189.6 g/mol | 18.015 g/mol | 44.013 g/mol | 260.5 g/mol phase | gas (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | -114.17 °C | -41.6 °C | 246 °C | 0 °C | -91 °C | -33 °C boiling point | -85 °C | 83 °C | 652 °C | 99.9839 °C | -88 °C | 114 °C density | 0.00149 g/cm^3 (at 25 °C) | 1.5129 g/cm^3 | 3.354 g/cm^3 | 1 g/cm^3 | 0.001799 g/cm^3 (at 25 °C) | 2.226 g/cm^3 solubility in water | miscible | miscible | | | | soluble surface tension | | | | 0.0728 N/m | 0.00175 N/m | dynamic viscosity | | 7.6×10^-4 Pa s (at 25 °C) | 7 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | 5.8×10^-4 Pa s (at 60 °C) odor | | | odorless | odorless | |

Units

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