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HCl + Na2SO3 + SnCl2 = H2O + NaCl + SnCl4 + SnS2

Input interpretation

HCl hydrogen chloride + Na_2SO_3 sodium sulfite + SnCl_2 stannous chloride ⟶ H_2O water + NaCl sodium chloride + SnCl_4 stannic chloride + SnS_2 tin(IV) sulfide
HCl hydrogen chloride + Na_2SO_3 sodium sulfite + SnCl_2 stannous chloride ⟶ H_2O water + NaCl sodium chloride + SnCl_4 stannic chloride + SnS_2 tin(IV) sulfide

Balanced equation

Balance the chemical equation algebraically: HCl + Na_2SO_3 + SnCl_2 ⟶ H_2O + NaCl + SnCl_4 + SnS_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Na_2SO_3 + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 NaCl + c_6 SnCl_4 + c_7 SnS_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O, S and Sn: Cl: | c_1 + 2 c_3 = c_5 + 4 c_6 H: | c_1 = 2 c_4 Na: | 2 c_2 = c_5 O: | 3 c_2 = c_4 S: | c_2 = 2 c_7 Sn: | c_3 = c_6 + c_7 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_7 = 1 and solve the system of equations for the remaining coefficients: c_1 = 12 c_2 = 2 c_3 = 6 c_4 = 6 c_5 = 4 c_6 = 5 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HCl + 2 Na_2SO_3 + 6 SnCl_2 ⟶ 6 H_2O + 4 NaCl + 5 SnCl_4 + SnS_2
Balance the chemical equation algebraically: HCl + Na_2SO_3 + SnCl_2 ⟶ H_2O + NaCl + SnCl_4 + SnS_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Na_2SO_3 + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 NaCl + c_6 SnCl_4 + c_7 SnS_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O, S and Sn: Cl: | c_1 + 2 c_3 = c_5 + 4 c_6 H: | c_1 = 2 c_4 Na: | 2 c_2 = c_5 O: | 3 c_2 = c_4 S: | c_2 = 2 c_7 Sn: | c_3 = c_6 + c_7 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_7 = 1 and solve the system of equations for the remaining coefficients: c_1 = 12 c_2 = 2 c_3 = 6 c_4 = 6 c_5 = 4 c_6 = 5 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HCl + 2 Na_2SO_3 + 6 SnCl_2 ⟶ 6 H_2O + 4 NaCl + 5 SnCl_4 + SnS_2

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

hydrogen chloride + sodium sulfite + stannous chloride ⟶ water + sodium chloride + stannic chloride + tin(IV) sulfide
hydrogen chloride + sodium sulfite + stannous chloride ⟶ water + sodium chloride + stannic chloride + tin(IV) sulfide

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + Na_2SO_3 + SnCl_2 ⟶ H_2O + NaCl + SnCl_4 + SnS_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: 12 HCl + 2 Na_2SO_3 + 6 SnCl_2 ⟶ 6 H_2O + 4 NaCl + 5 SnCl_4 + SnS_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 HCl | 12 | -12 Na_2SO_3 | 2 | -2 SnCl_2 | 6 | -6 H_2O | 6 | 6 NaCl | 4 | 4 SnCl_4 | 5 | 5 SnS_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 12 | -12 | ([HCl])^(-12) Na_2SO_3 | 2 | -2 | ([Na2SO3])^(-2) SnCl_2 | 6 | -6 | ([SnCl2])^(-6) H_2O | 6 | 6 | ([H2O])^6 NaCl | 4 | 4 | ([NaCl])^4 SnCl_4 | 5 | 5 | ([SnCl4])^5 SnS_2 | 1 | 1 | [SnS2] 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])^(-12) ([Na2SO3])^(-2) ([SnCl2])^(-6) ([H2O])^6 ([NaCl])^4 ([SnCl4])^5 [SnS2] = (([H2O])^6 ([NaCl])^4 ([SnCl4])^5 [SnS2])/(([HCl])^12 ([Na2SO3])^2 ([SnCl2])^6)
Construct the equilibrium constant, K, expression for: HCl + Na_2SO_3 + SnCl_2 ⟶ H_2O + NaCl + SnCl_4 + SnS_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: 12 HCl + 2 Na_2SO_3 + 6 SnCl_2 ⟶ 6 H_2O + 4 NaCl + 5 SnCl_4 + SnS_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 HCl | 12 | -12 Na_2SO_3 | 2 | -2 SnCl_2 | 6 | -6 H_2O | 6 | 6 NaCl | 4 | 4 SnCl_4 | 5 | 5 SnS_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 12 | -12 | ([HCl])^(-12) Na_2SO_3 | 2 | -2 | ([Na2SO3])^(-2) SnCl_2 | 6 | -6 | ([SnCl2])^(-6) H_2O | 6 | 6 | ([H2O])^6 NaCl | 4 | 4 | ([NaCl])^4 SnCl_4 | 5 | 5 | ([SnCl4])^5 SnS_2 | 1 | 1 | [SnS2] 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])^(-12) ([Na2SO3])^(-2) ([SnCl2])^(-6) ([H2O])^6 ([NaCl])^4 ([SnCl4])^5 [SnS2] = (([H2O])^6 ([NaCl])^4 ([SnCl4])^5 [SnS2])/(([HCl])^12 ([Na2SO3])^2 ([SnCl2])^6)

Rate of reaction

Construct the rate of reaction expression for: HCl + Na_2SO_3 + SnCl_2 ⟶ H_2O + NaCl + SnCl_4 + SnS_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: 12 HCl + 2 Na_2SO_3 + 6 SnCl_2 ⟶ 6 H_2O + 4 NaCl + 5 SnCl_4 + SnS_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 HCl | 12 | -12 Na_2SO_3 | 2 | -2 SnCl_2 | 6 | -6 H_2O | 6 | 6 NaCl | 4 | 4 SnCl_4 | 5 | 5 SnS_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 HCl | 12 | -12 | -1/12 (Δ[HCl])/(Δt) Na_2SO_3 | 2 | -2 | -1/2 (Δ[Na2SO3])/(Δt) SnCl_2 | 6 | -6 | -1/6 (Δ[SnCl2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) NaCl | 4 | 4 | 1/4 (Δ[NaCl])/(Δt) SnCl_4 | 5 | 5 | 1/5 (Δ[SnCl4])/(Δt) SnS_2 | 1 | 1 | (Δ[SnS2])/(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 = -1/12 (Δ[HCl])/(Δt) = -1/2 (Δ[Na2SO3])/(Δt) = -1/6 (Δ[SnCl2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/4 (Δ[NaCl])/(Δt) = 1/5 (Δ[SnCl4])/(Δt) = (Δ[SnS2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + Na_2SO_3 + SnCl_2 ⟶ H_2O + NaCl + SnCl_4 + SnS_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: 12 HCl + 2 Na_2SO_3 + 6 SnCl_2 ⟶ 6 H_2O + 4 NaCl + 5 SnCl_4 + SnS_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 HCl | 12 | -12 Na_2SO_3 | 2 | -2 SnCl_2 | 6 | -6 H_2O | 6 | 6 NaCl | 4 | 4 SnCl_4 | 5 | 5 SnS_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 HCl | 12 | -12 | -1/12 (Δ[HCl])/(Δt) Na_2SO_3 | 2 | -2 | -1/2 (Δ[Na2SO3])/(Δt) SnCl_2 | 6 | -6 | -1/6 (Δ[SnCl2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) NaCl | 4 | 4 | 1/4 (Δ[NaCl])/(Δt) SnCl_4 | 5 | 5 | 1/5 (Δ[SnCl4])/(Δt) SnS_2 | 1 | 1 | (Δ[SnS2])/(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 = -1/12 (Δ[HCl])/(Δt) = -1/2 (Δ[Na2SO3])/(Δt) = -1/6 (Δ[SnCl2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/4 (Δ[NaCl])/(Δt) = 1/5 (Δ[SnCl4])/(Δt) = (Δ[SnS2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | sodium sulfite | stannous chloride | water | sodium chloride | stannic chloride | tin(IV) sulfide formula | HCl | Na_2SO_3 | SnCl_2 | H_2O | NaCl | SnCl_4 | SnS_2 Hill formula | ClH | Na_2O_3S | Cl_2Sn | H_2O | ClNa | Cl_4Sn | S_2Sn name | hydrogen chloride | sodium sulfite | stannous chloride | water | sodium chloride | stannic chloride | tin(IV) sulfide IUPAC name | hydrogen chloride | disodium sulfite | dichlorotin | water | sodium chloride | tetrachlorostannane | tin(+4) cation disulfide
| hydrogen chloride | sodium sulfite | stannous chloride | water | sodium chloride | stannic chloride | tin(IV) sulfide formula | HCl | Na_2SO_3 | SnCl_2 | H_2O | NaCl | SnCl_4 | SnS_2 Hill formula | ClH | Na_2O_3S | Cl_2Sn | H_2O | ClNa | Cl_4Sn | S_2Sn name | hydrogen chloride | sodium sulfite | stannous chloride | water | sodium chloride | stannic chloride | tin(IV) sulfide IUPAC name | hydrogen chloride | disodium sulfite | dichlorotin | water | sodium chloride | tetrachlorostannane | tin(+4) cation disulfide

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