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HCl + Sb2S5 = S + H2S + SbCl3

Input interpretation

HCl hydrogen chloride + Sb_2S_5 antimony(V) sulfide ⟶ S mixed sulfur + H_2S hydrogen sulfide + SbCl_3 antimony(III) chloride
HCl hydrogen chloride + Sb_2S_5 antimony(V) sulfide ⟶ S mixed sulfur + H_2S hydrogen sulfide + SbCl_3 antimony(III) chloride

Balanced equation

Balance the chemical equation algebraically: HCl + Sb_2S_5 ⟶ S + H_2S + SbCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Sb_2S_5 ⟶ c_3 S + c_4 H_2S + c_5 SbCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, S and Sb: Cl: | c_1 = 3 c_5 H: | c_1 = 2 c_4 S: | 5 c_2 = c_3 + c_4 Sb: | 2 c_2 = 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 = 6 c_2 = 1 c_3 = 2 c_4 = 3 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + Sb_2S_5 ⟶ 2 S + 3 H_2S + 2 SbCl_3
Balance the chemical equation algebraically: HCl + Sb_2S_5 ⟶ S + H_2S + SbCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Sb_2S_5 ⟶ c_3 S + c_4 H_2S + c_5 SbCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, S and Sb: Cl: | c_1 = 3 c_5 H: | c_1 = 2 c_4 S: | 5 c_2 = c_3 + c_4 Sb: | 2 c_2 = 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 = 6 c_2 = 1 c_3 = 2 c_4 = 3 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + Sb_2S_5 ⟶ 2 S + 3 H_2S + 2 SbCl_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

hydrogen chloride + antimony(V) sulfide ⟶ mixed sulfur + hydrogen sulfide + antimony(III) chloride
hydrogen chloride + antimony(V) sulfide ⟶ mixed sulfur + hydrogen sulfide + antimony(III) chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + Sb_2S_5 ⟶ S + H_2S + SbCl_3 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: 6 HCl + Sb_2S_5 ⟶ 2 S + 3 H_2S + 2 SbCl_3 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 | 6 | -6 Sb_2S_5 | 1 | -1 S | 2 | 2 H_2S | 3 | 3 SbCl_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) Sb_2S_5 | 1 | -1 | ([Sb2S5])^(-1) S | 2 | 2 | ([S])^2 H_2S | 3 | 3 | ([H2S])^3 SbCl_3 | 2 | 2 | ([SbCl3])^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 = ([HCl])^(-6) ([Sb2S5])^(-1) ([S])^2 ([H2S])^3 ([SbCl3])^2 = (([S])^2 ([H2S])^3 ([SbCl3])^2)/(([HCl])^6 [Sb2S5])
Construct the equilibrium constant, K, expression for: HCl + Sb_2S_5 ⟶ S + H_2S + SbCl_3 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: 6 HCl + Sb_2S_5 ⟶ 2 S + 3 H_2S + 2 SbCl_3 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 | 6 | -6 Sb_2S_5 | 1 | -1 S | 2 | 2 H_2S | 3 | 3 SbCl_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) Sb_2S_5 | 1 | -1 | ([Sb2S5])^(-1) S | 2 | 2 | ([S])^2 H_2S | 3 | 3 | ([H2S])^3 SbCl_3 | 2 | 2 | ([SbCl3])^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 = ([HCl])^(-6) ([Sb2S5])^(-1) ([S])^2 ([H2S])^3 ([SbCl3])^2 = (([S])^2 ([H2S])^3 ([SbCl3])^2)/(([HCl])^6 [Sb2S5])

Rate of reaction

Construct the rate of reaction expression for: HCl + Sb_2S_5 ⟶ S + H_2S + SbCl_3 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: 6 HCl + Sb_2S_5 ⟶ 2 S + 3 H_2S + 2 SbCl_3 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 | 6 | -6 Sb_2S_5 | 1 | -1 S | 2 | 2 H_2S | 3 | 3 SbCl_3 | 2 | 2 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) Sb_2S_5 | 1 | -1 | -(Δ[Sb2S5])/(Δt) S | 2 | 2 | 1/2 (Δ[S])/(Δt) H_2S | 3 | 3 | 1/3 (Δ[H2S])/(Δt) SbCl_3 | 2 | 2 | 1/2 (Δ[SbCl3])/(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 = -1/6 (Δ[HCl])/(Δt) = -(Δ[Sb2S5])/(Δt) = 1/2 (Δ[S])/(Δt) = 1/3 (Δ[H2S])/(Δt) = 1/2 (Δ[SbCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + Sb_2S_5 ⟶ S + H_2S + SbCl_3 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: 6 HCl + Sb_2S_5 ⟶ 2 S + 3 H_2S + 2 SbCl_3 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 | 6 | -6 Sb_2S_5 | 1 | -1 S | 2 | 2 H_2S | 3 | 3 SbCl_3 | 2 | 2 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) Sb_2S_5 | 1 | -1 | -(Δ[Sb2S5])/(Δt) S | 2 | 2 | 1/2 (Δ[S])/(Δt) H_2S | 3 | 3 | 1/3 (Δ[H2S])/(Δt) SbCl_3 | 2 | 2 | 1/2 (Δ[SbCl3])/(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 = -1/6 (Δ[HCl])/(Δt) = -(Δ[Sb2S5])/(Δt) = 1/2 (Δ[S])/(Δt) = 1/3 (Δ[H2S])/(Δt) = 1/2 (Δ[SbCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | antimony(V) sulfide | mixed sulfur | hydrogen sulfide | antimony(III) chloride formula | HCl | Sb_2S_5 | S | H_2S | SbCl_3 Hill formula | ClH | S_5Sb_2 | S | H_2S | Cl_3Sb name | hydrogen chloride | antimony(V) sulfide | mixed sulfur | hydrogen sulfide | antimony(III) chloride IUPAC name | hydrogen chloride | | sulfur | hydrogen sulfide | trichlorostibane
| hydrogen chloride | antimony(V) sulfide | mixed sulfur | hydrogen sulfide | antimony(III) chloride formula | HCl | Sb_2S_5 | S | H_2S | SbCl_3 Hill formula | ClH | S_5Sb_2 | S | H_2S | Cl_3Sb name | hydrogen chloride | antimony(V) sulfide | mixed sulfur | hydrogen sulfide | antimony(III) chloride IUPAC name | hydrogen chloride | | sulfur | hydrogen sulfide | trichlorostibane

Substance properties

| hydrogen chloride | antimony(V) sulfide | mixed sulfur | hydrogen sulfide | antimony(III) chloride molar mass | 36.46 g/mol | 403.8 g/mol | 32.06 g/mol | 34.08 g/mol | 228.1 g/mol phase | gas (at STP) | | solid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 112.8 °C | -85 °C | 73.4 °C boiling point | -85 °C | | 444.7 °C | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 2.07 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | solubility in water | miscible | | | | dynamic viscosity | | | | 1.239×10^-5 Pa s (at 25 °C) |
| hydrogen chloride | antimony(V) sulfide | mixed sulfur | hydrogen sulfide | antimony(III) chloride molar mass | 36.46 g/mol | 403.8 g/mol | 32.06 g/mol | 34.08 g/mol | 228.1 g/mol phase | gas (at STP) | | solid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 112.8 °C | -85 °C | 73.4 °C boiling point | -85 °C | | 444.7 °C | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 2.07 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | solubility in water | miscible | | | | dynamic viscosity | | | | 1.239×10^-5 Pa s (at 25 °C) |

Units

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