Search

HCl + Sb2S3 = H2S + H3SbCl6

Input interpretation

HCl hydrogen chloride + Sb_2S_3 antimony(III) sulfide ⟶ H_2S hydrogen sulfide + H3SbCl6
HCl hydrogen chloride + Sb_2S_3 antimony(III) sulfide ⟶ H_2S hydrogen sulfide + H3SbCl6

Balanced equation

Balance the chemical equation algebraically: HCl + Sb_2S_3 ⟶ H_2S + H3SbCl6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Sb_2S_3 ⟶ c_3 H_2S + c_4 H3SbCl6 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 = 6 c_4 H: | c_1 = 2 c_3 + 3 c_4 S: | 3 c_2 = c_3 Sb: | 2 c_2 = c_4 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 = 12 c_2 = 1 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HCl + Sb_2S_3 ⟶ 3 H_2S + 2 H3SbCl6
Balance the chemical equation algebraically: HCl + Sb_2S_3 ⟶ H_2S + H3SbCl6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Sb_2S_3 ⟶ c_3 H_2S + c_4 H3SbCl6 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 = 6 c_4 H: | c_1 = 2 c_3 + 3 c_4 S: | 3 c_2 = c_3 Sb: | 2 c_2 = c_4 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 = 12 c_2 = 1 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HCl + Sb_2S_3 ⟶ 3 H_2S + 2 H3SbCl6

Structures

+ ⟶ + H3SbCl6
+ ⟶ + H3SbCl6

Names

hydrogen chloride + antimony(III) sulfide ⟶ hydrogen sulfide + H3SbCl6
hydrogen chloride + antimony(III) sulfide ⟶ hydrogen sulfide + H3SbCl6

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + Sb_2S_3 ⟶ H_2S + H3SbCl6 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 + Sb_2S_3 ⟶ 3 H_2S + 2 H3SbCl6 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 Sb_2S_3 | 1 | -1 H_2S | 3 | 3 H3SbCl6 | 2 | 2 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) Sb_2S_3 | 1 | -1 | ([Sb2S3])^(-1) H_2S | 3 | 3 | ([H2S])^3 H3SbCl6 | 2 | 2 | ([H3SbCl6])^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])^(-12) ([Sb2S3])^(-1) ([H2S])^3 ([H3SbCl6])^2 = (([H2S])^3 ([H3SbCl6])^2)/(([HCl])^12 [Sb2S3])
Construct the equilibrium constant, K, expression for: HCl + Sb_2S_3 ⟶ H_2S + H3SbCl6 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 + Sb_2S_3 ⟶ 3 H_2S + 2 H3SbCl6 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 Sb_2S_3 | 1 | -1 H_2S | 3 | 3 H3SbCl6 | 2 | 2 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) Sb_2S_3 | 1 | -1 | ([Sb2S3])^(-1) H_2S | 3 | 3 | ([H2S])^3 H3SbCl6 | 2 | 2 | ([H3SbCl6])^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])^(-12) ([Sb2S3])^(-1) ([H2S])^3 ([H3SbCl6])^2 = (([H2S])^3 ([H3SbCl6])^2)/(([HCl])^12 [Sb2S3])

Rate of reaction

Construct the rate of reaction expression for: HCl + Sb_2S_3 ⟶ H_2S + H3SbCl6 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 + Sb_2S_3 ⟶ 3 H_2S + 2 H3SbCl6 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 Sb_2S_3 | 1 | -1 H_2S | 3 | 3 H3SbCl6 | 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 | 12 | -12 | -1/12 (Δ[HCl])/(Δt) Sb_2S_3 | 1 | -1 | -(Δ[Sb2S3])/(Δt) H_2S | 3 | 3 | 1/3 (Δ[H2S])/(Δt) H3SbCl6 | 2 | 2 | 1/2 (Δ[H3SbCl6])/(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) = -(Δ[Sb2S3])/(Δt) = 1/3 (Δ[H2S])/(Δt) = 1/2 (Δ[H3SbCl6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + Sb_2S_3 ⟶ H_2S + H3SbCl6 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 + Sb_2S_3 ⟶ 3 H_2S + 2 H3SbCl6 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 Sb_2S_3 | 1 | -1 H_2S | 3 | 3 H3SbCl6 | 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 | 12 | -12 | -1/12 (Δ[HCl])/(Δt) Sb_2S_3 | 1 | -1 | -(Δ[Sb2S3])/(Δt) H_2S | 3 | 3 | 1/3 (Δ[H2S])/(Δt) H3SbCl6 | 2 | 2 | 1/2 (Δ[H3SbCl6])/(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) = -(Δ[Sb2S3])/(Δt) = 1/3 (Δ[H2S])/(Δt) = 1/2 (Δ[H3SbCl6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | antimony(III) sulfide | hydrogen sulfide | H3SbCl6 formula | HCl | Sb_2S_3 | H_2S | H3SbCl6 Hill formula | ClH | S_3Sb_2 | H_2S | H3Cl6Sb name | hydrogen chloride | antimony(III) sulfide | hydrogen sulfide | IUPAC name | hydrogen chloride | thioxo-(thioxostibanylthio)stibane | hydrogen sulfide |
| hydrogen chloride | antimony(III) sulfide | hydrogen sulfide | H3SbCl6 formula | HCl | Sb_2S_3 | H_2S | H3SbCl6 Hill formula | ClH | S_3Sb_2 | H_2S | H3Cl6Sb name | hydrogen chloride | antimony(III) sulfide | hydrogen sulfide | IUPAC name | hydrogen chloride | thioxo-(thioxostibanylthio)stibane | hydrogen sulfide |

Substance properties

| hydrogen chloride | antimony(III) sulfide | hydrogen sulfide | H3SbCl6 molar mass | 36.46 g/mol | 339.7 g/mol | 34.08 g/mol | 337.5 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | melting point | -114.17 °C | 550 °C | -85 °C | boiling point | -85 °C | | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | 4.64 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(III) sulfide | hydrogen sulfide | H3SbCl6 molar mass | 36.46 g/mol | 339.7 g/mol | 34.08 g/mol | 337.5 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | melting point | -114.17 °C | 550 °C | -85 °C | boiling point | -85 °C | | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | 4.64 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

Random Queries

prices of semiconductors
name of silver cyclohexanebutyrate vs mercuric sulfate
alternate names of barium chloride vs sodium hypophosphite hydrate
boiling point of manganese
formula of antimony pentafluoride
freezing point of antimony(III) sulfide
InChI identifier of gallium selenide
formula zinc oxide
name of nickel(II) chloride vs sodium permanganate
CAS number of zinc vs boron