Search

FeCl3 + K2S = S + KCl + FeS

Input interpretation

FeCl_3 iron(III) chloride + K2S ⟶ S mixed sulfur + KCl potassium chloride + FeS ferrous sulfide
FeCl_3 iron(III) chloride + K2S ⟶ S mixed sulfur + KCl potassium chloride + FeS ferrous sulfide

Balanced equation

Balance the chemical equation algebraically: FeCl_3 + K2S ⟶ S + KCl + FeS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeCl_3 + c_2 K2S ⟶ c_3 S + c_4 KCl + c_5 FeS Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Fe, K and S: Cl: | 3 c_1 = c_4 Fe: | c_1 = c_5 K: | 2 c_2 = c_4 S: | c_2 = c_3 + 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 1 c_4 = 6 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 FeCl_3 + 3 K2S ⟶ S + 6 KCl + 2 FeS
Balance the chemical equation algebraically: FeCl_3 + K2S ⟶ S + KCl + FeS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeCl_3 + c_2 K2S ⟶ c_3 S + c_4 KCl + c_5 FeS Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Fe, K and S: Cl: | 3 c_1 = c_4 Fe: | c_1 = c_5 K: | 2 c_2 = c_4 S: | c_2 = c_3 + 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 1 c_4 = 6 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 FeCl_3 + 3 K2S ⟶ S + 6 KCl + 2 FeS

Structures

+ K2S ⟶ + +
+ K2S ⟶ + +

Names

iron(III) chloride + K2S ⟶ mixed sulfur + potassium chloride + ferrous sulfide
iron(III) chloride + K2S ⟶ mixed sulfur + potassium chloride + ferrous sulfide

Equilibrium constant

Construct the equilibrium constant, K, expression for: FeCl_3 + K2S ⟶ S + KCl + FeS 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 FeCl_3 + 3 K2S ⟶ S + 6 KCl + 2 FeS 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 FeCl_3 | 2 | -2 K2S | 3 | -3 S | 1 | 1 KCl | 6 | 6 FeS | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeCl_3 | 2 | -2 | ([FeCl3])^(-2) K2S | 3 | -3 | ([K2S])^(-3) S | 1 | 1 | [S] KCl | 6 | 6 | ([KCl])^6 FeS | 2 | 2 | ([FeS])^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 = ([FeCl3])^(-2) ([K2S])^(-3) [S] ([KCl])^6 ([FeS])^2 = ([S] ([KCl])^6 ([FeS])^2)/(([FeCl3])^2 ([K2S])^3)
Construct the equilibrium constant, K, expression for: FeCl_3 + K2S ⟶ S + KCl + FeS 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 FeCl_3 + 3 K2S ⟶ S + 6 KCl + 2 FeS 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 FeCl_3 | 2 | -2 K2S | 3 | -3 S | 1 | 1 KCl | 6 | 6 FeS | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeCl_3 | 2 | -2 | ([FeCl3])^(-2) K2S | 3 | -3 | ([K2S])^(-3) S | 1 | 1 | [S] KCl | 6 | 6 | ([KCl])^6 FeS | 2 | 2 | ([FeS])^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 = ([FeCl3])^(-2) ([K2S])^(-3) [S] ([KCl])^6 ([FeS])^2 = ([S] ([KCl])^6 ([FeS])^2)/(([FeCl3])^2 ([K2S])^3)

Rate of reaction

Construct the rate of reaction expression for: FeCl_3 + K2S ⟶ S + KCl + FeS 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 FeCl_3 + 3 K2S ⟶ S + 6 KCl + 2 FeS 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 FeCl_3 | 2 | -2 K2S | 3 | -3 S | 1 | 1 KCl | 6 | 6 FeS | 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 FeCl_3 | 2 | -2 | -1/2 (Δ[FeCl3])/(Δt) K2S | 3 | -3 | -1/3 (Δ[K2S])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) FeS | 2 | 2 | 1/2 (Δ[FeS])/(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[FeCl3])/(Δt) = -1/3 (Δ[K2S])/(Δt) = (Δ[S])/(Δt) = 1/6 (Δ[KCl])/(Δt) = 1/2 (Δ[FeS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: FeCl_3 + K2S ⟶ S + KCl + FeS 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 FeCl_3 + 3 K2S ⟶ S + 6 KCl + 2 FeS 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 FeCl_3 | 2 | -2 K2S | 3 | -3 S | 1 | 1 KCl | 6 | 6 FeS | 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 FeCl_3 | 2 | -2 | -1/2 (Δ[FeCl3])/(Δt) K2S | 3 | -3 | -1/3 (Δ[K2S])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) FeS | 2 | 2 | 1/2 (Δ[FeS])/(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[FeCl3])/(Δt) = -1/3 (Δ[K2S])/(Δt) = (Δ[S])/(Δt) = 1/6 (Δ[KCl])/(Δt) = 1/2 (Δ[FeS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iron(III) chloride | K2S | mixed sulfur | potassium chloride | ferrous sulfide formula | FeCl_3 | K2S | S | KCl | FeS Hill formula | Cl_3Fe | K2S | S | ClK | FeS name | iron(III) chloride | | mixed sulfur | potassium chloride | ferrous sulfide IUPAC name | trichloroiron | | sulfur | potassium chloride |
| iron(III) chloride | K2S | mixed sulfur | potassium chloride | ferrous sulfide formula | FeCl_3 | K2S | S | KCl | FeS Hill formula | Cl_3Fe | K2S | S | ClK | FeS name | iron(III) chloride | | mixed sulfur | potassium chloride | ferrous sulfide IUPAC name | trichloroiron | | sulfur | potassium chloride |

Substance properties

| iron(III) chloride | K2S | mixed sulfur | potassium chloride | ferrous sulfide molar mass | 162.2 g/mol | 110.26 g/mol | 32.06 g/mol | 74.55 g/mol | 87.9 g/mol phase | solid (at STP) | | solid (at STP) | solid (at STP) | solid (at STP) melting point | 304 °C | | 112.8 °C | 770 °C | 1195 °C boiling point | | | 444.7 °C | 1420 °C | density | | | 2.07 g/cm^3 | 1.98 g/cm^3 | 4.84 g/cm^3 solubility in water | | | | soluble | insoluble dynamic viscosity | | | | | 0.00343 Pa s (at 1250 °C) odor | | | | odorless |
| iron(III) chloride | K2S | mixed sulfur | potassium chloride | ferrous sulfide molar mass | 162.2 g/mol | 110.26 g/mol | 32.06 g/mol | 74.55 g/mol | 87.9 g/mol phase | solid (at STP) | | solid (at STP) | solid (at STP) | solid (at STP) melting point | 304 °C | | 112.8 °C | 770 °C | 1195 °C boiling point | | | 444.7 °C | 1420 °C | density | | | 2.07 g/cm^3 | 1.98 g/cm^3 | 4.84 g/cm^3 solubility in water | | | | soluble | insoluble dynamic viscosity | | | | | 0.00343 Pa s (at 1250 °C) odor | | | | odorless |

Units

Random Queries

solubility iron
ion electron configuration of iodine(III) cation
formula of potassium phthalimide
InChI identifier of 4-bromophenyl trifluoromethyl sulfide
edge types of silicon nitride
color of silver vs palladium
density of sodium phosphomolybdate hydrate
chemical types of hypochlorous acid vs chlorocyclopentane
HNO3 + FeSO4 = H2O + H2SO4 + NO + Fe(NO3)3
chemical types of iodine bromide vs iron