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K2S + Pb(CH3COO)2 = PbS + CH3COOK

Input interpretation

K2S + Pb(CH_3CO_2)_2 lead(II) acetate ⟶ PbS lead sulfide + CH_3COOK potassium acetate
K2S + Pb(CH_3CO_2)_2 lead(II) acetate ⟶ PbS lead sulfide + CH_3COOK potassium acetate

Balanced equation

Balance the chemical equation algebraically: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + CH_3COOK Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K2S + c_2 Pb(CH_3CO_2)_2 ⟶ c_3 PbS + c_4 CH_3COOK Set the number of atoms in the reactants equal to the number of atoms in the products for K, S, C, H, O and Pb: K: | 2 c_1 = c_4 S: | c_1 = c_3 C: | 4 c_2 = 2 c_4 H: | 6 c_2 = 3 c_4 O: | 4 c_2 = 2 c_4 Pb: | c_2 = c_3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K2S + Pb(CH_3CO_2)_2 ⟶ PbS + 2 CH_3COOK
Balance the chemical equation algebraically: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + CH_3COOK Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K2S + c_2 Pb(CH_3CO_2)_2 ⟶ c_3 PbS + c_4 CH_3COOK Set the number of atoms in the reactants equal to the number of atoms in the products for K, S, C, H, O and Pb: K: | 2 c_1 = c_4 S: | c_1 = c_3 C: | 4 c_2 = 2 c_4 H: | 6 c_2 = 3 c_4 O: | 4 c_2 = 2 c_4 Pb: | c_2 = c_3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K2S + Pb(CH_3CO_2)_2 ⟶ PbS + 2 CH_3COOK

Structures

K2S + ⟶ +
K2S + ⟶ +

Names

K2S + lead(II) acetate ⟶ lead sulfide + potassium acetate
K2S + lead(II) acetate ⟶ lead sulfide + potassium acetate

Equilibrium constant

Construct the equilibrium constant, K, expression for: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + CH_3COOK 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: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + 2 CH_3COOK 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 K2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 PbS | 1 | 1 CH_3COOK | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K2S | 1 | -1 | ([K2S])^(-1) Pb(CH_3CO_2)_2 | 1 | -1 | ([Pb(CH3CO2)2])^(-1) PbS | 1 | 1 | [PbS] CH_3COOK | 2 | 2 | ([CH3COOK])^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 = ([K2S])^(-1) ([Pb(CH3CO2)2])^(-1) [PbS] ([CH3COOK])^2 = ([PbS] ([CH3COOK])^2)/([K2S] [Pb(CH3CO2)2])
Construct the equilibrium constant, K, expression for: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + CH_3COOK 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: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + 2 CH_3COOK 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 K2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 PbS | 1 | 1 CH_3COOK | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K2S | 1 | -1 | ([K2S])^(-1) Pb(CH_3CO_2)_2 | 1 | -1 | ([Pb(CH3CO2)2])^(-1) PbS | 1 | 1 | [PbS] CH_3COOK | 2 | 2 | ([CH3COOK])^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 = ([K2S])^(-1) ([Pb(CH3CO2)2])^(-1) [PbS] ([CH3COOK])^2 = ([PbS] ([CH3COOK])^2)/([K2S] [Pb(CH3CO2)2])

Rate of reaction

Construct the rate of reaction expression for: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + CH_3COOK 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: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + 2 CH_3COOK 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 K2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 PbS | 1 | 1 CH_3COOK | 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 K2S | 1 | -1 | -(Δ[K2S])/(Δt) Pb(CH_3CO_2)_2 | 1 | -1 | -(Δ[Pb(CH3CO2)2])/(Δt) PbS | 1 | 1 | (Δ[PbS])/(Δt) CH_3COOK | 2 | 2 | 1/2 (Δ[CH3COOK])/(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 = -(Δ[K2S])/(Δt) = -(Δ[Pb(CH3CO2)2])/(Δt) = (Δ[PbS])/(Δt) = 1/2 (Δ[CH3COOK])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + CH_3COOK 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: K2S + Pb(CH_3CO_2)_2 ⟶ PbS + 2 CH_3COOK 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 K2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 PbS | 1 | 1 CH_3COOK | 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 K2S | 1 | -1 | -(Δ[K2S])/(Δt) Pb(CH_3CO_2)_2 | 1 | -1 | -(Δ[Pb(CH3CO2)2])/(Δt) PbS | 1 | 1 | (Δ[PbS])/(Δt) CH_3COOK | 2 | 2 | 1/2 (Δ[CH3COOK])/(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 = -(Δ[K2S])/(Δt) = -(Δ[Pb(CH3CO2)2])/(Δt) = (Δ[PbS])/(Δt) = 1/2 (Δ[CH3COOK])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| K2S | lead(II) acetate | lead sulfide | potassium acetate formula | K2S | Pb(CH_3CO_2)_2 | PbS | CH_3COOK Hill formula | K2S | C_4H_6O_4Pb | PbS | C_2H_3KO_2 name | | lead(II) acetate | lead sulfide | potassium acetate IUPAC name | | lead(2+) diacetate | | potassium acetate
| K2S | lead(II) acetate | lead sulfide | potassium acetate formula | K2S | Pb(CH_3CO_2)_2 | PbS | CH_3COOK Hill formula | K2S | C_4H_6O_4Pb | PbS | C_2H_3KO_2 name | | lead(II) acetate | lead sulfide | potassium acetate IUPAC name | | lead(2+) diacetate | | potassium acetate

Substance properties

| K2S | lead(II) acetate | lead sulfide | potassium acetate molar mass | 110.26 g/mol | 325.3 g/mol | 239.3 g/mol | 98.142 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 280 °C | 1114 °C | 304 °C boiling point | | | 1344 °C | density | | 3.25 g/cm^3 | 7.5 g/cm^3 | 1.57 g/cm^3 solubility in water | | | insoluble | surface tension | | | | 0.0256 N/m
| K2S | lead(II) acetate | lead sulfide | potassium acetate molar mass | 110.26 g/mol | 325.3 g/mol | 239.3 g/mol | 98.142 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 280 °C | 1114 °C | 304 °C boiling point | | | 1344 °C | density | | 3.25 g/cm^3 | 7.5 g/cm^3 | 1.57 g/cm^3 solubility in water | | | insoluble | surface tension | | | | 0.0256 N/m

Units

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