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H2S + (CH3COO)2Pb = CH3COOH + PbS

Input interpretation

H_2S hydrogen sulfide + Pb(CH_3CO_2)_2 lead(II) acetate ⟶ CH_3CO_2H acetic acid + PbS lead sulfide
H_2S hydrogen sulfide + Pb(CH_3CO_2)_2 lead(II) acetate ⟶ CH_3CO_2H acetic acid + PbS lead sulfide

Balanced equation

Balance the chemical equation algebraically: H_2S + Pb(CH_3CO_2)_2 ⟶ CH_3CO_2H + PbS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 Pb(CH_3CO_2)_2 ⟶ c_3 CH_3CO_2H + c_4 PbS Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, C, O and Pb: H: | 2 c_1 + 6 c_2 = 4 c_3 S: | c_1 = c_4 C: | 4 c_2 = 2 c_3 O: | 4 c_2 = 2 c_3 Pb: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2S + Pb(CH_3CO_2)_2 ⟶ 2 CH_3CO_2H + PbS
Balance the chemical equation algebraically: H_2S + Pb(CH_3CO_2)_2 ⟶ CH_3CO_2H + PbS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 Pb(CH_3CO_2)_2 ⟶ c_3 CH_3CO_2H + c_4 PbS Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, C, O and Pb: H: | 2 c_1 + 6 c_2 = 4 c_3 S: | c_1 = c_4 C: | 4 c_2 = 2 c_3 O: | 4 c_2 = 2 c_3 Pb: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2S + Pb(CH_3CO_2)_2 ⟶ 2 CH_3CO_2H + PbS

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen sulfide + lead(II) acetate ⟶ acetic acid + lead sulfide
hydrogen sulfide + lead(II) acetate ⟶ acetic acid + lead sulfide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2S + Pb(CH_3CO_2)_2 ⟶ CH_3CO_2H + PbS 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: H_2S + Pb(CH_3CO_2)_2 ⟶ 2 CH_3CO_2H + PbS 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 H_2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 CH_3CO_2H | 2 | 2 PbS | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 1 | -1 | ([H2S])^(-1) Pb(CH_3CO_2)_2 | 1 | -1 | ([Pb(CH3CO2)2])^(-1) CH_3CO_2H | 2 | 2 | ([CH3CO2H])^2 PbS | 1 | 1 | [PbS] 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 = ([H2S])^(-1) ([Pb(CH3CO2)2])^(-1) ([CH3CO2H])^2 [PbS] = (([CH3CO2H])^2 [PbS])/([H2S] [Pb(CH3CO2)2])
Construct the equilibrium constant, K, expression for: H_2S + Pb(CH_3CO_2)_2 ⟶ CH_3CO_2H + PbS 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: H_2S + Pb(CH_3CO_2)_2 ⟶ 2 CH_3CO_2H + PbS 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 H_2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 CH_3CO_2H | 2 | 2 PbS | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 1 | -1 | ([H2S])^(-1) Pb(CH_3CO_2)_2 | 1 | -1 | ([Pb(CH3CO2)2])^(-1) CH_3CO_2H | 2 | 2 | ([CH3CO2H])^2 PbS | 1 | 1 | [PbS] 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 = ([H2S])^(-1) ([Pb(CH3CO2)2])^(-1) ([CH3CO2H])^2 [PbS] = (([CH3CO2H])^2 [PbS])/([H2S] [Pb(CH3CO2)2])

Rate of reaction

Construct the rate of reaction expression for: H_2S + Pb(CH_3CO_2)_2 ⟶ CH_3CO_2H + PbS 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: H_2S + Pb(CH_3CO_2)_2 ⟶ 2 CH_3CO_2H + PbS 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 H_2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 CH_3CO_2H | 2 | 2 PbS | 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 H_2S | 1 | -1 | -(Δ[H2S])/(Δt) Pb(CH_3CO_2)_2 | 1 | -1 | -(Δ[Pb(CH3CO2)2])/(Δt) CH_3CO_2H | 2 | 2 | 1/2 (Δ[CH3CO2H])/(Δt) PbS | 1 | 1 | (Δ[PbS])/(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[H2S])/(Δt) = -(Δ[Pb(CH3CO2)2])/(Δt) = 1/2 (Δ[CH3CO2H])/(Δt) = (Δ[PbS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2S + Pb(CH_3CO_2)_2 ⟶ CH_3CO_2H + PbS 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: H_2S + Pb(CH_3CO_2)_2 ⟶ 2 CH_3CO_2H + PbS 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 H_2S | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 CH_3CO_2H | 2 | 2 PbS | 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 H_2S | 1 | -1 | -(Δ[H2S])/(Δt) Pb(CH_3CO_2)_2 | 1 | -1 | -(Δ[Pb(CH3CO2)2])/(Δt) CH_3CO_2H | 2 | 2 | 1/2 (Δ[CH3CO2H])/(Δt) PbS | 1 | 1 | (Δ[PbS])/(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[H2S])/(Δt) = -(Δ[Pb(CH3CO2)2])/(Δt) = 1/2 (Δ[CH3CO2H])/(Δt) = (Δ[PbS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen sulfide | lead(II) acetate | acetic acid | lead sulfide formula | H_2S | Pb(CH_3CO_2)_2 | CH_3CO_2H | PbS Hill formula | H_2S | C_4H_6O_4Pb | C_2H_4O_2 | PbS name | hydrogen sulfide | lead(II) acetate | acetic acid | lead sulfide IUPAC name | hydrogen sulfide | lead(2+) diacetate | acetic acid |
| hydrogen sulfide | lead(II) acetate | acetic acid | lead sulfide formula | H_2S | Pb(CH_3CO_2)_2 | CH_3CO_2H | PbS Hill formula | H_2S | C_4H_6O_4Pb | C_2H_4O_2 | PbS name | hydrogen sulfide | lead(II) acetate | acetic acid | lead sulfide IUPAC name | hydrogen sulfide | lead(2+) diacetate | acetic acid |

Substance properties

| hydrogen sulfide | lead(II) acetate | acetic acid | lead sulfide molar mass | 34.08 g/mol | 325.3 g/mol | 60.052 g/mol | 239.3 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -85 °C | 280 °C | 16.2 °C | 1114 °C boiling point | -60 °C | | 117.5 °C | 1344 °C density | 0.001393 g/cm^3 (at 25 °C) | 3.25 g/cm^3 | 1.049 g/cm^3 | 7.5 g/cm^3 solubility in water | | | miscible | insoluble surface tension | | | 0.0288 N/m | dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 0.001056 Pa s (at 25 °C) | odor | | | vinegar-like |
| hydrogen sulfide | lead(II) acetate | acetic acid | lead sulfide molar mass | 34.08 g/mol | 325.3 g/mol | 60.052 g/mol | 239.3 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -85 °C | 280 °C | 16.2 °C | 1114 °C boiling point | -60 °C | | 117.5 °C | 1344 °C density | 0.001393 g/cm^3 (at 25 °C) | 3.25 g/cm^3 | 1.049 g/cm^3 | 7.5 g/cm^3 solubility in water | | | miscible | insoluble surface tension | | | 0.0288 N/m | dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 0.001056 Pa s (at 25 °C) | odor | | | vinegar-like |

Units

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