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H2O2 + PbS = H2O + SO2 + Pb(OH)2

Input interpretation

H_2O_2 hydrogen peroxide + PbS lead sulfide ⟶ H_2O water + SO_2 sulfur dioxide + Pb(OH)_2 lead(II) hydroxide
H_2O_2 hydrogen peroxide + PbS lead sulfide ⟶ H_2O water + SO_2 sulfur dioxide + Pb(OH)_2 lead(II) hydroxide

Balanced equation

Balance the chemical equation algebraically: H_2O_2 + PbS ⟶ H_2O + SO_2 + Pb(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 PbS ⟶ c_3 H_2O + c_4 SO_2 + c_5 Pb(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Pb and S: H: | 2 c_1 = 2 c_3 + 2 c_5 O: | 2 c_1 = c_3 + 2 c_4 + 2 c_5 Pb: | c_2 = c_5 S: | 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 = 3 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O_2 + PbS ⟶ 2 H_2O + SO_2 + Pb(OH)_2
Balance the chemical equation algebraically: H_2O_2 + PbS ⟶ H_2O + SO_2 + Pb(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 PbS ⟶ c_3 H_2O + c_4 SO_2 + c_5 Pb(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Pb and S: H: | 2 c_1 = 2 c_3 + 2 c_5 O: | 2 c_1 = c_3 + 2 c_4 + 2 c_5 Pb: | c_2 = c_5 S: | 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 = 3 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O_2 + PbS ⟶ 2 H_2O + SO_2 + Pb(OH)_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

hydrogen peroxide + lead sulfide ⟶ water + sulfur dioxide + lead(II) hydroxide
hydrogen peroxide + lead sulfide ⟶ water + sulfur dioxide + lead(II) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O_2 + PbS ⟶ H_2O + SO_2 + Pb(OH)_2 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: 3 H_2O_2 + PbS ⟶ 2 H_2O + SO_2 + Pb(OH)_2 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_2O_2 | 3 | -3 PbS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O_2 | 3 | -3 | ([H2O2])^(-3) PbS | 1 | -1 | ([PbS])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] Pb(OH)_2 | 1 | 1 | [Pb(OH)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 = ([H2O2])^(-3) ([PbS])^(-1) ([H2O])^2 [SO2] [Pb(OH)2] = (([H2O])^2 [SO2] [Pb(OH)2])/(([H2O2])^3 [PbS])
Construct the equilibrium constant, K, expression for: H_2O_2 + PbS ⟶ H_2O + SO_2 + Pb(OH)_2 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: 3 H_2O_2 + PbS ⟶ 2 H_2O + SO_2 + Pb(OH)_2 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_2O_2 | 3 | -3 PbS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O_2 | 3 | -3 | ([H2O2])^(-3) PbS | 1 | -1 | ([PbS])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] Pb(OH)_2 | 1 | 1 | [Pb(OH)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 = ([H2O2])^(-3) ([PbS])^(-1) ([H2O])^2 [SO2] [Pb(OH)2] = (([H2O])^2 [SO2] [Pb(OH)2])/(([H2O2])^3 [PbS])

Rate of reaction

Construct the rate of reaction expression for: H_2O_2 + PbS ⟶ H_2O + SO_2 + Pb(OH)_2 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: 3 H_2O_2 + PbS ⟶ 2 H_2O + SO_2 + Pb(OH)_2 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_2O_2 | 3 | -3 PbS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(OH)_2 | 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_2O_2 | 3 | -3 | -1/3 (Δ[H2O2])/(Δt) PbS | 1 | -1 | -(Δ[PbS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) Pb(OH)_2 | 1 | 1 | (Δ[Pb(OH)2])/(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 = -1/3 (Δ[H2O2])/(Δt) = -(Δ[PbS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[Pb(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O_2 + PbS ⟶ H_2O + SO_2 + Pb(OH)_2 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: 3 H_2O_2 + PbS ⟶ 2 H_2O + SO_2 + Pb(OH)_2 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_2O_2 | 3 | -3 PbS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(OH)_2 | 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_2O_2 | 3 | -3 | -1/3 (Δ[H2O2])/(Δt) PbS | 1 | -1 | -(Δ[PbS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) Pb(OH)_2 | 1 | 1 | (Δ[Pb(OH)2])/(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 = -1/3 (Δ[H2O2])/(Δt) = -(Δ[PbS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[Pb(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen peroxide | lead sulfide | water | sulfur dioxide | lead(II) hydroxide formula | H_2O_2 | PbS | H_2O | SO_2 | Pb(OH)_2 Hill formula | H_2O_2 | PbS | H_2O | O_2S | H_2O_2Pb name | hydrogen peroxide | lead sulfide | water | sulfur dioxide | lead(II) hydroxide IUPAC name | hydrogen peroxide | | water | sulfur dioxide | plumbous dihydroxide
| hydrogen peroxide | lead sulfide | water | sulfur dioxide | lead(II) hydroxide formula | H_2O_2 | PbS | H_2O | SO_2 | Pb(OH)_2 Hill formula | H_2O_2 | PbS | H_2O | O_2S | H_2O_2Pb name | hydrogen peroxide | lead sulfide | water | sulfur dioxide | lead(II) hydroxide IUPAC name | hydrogen peroxide | | water | sulfur dioxide | plumbous dihydroxide

Substance properties

| hydrogen peroxide | lead sulfide | water | sulfur dioxide | lead(II) hydroxide molar mass | 34.014 g/mol | 239.3 g/mol | 18.015 g/mol | 64.06 g/mol | 241.2 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | -0.43 °C | 1114 °C | 0 °C | -73 °C | boiling point | 150.2 °C | 1344 °C | 99.9839 °C | -10 °C | density | 1.44 g/cm^3 | 7.5 g/cm^3 | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | solubility in water | miscible | insoluble | | | surface tension | 0.0804 N/m | | 0.0728 N/m | 0.02859 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | odor | | | odorless | |
| hydrogen peroxide | lead sulfide | water | sulfur dioxide | lead(II) hydroxide molar mass | 34.014 g/mol | 239.3 g/mol | 18.015 g/mol | 64.06 g/mol | 241.2 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | -0.43 °C | 1114 °C | 0 °C | -73 °C | boiling point | 150.2 °C | 1344 °C | 99.9839 °C | -10 °C | density | 1.44 g/cm^3 | 7.5 g/cm^3 | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | solubility in water | miscible | insoluble | | | surface tension | 0.0804 N/m | | 0.0728 N/m | 0.02859 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | odor | | | odorless | |

Units

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