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HCl + Pb3O4 = H2O + Cl2 + PbO

Input interpretation

HCl hydrogen chloride + Pb_3O_4 lead(II, IV) oxide ⟶ H_2O water + Cl_2 chlorine + PbO lead monoxide
HCl hydrogen chloride + Pb_3O_4 lead(II, IV) oxide ⟶ H_2O water + Cl_2 chlorine + PbO lead monoxide

Balanced equation

Balance the chemical equation algebraically: HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + PbO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Pb_3O_4 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 PbO Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O and Pb: Cl: | c_1 = 2 c_4 H: | c_1 = 2 c_3 O: | 4 c_2 = c_3 + c_5 Pb: | 3 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + 3 PbO
Balance the chemical equation algebraically: HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + PbO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Pb_3O_4 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 PbO Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O and Pb: Cl: | c_1 = 2 c_4 H: | c_1 = 2 c_3 O: | 4 c_2 = c_3 + c_5 Pb: | 3 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + 3 PbO

Structures

+ ⟶ + +
+ ⟶ + +

Names

hydrogen chloride + lead(II, IV) oxide ⟶ water + chlorine + lead monoxide
hydrogen chloride + lead(II, IV) oxide ⟶ water + chlorine + lead monoxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + PbO 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 HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + 3 PbO 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 | 2 | -2 Pb_3O_4 | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 PbO | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) Pb_3O_4 | 1 | -1 | ([Pb3O4])^(-1) H_2O | 1 | 1 | [H2O] Cl_2 | 1 | 1 | [Cl2] PbO | 3 | 3 | ([PbO])^3 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])^(-2) ([Pb3O4])^(-1) [H2O] [Cl2] ([PbO])^3 = ([H2O] [Cl2] ([PbO])^3)/(([HCl])^2 [Pb3O4])
Construct the equilibrium constant, K, expression for: HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + PbO 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 HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + 3 PbO 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 | 2 | -2 Pb_3O_4 | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 PbO | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) Pb_3O_4 | 1 | -1 | ([Pb3O4])^(-1) H_2O | 1 | 1 | [H2O] Cl_2 | 1 | 1 | [Cl2] PbO | 3 | 3 | ([PbO])^3 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])^(-2) ([Pb3O4])^(-1) [H2O] [Cl2] ([PbO])^3 = ([H2O] [Cl2] ([PbO])^3)/(([HCl])^2 [Pb3O4])

Rate of reaction

Construct the rate of reaction expression for: HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + PbO 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 HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + 3 PbO 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 | 2 | -2 Pb_3O_4 | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 PbO | 3 | 3 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) Pb_3O_4 | 1 | -1 | -(Δ[Pb3O4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) PbO | 3 | 3 | 1/3 (Δ[PbO])/(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[HCl])/(Δt) = -(Δ[Pb3O4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = 1/3 (Δ[PbO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + PbO 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 HCl + Pb_3O_4 ⟶ H_2O + Cl_2 + 3 PbO 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 | 2 | -2 Pb_3O_4 | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 PbO | 3 | 3 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) Pb_3O_4 | 1 | -1 | -(Δ[Pb3O4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) PbO | 3 | 3 | 1/3 (Δ[PbO])/(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[HCl])/(Δt) = -(Δ[Pb3O4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = 1/3 (Δ[PbO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | lead(II, IV) oxide | water | chlorine | lead monoxide formula | HCl | Pb_3O_4 | H_2O | Cl_2 | PbO Hill formula | ClH | O_4Pb_3 | H_2O | Cl_2 | OPb name | hydrogen chloride | lead(II, IV) oxide | water | chlorine | lead monoxide IUPAC name | hydrogen chloride | lead tetraoxide | water | molecular chlorine |
| hydrogen chloride | lead(II, IV) oxide | water | chlorine | lead monoxide formula | HCl | Pb_3O_4 | H_2O | Cl_2 | PbO Hill formula | ClH | O_4Pb_3 | H_2O | Cl_2 | OPb name | hydrogen chloride | lead(II, IV) oxide | water | chlorine | lead monoxide IUPAC name | hydrogen chloride | lead tetraoxide | water | molecular chlorine |

Substance properties

| hydrogen chloride | lead(II, IV) oxide | water | chlorine | lead monoxide molar mass | 36.46 g/mol | 685.6 g/mol | 18.015 g/mol | 70.9 g/mol | 223.2 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -101 °C | 886 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | 1470 °C density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 9.5 g/cm^3 solubility in water | miscible | | | | insoluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | 1.45×10^-4 Pa s (at 1000 °C) odor | | | odorless | |
| hydrogen chloride | lead(II, IV) oxide | water | chlorine | lead monoxide molar mass | 36.46 g/mol | 685.6 g/mol | 18.015 g/mol | 70.9 g/mol | 223.2 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -101 °C | 886 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | 1470 °C density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 9.5 g/cm^3 solubility in water | miscible | | | | insoluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | 1.45×10^-4 Pa s (at 1000 °C) odor | | | odorless | |

Units

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