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K2CO3 + PbCl2 = KCl + PbCO3

Input interpretation

K_2CO_3 pearl ash + PbCl_2 lead(II) chloride ⟶ KCl potassium chloride + PbCO_3 cerussete
K_2CO_3 pearl ash + PbCl_2 lead(II) chloride ⟶ KCl potassium chloride + PbCO_3 cerussete

Balanced equation

Balance the chemical equation algebraically: K_2CO_3 + PbCl_2 ⟶ KCl + PbCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2CO_3 + c_2 PbCl_2 ⟶ c_3 KCl + c_4 PbCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, K, O, Cl and Pb: C: | c_1 = c_4 K: | 2 c_1 = c_3 O: | 3 c_1 = 3 c_4 Cl: | 2 c_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: | | K_2CO_3 + PbCl_2 ⟶ 2 KCl + PbCO_3
Balance the chemical equation algebraically: K_2CO_3 + PbCl_2 ⟶ KCl + PbCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2CO_3 + c_2 PbCl_2 ⟶ c_3 KCl + c_4 PbCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, K, O, Cl and Pb: C: | c_1 = c_4 K: | 2 c_1 = c_3 O: | 3 c_1 = 3 c_4 Cl: | 2 c_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: | | K_2CO_3 + PbCl_2 ⟶ 2 KCl + PbCO_3

Structures

+ ⟶ +
+ ⟶ +

Names

pearl ash + lead(II) chloride ⟶ potassium chloride + cerussete
pearl ash + lead(II) chloride ⟶ potassium chloride + cerussete

Equilibrium constant

Construct the equilibrium constant, K, expression for: K_2CO_3 + PbCl_2 ⟶ KCl + PbCO_3 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: K_2CO_3 + PbCl_2 ⟶ 2 KCl + PbCO_3 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 K_2CO_3 | 1 | -1 PbCl_2 | 1 | -1 KCl | 2 | 2 PbCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2CO_3 | 1 | -1 | ([K2CO3])^(-1) PbCl_2 | 1 | -1 | ([PbCl2])^(-1) KCl | 2 | 2 | ([KCl])^2 PbCO_3 | 1 | 1 | [PbCO3] 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 = ([K2CO3])^(-1) ([PbCl2])^(-1) ([KCl])^2 [PbCO3] = (([KCl])^2 [PbCO3])/([K2CO3] [PbCl2])
Construct the equilibrium constant, K, expression for: K_2CO_3 + PbCl_2 ⟶ KCl + PbCO_3 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: K_2CO_3 + PbCl_2 ⟶ 2 KCl + PbCO_3 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 K_2CO_3 | 1 | -1 PbCl_2 | 1 | -1 KCl | 2 | 2 PbCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2CO_3 | 1 | -1 | ([K2CO3])^(-1) PbCl_2 | 1 | -1 | ([PbCl2])^(-1) KCl | 2 | 2 | ([KCl])^2 PbCO_3 | 1 | 1 | [PbCO3] 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 = ([K2CO3])^(-1) ([PbCl2])^(-1) ([KCl])^2 [PbCO3] = (([KCl])^2 [PbCO3])/([K2CO3] [PbCl2])

Rate of reaction

Construct the rate of reaction expression for: K_2CO_3 + PbCl_2 ⟶ KCl + PbCO_3 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: K_2CO_3 + PbCl_2 ⟶ 2 KCl + PbCO_3 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 K_2CO_3 | 1 | -1 PbCl_2 | 1 | -1 KCl | 2 | 2 PbCO_3 | 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 K_2CO_3 | 1 | -1 | -(Δ[K2CO3])/(Δt) PbCl_2 | 1 | -1 | -(Δ[PbCl2])/(Δt) KCl | 2 | 2 | 1/2 (Δ[KCl])/(Δt) PbCO_3 | 1 | 1 | (Δ[PbCO3])/(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[K2CO3])/(Δt) = -(Δ[PbCl2])/(Δt) = 1/2 (Δ[KCl])/(Δt) = (Δ[PbCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: K_2CO_3 + PbCl_2 ⟶ KCl + PbCO_3 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: K_2CO_3 + PbCl_2 ⟶ 2 KCl + PbCO_3 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 K_2CO_3 | 1 | -1 PbCl_2 | 1 | -1 KCl | 2 | 2 PbCO_3 | 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 K_2CO_3 | 1 | -1 | -(Δ[K2CO3])/(Δt) PbCl_2 | 1 | -1 | -(Δ[PbCl2])/(Δt) KCl | 2 | 2 | 1/2 (Δ[KCl])/(Δt) PbCO_3 | 1 | 1 | (Δ[PbCO3])/(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[K2CO3])/(Δt) = -(Δ[PbCl2])/(Δt) = 1/2 (Δ[KCl])/(Δt) = (Δ[PbCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| pearl ash | lead(II) chloride | potassium chloride | cerussete formula | K_2CO_3 | PbCl_2 | KCl | PbCO_3 Hill formula | CK_2O_3 | Cl_2Pb | ClK | CO_3Pb name | pearl ash | lead(II) chloride | potassium chloride | cerussete IUPAC name | dipotassium carbonate | dichlorolead | potassium chloride | lead(+2) cation carbonate
| pearl ash | lead(II) chloride | potassium chloride | cerussete formula | K_2CO_3 | PbCl_2 | KCl | PbCO_3 Hill formula | CK_2O_3 | Cl_2Pb | ClK | CO_3Pb name | pearl ash | lead(II) chloride | potassium chloride | cerussete IUPAC name | dipotassium carbonate | dichlorolead | potassium chloride | lead(+2) cation carbonate

Substance properties

| pearl ash | lead(II) chloride | potassium chloride | cerussete molar mass | 138.2 g/mol | 278.1 g/mol | 74.55 g/mol | 267.2 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 891 °C | 501 °C | 770 °C | boiling point | | 950 °C | 1420 °C | density | 2.43 g/cm^3 | 5.85 g/cm^3 | 1.98 g/cm^3 | 6.43 g/cm^3 solubility in water | soluble | | soluble | insoluble odor | | | odorless |
| pearl ash | lead(II) chloride | potassium chloride | cerussete molar mass | 138.2 g/mol | 278.1 g/mol | 74.55 g/mol | 267.2 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 891 °C | 501 °C | 770 °C | boiling point | | 950 °C | 1420 °C | density | 2.43 g/cm^3 | 5.85 g/cm^3 | 1.98 g/cm^3 | 6.43 g/cm^3 solubility in water | soluble | | soluble | insoluble odor | | | odorless |

Units

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