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Pb(NO3)2 + NH4Cl = NH4NO3 + PbCl2

Input interpretation

Pb(NO_3)_2 lead(II) nitrate + NH_4Cl ammonium chloride ⟶ NH_4NO_3 ammonium nitrate + PbCl_2 lead(II) chloride
Pb(NO_3)_2 lead(II) nitrate + NH_4Cl ammonium chloride ⟶ NH_4NO_3 ammonium nitrate + PbCl_2 lead(II) chloride

Balanced equation

Balance the chemical equation algebraically: Pb(NO_3)_2 + NH_4Cl ⟶ NH_4NO_3 + PbCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 NH_4Cl ⟶ c_3 NH_4NO_3 + c_4 PbCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb, Cl and H: N: | 2 c_1 + c_2 = 2 c_3 O: | 6 c_1 = 3 c_3 Pb: | c_1 = c_4 Cl: | c_2 = 2 c_4 H: | 4 c_2 = 4 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Pb(NO_3)_2 + 2 NH_4Cl ⟶ 2 NH_4NO_3 + PbCl_2
Balance the chemical equation algebraically: Pb(NO_3)_2 + NH_4Cl ⟶ NH_4NO_3 + PbCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 NH_4Cl ⟶ c_3 NH_4NO_3 + c_4 PbCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb, Cl and H: N: | 2 c_1 + c_2 = 2 c_3 O: | 6 c_1 = 3 c_3 Pb: | c_1 = c_4 Cl: | c_2 = 2 c_4 H: | 4 c_2 = 4 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Pb(NO_3)_2 + 2 NH_4Cl ⟶ 2 NH_4NO_3 + PbCl_2

Structures

+ ⟶ +
+ ⟶ +

Names

lead(II) nitrate + ammonium chloride ⟶ ammonium nitrate + lead(II) chloride
lead(II) nitrate + ammonium chloride ⟶ ammonium nitrate + lead(II) chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + NH_4Cl ⟶ NH_4NO_3 + PbCl_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: Pb(NO_3)_2 + 2 NH_4Cl ⟶ 2 NH_4NO_3 + PbCl_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 Pb(NO_3)_2 | 1 | -1 NH_4Cl | 2 | -2 NH_4NO_3 | 2 | 2 PbCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Pb(NO_3)_2 | 1 | -1 | ([Pb(NO3)2])^(-1) NH_4Cl | 2 | -2 | ([NH4Cl])^(-2) NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 PbCl_2 | 1 | 1 | [PbCl2] 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 = ([Pb(NO3)2])^(-1) ([NH4Cl])^(-2) ([NH4NO3])^2 [PbCl2] = (([NH4NO3])^2 [PbCl2])/([Pb(NO3)2] ([NH4Cl])^2)
Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + NH_4Cl ⟶ NH_4NO_3 + PbCl_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: Pb(NO_3)_2 + 2 NH_4Cl ⟶ 2 NH_4NO_3 + PbCl_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 Pb(NO_3)_2 | 1 | -1 NH_4Cl | 2 | -2 NH_4NO_3 | 2 | 2 PbCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Pb(NO_3)_2 | 1 | -1 | ([Pb(NO3)2])^(-1) NH_4Cl | 2 | -2 | ([NH4Cl])^(-2) NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 PbCl_2 | 1 | 1 | [PbCl2] 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 = ([Pb(NO3)2])^(-1) ([NH4Cl])^(-2) ([NH4NO3])^2 [PbCl2] = (([NH4NO3])^2 [PbCl2])/([Pb(NO3)2] ([NH4Cl])^2)

Rate of reaction

Construct the rate of reaction expression for: Pb(NO_3)_2 + NH_4Cl ⟶ NH_4NO_3 + PbCl_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: Pb(NO_3)_2 + 2 NH_4Cl ⟶ 2 NH_4NO_3 + PbCl_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 Pb(NO_3)_2 | 1 | -1 NH_4Cl | 2 | -2 NH_4NO_3 | 2 | 2 PbCl_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 Pb(NO_3)_2 | 1 | -1 | -(Δ[Pb(NO3)2])/(Δt) NH_4Cl | 2 | -2 | -1/2 (Δ[NH4Cl])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(Δt) PbCl_2 | 1 | 1 | (Δ[PbCl2])/(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[Pb(NO3)2])/(Δt) = -1/2 (Δ[NH4Cl])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) = (Δ[PbCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Pb(NO_3)_2 + NH_4Cl ⟶ NH_4NO_3 + PbCl_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: Pb(NO_3)_2 + 2 NH_4Cl ⟶ 2 NH_4NO_3 + PbCl_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 Pb(NO_3)_2 | 1 | -1 NH_4Cl | 2 | -2 NH_4NO_3 | 2 | 2 PbCl_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 Pb(NO_3)_2 | 1 | -1 | -(Δ[Pb(NO3)2])/(Δt) NH_4Cl | 2 | -2 | -1/2 (Δ[NH4Cl])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(Δt) PbCl_2 | 1 | 1 | (Δ[PbCl2])/(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[Pb(NO3)2])/(Δt) = -1/2 (Δ[NH4Cl])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) = (Δ[PbCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| lead(II) nitrate | ammonium chloride | ammonium nitrate | lead(II) chloride formula | Pb(NO_3)_2 | NH_4Cl | NH_4NO_3 | PbCl_2 Hill formula | N_2O_6Pb | ClH_4N | H_4N_2O_3 | Cl_2Pb name | lead(II) nitrate | ammonium chloride | ammonium nitrate | lead(II) chloride IUPAC name | plumbous dinitrate | ammonium chloride | | dichlorolead
| lead(II) nitrate | ammonium chloride | ammonium nitrate | lead(II) chloride formula | Pb(NO_3)_2 | NH_4Cl | NH_4NO_3 | PbCl_2 Hill formula | N_2O_6Pb | ClH_4N | H_4N_2O_3 | Cl_2Pb name | lead(II) nitrate | ammonium chloride | ammonium nitrate | lead(II) chloride IUPAC name | plumbous dinitrate | ammonium chloride | | dichlorolead

Substance properties

| lead(II) nitrate | ammonium chloride | ammonium nitrate | lead(II) chloride molar mass | 331.2 g/mol | 53.49 g/mol | 80.04 g/mol | 278.1 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 340 °C | 169 °C | 501 °C boiling point | | | 210 °C | 950 °C density | | 1.5256 g/cm^3 | 1.73 g/cm^3 | 5.85 g/cm^3 solubility in water | | soluble | | odor | odorless | | odorless |
| lead(II) nitrate | ammonium chloride | ammonium nitrate | lead(II) chloride molar mass | 331.2 g/mol | 53.49 g/mol | 80.04 g/mol | 278.1 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 340 °C | 169 °C | 501 °C boiling point | | | 210 °C | 950 °C density | | 1.5256 g/cm^3 | 1.73 g/cm^3 | 5.85 g/cm^3 solubility in water | | soluble | | odor | odorless | | odorless |

Units

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