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AgNO3 + FeCl2 = AgCl + Fe(NO3)2

Input interpretation

AgNO_3 silver nitrate + FeCl_2 iron(II) chloride ⟶ AgCl silver chloride + Fe(NO_3)_2 iron(II) nitrate
AgNO_3 silver nitrate + FeCl_2 iron(II) chloride ⟶ AgCl silver chloride + Fe(NO_3)_2 iron(II) nitrate

Balanced equation

Balance the chemical equation algebraically: AgNO_3 + FeCl_2 ⟶ AgCl + Fe(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 FeCl_2 ⟶ c_3 AgCl + c_4 Fe(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Cl and Fe: Ag: | c_1 = c_3 N: | c_1 = 2 c_4 O: | 3 c_1 = 6 c_4 Cl: | 2 c_2 = c_3 Fe: | 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 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + FeCl_2 ⟶ 2 AgCl + Fe(NO_3)_2
Balance the chemical equation algebraically: AgNO_3 + FeCl_2 ⟶ AgCl + Fe(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 FeCl_2 ⟶ c_3 AgCl + c_4 Fe(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Cl and Fe: Ag: | c_1 = c_3 N: | c_1 = 2 c_4 O: | 3 c_1 = 6 c_4 Cl: | 2 c_2 = c_3 Fe: | 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 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + FeCl_2 ⟶ 2 AgCl + Fe(NO_3)_2

Structures

+ ⟶ +
+ ⟶ +

Names

silver nitrate + iron(II) chloride ⟶ silver chloride + iron(II) nitrate
silver nitrate + iron(II) chloride ⟶ silver chloride + iron(II) nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: AgNO_3 + FeCl_2 ⟶ AgCl + Fe(NO_3)_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: 2 AgNO_3 + FeCl_2 ⟶ 2 AgCl + Fe(NO_3)_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 AgNO_3 | 2 | -2 FeCl_2 | 1 | -1 AgCl | 2 | 2 Fe(NO_3)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 2 | -2 | ([AgNO3])^(-2) FeCl_2 | 1 | -1 | ([FeCl2])^(-1) AgCl | 2 | 2 | ([AgCl])^2 Fe(NO_3)_2 | 1 | 1 | [Fe(NO3)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 = ([AgNO3])^(-2) ([FeCl2])^(-1) ([AgCl])^2 [Fe(NO3)2] = (([AgCl])^2 [Fe(NO3)2])/(([AgNO3])^2 [FeCl2])
Construct the equilibrium constant, K, expression for: AgNO_3 + FeCl_2 ⟶ AgCl + Fe(NO_3)_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: 2 AgNO_3 + FeCl_2 ⟶ 2 AgCl + Fe(NO_3)_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 AgNO_3 | 2 | -2 FeCl_2 | 1 | -1 AgCl | 2 | 2 Fe(NO_3)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 2 | -2 | ([AgNO3])^(-2) FeCl_2 | 1 | -1 | ([FeCl2])^(-1) AgCl | 2 | 2 | ([AgCl])^2 Fe(NO_3)_2 | 1 | 1 | [Fe(NO3)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 = ([AgNO3])^(-2) ([FeCl2])^(-1) ([AgCl])^2 [Fe(NO3)2] = (([AgCl])^2 [Fe(NO3)2])/(([AgNO3])^2 [FeCl2])

Rate of reaction

Construct the rate of reaction expression for: AgNO_3 + FeCl_2 ⟶ AgCl + Fe(NO_3)_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: 2 AgNO_3 + FeCl_2 ⟶ 2 AgCl + Fe(NO_3)_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 AgNO_3 | 2 | -2 FeCl_2 | 1 | -1 AgCl | 2 | 2 Fe(NO_3)_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 AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) FeCl_2 | 1 | -1 | -(Δ[FeCl2])/(Δt) AgCl | 2 | 2 | 1/2 (Δ[AgCl])/(Δt) Fe(NO_3)_2 | 1 | 1 | (Δ[Fe(NO3)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 = -1/2 (Δ[AgNO3])/(Δt) = -(Δ[FeCl2])/(Δt) = 1/2 (Δ[AgCl])/(Δt) = (Δ[Fe(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: AgNO_3 + FeCl_2 ⟶ AgCl + Fe(NO_3)_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: 2 AgNO_3 + FeCl_2 ⟶ 2 AgCl + Fe(NO_3)_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 AgNO_3 | 2 | -2 FeCl_2 | 1 | -1 AgCl | 2 | 2 Fe(NO_3)_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 AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) FeCl_2 | 1 | -1 | -(Δ[FeCl2])/(Δt) AgCl | 2 | 2 | 1/2 (Δ[AgCl])/(Δt) Fe(NO_3)_2 | 1 | 1 | (Δ[Fe(NO3)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 = -1/2 (Δ[AgNO3])/(Δt) = -(Δ[FeCl2])/(Δt) = 1/2 (Δ[AgCl])/(Δt) = (Δ[Fe(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| silver nitrate | iron(II) chloride | silver chloride | iron(II) nitrate formula | AgNO_3 | FeCl_2 | AgCl | Fe(NO_3)_2 Hill formula | AgNO_3 | Cl_2Fe | AgCl | FeN_2O_6 name | silver nitrate | iron(II) chloride | silver chloride | iron(II) nitrate IUPAC name | silver nitrate | dichloroiron | chlorosilver |
| silver nitrate | iron(II) chloride | silver chloride | iron(II) nitrate formula | AgNO_3 | FeCl_2 | AgCl | Fe(NO_3)_2 Hill formula | AgNO_3 | Cl_2Fe | AgCl | FeN_2O_6 name | silver nitrate | iron(II) chloride | silver chloride | iron(II) nitrate IUPAC name | silver nitrate | dichloroiron | chlorosilver |

Substance properties

| silver nitrate | iron(II) chloride | silver chloride | iron(II) nitrate molar mass | 169.87 g/mol | 126.7 g/mol | 143.32 g/mol | 179.85 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 212 °C | 677 °C | 455 °C | boiling point | | | 1554 °C | density | | 3.16 g/cm^3 | 5.56 g/cm^3 | solubility in water | soluble | | | odor | odorless | | |
| silver nitrate | iron(II) chloride | silver chloride | iron(II) nitrate molar mass | 169.87 g/mol | 126.7 g/mol | 143.32 g/mol | 179.85 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 212 °C | 677 °C | 455 °C | boiling point | | | 1554 °C | density | | 3.16 g/cm^3 | 5.56 g/cm^3 | solubility in water | soluble | | | odor | odorless | | |

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