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FeCl3 + AgNO3 = Fe(NO3)3 + AgCl

Input interpretation

FeCl_3 (iron(III) chloride) + AgNO_3 (silver nitrate) ⟶ Fe(NO_3)_3 (ferric nitrate) + AgCl (silver chloride)
FeCl_3 (iron(III) chloride) + AgNO_3 (silver nitrate) ⟶ Fe(NO_3)_3 (ferric nitrate) + AgCl (silver chloride)

Balanced equation

Balance the chemical equation algebraically: FeCl_3 + AgNO_3 ⟶ Fe(NO_3)_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeCl_3 + c_2 AgNO_3 ⟶ c_3 Fe(NO_3)_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Fe, Ag, N and O: Cl: | 3 c_1 = c_4 Fe: | c_1 = c_3 Ag: | c_2 = c_4 N: | c_2 = 3 c_3 O: | 3 c_2 = 9 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 = 3 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeCl_3 + 3 AgNO_3 ⟶ Fe(NO_3)_3 + 3 AgCl
Balance the chemical equation algebraically: FeCl_3 + AgNO_3 ⟶ Fe(NO_3)_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeCl_3 + c_2 AgNO_3 ⟶ c_3 Fe(NO_3)_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Fe, Ag, N and O: Cl: | 3 c_1 = c_4 Fe: | c_1 = c_3 Ag: | c_2 = c_4 N: | c_2 = 3 c_3 O: | 3 c_2 = 9 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 = 3 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeCl_3 + 3 AgNO_3 ⟶ Fe(NO_3)_3 + 3 AgCl

Structures

+ ⟶ +
+ ⟶ +

Names

iron(III) chloride + silver nitrate ⟶ ferric nitrate + silver chloride
iron(III) chloride + silver nitrate ⟶ ferric nitrate + silver chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: FeCl_3 + AgNO_3 ⟶ Fe(NO_3)_3 + AgCl 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: FeCl_3 + 3 AgNO_3 ⟶ Fe(NO_3)_3 + 3 AgCl 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 FeCl_3 | 1 | -1 AgNO_3 | 3 | -3 Fe(NO_3)_3 | 1 | 1 AgCl | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeCl_3 | 1 | -1 | ([FeCl3])^(-1) AgNO_3 | 3 | -3 | ([AgNO3])^(-3) Fe(NO_3)_3 | 1 | 1 | [Fe(NO3)3] AgCl | 3 | 3 | ([AgCl])^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 = ([FeCl3])^(-1) ([AgNO3])^(-3) [Fe(NO3)3] ([AgCl])^3 = ([Fe(NO3)3] ([AgCl])^3)/([FeCl3] ([AgNO3])^3)
Construct the equilibrium constant, K, expression for: FeCl_3 + AgNO_3 ⟶ Fe(NO_3)_3 + AgCl 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: FeCl_3 + 3 AgNO_3 ⟶ Fe(NO_3)_3 + 3 AgCl 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 FeCl_3 | 1 | -1 AgNO_3 | 3 | -3 Fe(NO_3)_3 | 1 | 1 AgCl | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeCl_3 | 1 | -1 | ([FeCl3])^(-1) AgNO_3 | 3 | -3 | ([AgNO3])^(-3) Fe(NO_3)_3 | 1 | 1 | [Fe(NO3)3] AgCl | 3 | 3 | ([AgCl])^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 = ([FeCl3])^(-1) ([AgNO3])^(-3) [Fe(NO3)3] ([AgCl])^3 = ([Fe(NO3)3] ([AgCl])^3)/([FeCl3] ([AgNO3])^3)

Rate of reaction

Construct the rate of reaction expression for: FeCl_3 + AgNO_3 ⟶ Fe(NO_3)_3 + AgCl 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: FeCl_3 + 3 AgNO_3 ⟶ Fe(NO_3)_3 + 3 AgCl 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 FeCl_3 | 1 | -1 AgNO_3 | 3 | -3 Fe(NO_3)_3 | 1 | 1 AgCl | 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 FeCl_3 | 1 | -1 | -(Δ[FeCl3])/(Δt) AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) Fe(NO_3)_3 | 1 | 1 | (Δ[Fe(NO3)3])/(Δt) AgCl | 3 | 3 | 1/3 (Δ[AgCl])/(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[FeCl3])/(Δt) = -1/3 (Δ[AgNO3])/(Δt) = (Δ[Fe(NO3)3])/(Δt) = 1/3 (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: FeCl_3 + AgNO_3 ⟶ Fe(NO_3)_3 + AgCl 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: FeCl_3 + 3 AgNO_3 ⟶ Fe(NO_3)_3 + 3 AgCl 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 FeCl_3 | 1 | -1 AgNO_3 | 3 | -3 Fe(NO_3)_3 | 1 | 1 AgCl | 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 FeCl_3 | 1 | -1 | -(Δ[FeCl3])/(Δt) AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) Fe(NO_3)_3 | 1 | 1 | (Δ[Fe(NO3)3])/(Δt) AgCl | 3 | 3 | 1/3 (Δ[AgCl])/(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[FeCl3])/(Δt) = -1/3 (Δ[AgNO3])/(Δt) = (Δ[Fe(NO3)3])/(Δt) = 1/3 (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iron(III) chloride | silver nitrate | ferric nitrate | silver chloride formula | FeCl_3 | AgNO_3 | Fe(NO_3)_3 | AgCl Hill formula | Cl_3Fe | AgNO_3 | FeN_3O_9 | AgCl name | iron(III) chloride | silver nitrate | ferric nitrate | silver chloride IUPAC name | trichloroiron | silver nitrate | iron(+3) cation trinitrate | chlorosilver
| iron(III) chloride | silver nitrate | ferric nitrate | silver chloride formula | FeCl_3 | AgNO_3 | Fe(NO_3)_3 | AgCl Hill formula | Cl_3Fe | AgNO_3 | FeN_3O_9 | AgCl name | iron(III) chloride | silver nitrate | ferric nitrate | silver chloride IUPAC name | trichloroiron | silver nitrate | iron(+3) cation trinitrate | chlorosilver

Substance properties

| iron(III) chloride | silver nitrate | ferric nitrate | silver chloride molar mass | 162.2 g/mol | 169.87 g/mol | 241.86 g/mol | 143.32 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 304 °C | 212 °C | 35 °C | 455 °C boiling point | | | | 1554 °C density | | | 1.7 g/cm^3 | 5.56 g/cm^3 solubility in water | | soluble | very soluble | odor | | odorless | |
| iron(III) chloride | silver nitrate | ferric nitrate | silver chloride molar mass | 162.2 g/mol | 169.87 g/mol | 241.86 g/mol | 143.32 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 304 °C | 212 °C | 35 °C | 455 °C boiling point | | | | 1554 °C density | | | 1.7 g/cm^3 | 5.56 g/cm^3 solubility in water | | soluble | very soluble | odor | | odorless | |

Units

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