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AgNO3 + FeBr2 = Fe(NO3)2 + AgBr

Input interpretation

AgNO_3 silver nitrate + FeBr_2 iron(II) bromide ⟶ Fe(NO_3)_2 iron(II) nitrate + AgBr silver bromide
AgNO_3 silver nitrate + FeBr_2 iron(II) bromide ⟶ Fe(NO_3)_2 iron(II) nitrate + AgBr silver bromide

Balanced equation

Balance the chemical equation algebraically: AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + AgBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 FeBr_2 ⟶ c_3 Fe(NO_3)_2 + c_4 AgBr Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Br and Fe: Ag: | c_1 = c_4 N: | c_1 = 2 c_3 O: | 3 c_1 = 6 c_3 Br: | 2 c_2 = c_4 Fe: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + 2 AgBr
Balance the chemical equation algebraically: AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + AgBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 FeBr_2 ⟶ c_3 Fe(NO_3)_2 + c_4 AgBr Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Br and Fe: Ag: | c_1 = c_4 N: | c_1 = 2 c_3 O: | 3 c_1 = 6 c_3 Br: | 2 c_2 = c_4 Fe: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + 2 AgBr

Structures

+ ⟶ +
+ ⟶ +

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + AgBr 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 + FeBr_2 ⟶ Fe(NO_3)_2 + 2 AgBr 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 FeBr_2 | 1 | -1 Fe(NO_3)_2 | 1 | 1 AgBr | 2 | 2 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) FeBr_2 | 1 | -1 | ([FeBr2])^(-1) Fe(NO_3)_2 | 1 | 1 | [Fe(NO3)2] AgBr | 2 | 2 | ([AgBr])^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) ([FeBr2])^(-1) [Fe(NO3)2] ([AgBr])^2 = ([Fe(NO3)2] ([AgBr])^2)/(([AgNO3])^2 [FeBr2])
Construct the equilibrium constant, K, expression for: AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + AgBr 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 + FeBr_2 ⟶ Fe(NO_3)_2 + 2 AgBr 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 FeBr_2 | 1 | -1 Fe(NO_3)_2 | 1 | 1 AgBr | 2 | 2 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) FeBr_2 | 1 | -1 | ([FeBr2])^(-1) Fe(NO_3)_2 | 1 | 1 | [Fe(NO3)2] AgBr | 2 | 2 | ([AgBr])^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) ([FeBr2])^(-1) [Fe(NO3)2] ([AgBr])^2 = ([Fe(NO3)2] ([AgBr])^2)/(([AgNO3])^2 [FeBr2])

Rate of reaction

Construct the rate of reaction expression for: AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + AgBr 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 + FeBr_2 ⟶ Fe(NO_3)_2 + 2 AgBr 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 FeBr_2 | 1 | -1 Fe(NO_3)_2 | 1 | 1 AgBr | 2 | 2 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) FeBr_2 | 1 | -1 | -(Δ[FeBr2])/(Δt) Fe(NO_3)_2 | 1 | 1 | (Δ[Fe(NO3)2])/(Δt) AgBr | 2 | 2 | 1/2 (Δ[AgBr])/(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[FeBr2])/(Δt) = (Δ[Fe(NO3)2])/(Δt) = 1/2 (Δ[AgBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: AgNO_3 + FeBr_2 ⟶ Fe(NO_3)_2 + AgBr 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 + FeBr_2 ⟶ Fe(NO_3)_2 + 2 AgBr 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 FeBr_2 | 1 | -1 Fe(NO_3)_2 | 1 | 1 AgBr | 2 | 2 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) FeBr_2 | 1 | -1 | -(Δ[FeBr2])/(Δt) Fe(NO_3)_2 | 1 | 1 | (Δ[Fe(NO3)2])/(Δt) AgBr | 2 | 2 | 1/2 (Δ[AgBr])/(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[FeBr2])/(Δt) = (Δ[Fe(NO3)2])/(Δt) = 1/2 (Δ[AgBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| silver nitrate | iron(II) bromide | iron(II) nitrate | silver bromide formula | AgNO_3 | FeBr_2 | Fe(NO_3)_2 | AgBr Hill formula | AgNO_3 | Br_2Fe | FeN_2O_6 | AgBr name | silver nitrate | iron(II) bromide | iron(II) nitrate | silver bromide IUPAC name | silver nitrate | dibromoiron | | bromosilver
| silver nitrate | iron(II) bromide | iron(II) nitrate | silver bromide formula | AgNO_3 | FeBr_2 | Fe(NO_3)_2 | AgBr Hill formula | AgNO_3 | Br_2Fe | FeN_2O_6 | AgBr name | silver nitrate | iron(II) bromide | iron(II) nitrate | silver bromide IUPAC name | silver nitrate | dibromoiron | | bromosilver

Substance properties

| silver nitrate | iron(II) bromide | iron(II) nitrate | silver bromide molar mass | 169.87 g/mol | 215.65 g/mol | 179.85 g/mol | 187.77 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 212 °C | 684 °C | | 432 °C boiling point | | 934 °C | | 1300 °C density | | 4.63 g/cm^3 | | 6.473 g/cm^3 solubility in water | soluble | | | insoluble odor | odorless | | |
| silver nitrate | iron(II) bromide | iron(II) nitrate | silver bromide molar mass | 169.87 g/mol | 215.65 g/mol | 179.85 g/mol | 187.77 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 212 °C | 684 °C | | 432 °C boiling point | | 934 °C | | 1300 °C density | | 4.63 g/cm^3 | | 6.473 g/cm^3 solubility in water | soluble | | | insoluble odor | odorless | | |

Units

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