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FeSO4 + Ba(NO3)2 = BaSO4 + Fe(NO3)2

Input interpretation

FeSO_4 duretter + Ba(NO_3)_2 barium nitrate ⟶ BaSO_4 barium sulfate + Fe(NO_3)_2 iron(II) nitrate
FeSO_4 duretter + Ba(NO_3)_2 barium nitrate ⟶ BaSO_4 barium sulfate + Fe(NO_3)_2 iron(II) nitrate

Balanced equation

Balance the chemical equation algebraically: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + Fe(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeSO_4 + c_2 Ba(NO_3)_2 ⟶ c_3 BaSO_4 + c_4 Fe(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, Ba and N: Fe: | c_1 = c_4 O: | 4 c_1 + 6 c_2 = 4 c_3 + 6 c_4 S: | c_1 = c_3 Ba: | c_2 = c_3 N: | 2 c_2 = 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + Fe(NO_3)_2
Balance the chemical equation algebraically: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + Fe(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeSO_4 + c_2 Ba(NO_3)_2 ⟶ c_3 BaSO_4 + c_4 Fe(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, Ba and N: Fe: | c_1 = c_4 O: | 4 c_1 + 6 c_2 = 4 c_3 + 6 c_4 S: | c_1 = c_3 Ba: | c_2 = c_3 N: | 2 c_2 = 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + Fe(NO_3)_2

Structures

+ ⟶ +
+ ⟶ +

Names

duretter + barium nitrate ⟶ barium sulfate + iron(II) nitrate
duretter + barium nitrate ⟶ barium sulfate + iron(II) nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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 FeSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 BaSO_4 | 1 | 1 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 FeSO_4 | 1 | -1 | ([FeSO4])^(-1) Ba(NO_3)_2 | 1 | -1 | ([Ba(NO3)2])^(-1) BaSO_4 | 1 | 1 | [BaSO4] 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 = ([FeSO4])^(-1) ([Ba(NO3)2])^(-1) [BaSO4] [Fe(NO3)2] = ([BaSO4] [Fe(NO3)2])/([FeSO4] [Ba(NO3)2])
Construct the equilibrium constant, K, expression for: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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 FeSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 BaSO_4 | 1 | 1 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 FeSO_4 | 1 | -1 | ([FeSO4])^(-1) Ba(NO_3)_2 | 1 | -1 | ([Ba(NO3)2])^(-1) BaSO_4 | 1 | 1 | [BaSO4] 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 = ([FeSO4])^(-1) ([Ba(NO3)2])^(-1) [BaSO4] [Fe(NO3)2] = ([BaSO4] [Fe(NO3)2])/([FeSO4] [Ba(NO3)2])

Rate of reaction

Construct the rate of reaction expression for: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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 FeSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 BaSO_4 | 1 | 1 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 FeSO_4 | 1 | -1 | -(Δ[FeSO4])/(Δt) Ba(NO_3)_2 | 1 | -1 | -(Δ[Ba(NO3)2])/(Δt) BaSO_4 | 1 | 1 | (Δ[BaSO4])/(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 = -(Δ[FeSO4])/(Δt) = -(Δ[Ba(NO3)2])/(Δt) = (Δ[BaSO4])/(Δt) = (Δ[Fe(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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: FeSO_4 + Ba(NO_3)_2 ⟶ BaSO_4 + 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 FeSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 BaSO_4 | 1 | 1 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 FeSO_4 | 1 | -1 | -(Δ[FeSO4])/(Δt) Ba(NO_3)_2 | 1 | -1 | -(Δ[Ba(NO3)2])/(Δt) BaSO_4 | 1 | 1 | (Δ[BaSO4])/(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 = -(Δ[FeSO4])/(Δt) = -(Δ[Ba(NO3)2])/(Δt) = (Δ[BaSO4])/(Δt) = (Δ[Fe(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| duretter | barium nitrate | barium sulfate | iron(II) nitrate formula | FeSO_4 | Ba(NO_3)_2 | BaSO_4 | Fe(NO_3)_2 Hill formula | FeO_4S | BaN_2O_6 | BaO_4S | FeN_2O_6 name | duretter | barium nitrate | barium sulfate | iron(II) nitrate IUPAC name | iron(+2) cation sulfate | barium(+2) cation dinitrate | barium(+2) cation sulfate |
| duretter | barium nitrate | barium sulfate | iron(II) nitrate formula | FeSO_4 | Ba(NO_3)_2 | BaSO_4 | Fe(NO_3)_2 Hill formula | FeO_4S | BaN_2O_6 | BaO_4S | FeN_2O_6 name | duretter | barium nitrate | barium sulfate | iron(II) nitrate IUPAC name | iron(+2) cation sulfate | barium(+2) cation dinitrate | barium(+2) cation sulfate |

Substance properties

| duretter | barium nitrate | barium sulfate | iron(II) nitrate molar mass | 151.9 g/mol | 261.34 g/mol | 233.38 g/mol | 179.85 g/mol phase | | solid (at STP) | solid (at STP) | melting point | | 592 °C | 1345 °C | density | 2.841 g/cm^3 | 3.23 g/cm^3 | 4.5 g/cm^3 | solubility in water | | | insoluble |
| duretter | barium nitrate | barium sulfate | iron(II) nitrate molar mass | 151.9 g/mol | 261.34 g/mol | 233.38 g/mol | 179.85 g/mol phase | | solid (at STP) | solid (at STP) | melting point | | 592 °C | 1345 °C | density | 2.841 g/cm^3 | 3.23 g/cm^3 | 4.5 g/cm^3 | solubility in water | | | insoluble |

Units

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