Input interpretation
FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3
Balanced equation
Balance the chemical equation algebraically: FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeSO4Ce(SO4)2 ⟶ c_2 Fe2(SO4)3Ce2(SO4)3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, S, O and Ce: Fe: | c_1 = 2 c_2 S: | 3 c_1 = 6 c_2 O: | 12 c_1 = 24 c_2 Ce: | c_1 = 2 c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3
Structures
FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3
Names
FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3
Equilibrium constant
![Construct the equilibrium constant, K, expression for: FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 | 2 | -2 Fe2(SO4)3Ce2(SO4)3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeSO4Ce(SO4)2 | 2 | -2 | ([FeSO4Ce(SO4)2])^(-2) Fe2(SO4)3Ce2(SO4)3 | 1 | 1 | [Fe2(SO4)3Ce2(SO4)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 = ([FeSO4Ce(SO4)2])^(-2) [Fe2(SO4)3Ce2(SO4)3] = ([Fe2(SO4)3Ce2(SO4)3])/([FeSO4Ce(SO4)2])^2](../image_source/7d8aef98de97be3b5cfc49dea94e21eb.png)
Construct the equilibrium constant, K, expression for: FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 | 2 | -2 Fe2(SO4)3Ce2(SO4)3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeSO4Ce(SO4)2 | 2 | -2 | ([FeSO4Ce(SO4)2])^(-2) Fe2(SO4)3Ce2(SO4)3 | 1 | 1 | [Fe2(SO4)3Ce2(SO4)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 = ([FeSO4Ce(SO4)2])^(-2) [Fe2(SO4)3Ce2(SO4)3] = ([Fe2(SO4)3Ce2(SO4)3])/([FeSO4Ce(SO4)2])^2
Rate of reaction
![Construct the rate of reaction expression for: FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 | 2 | -2 Fe2(SO4)3Ce2(SO4)3 | 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 FeSO4Ce(SO4)2 | 2 | -2 | -1/2 (Δ[FeSO4Ce(SO4)2])/(Δt) Fe2(SO4)3Ce2(SO4)3 | 1 | 1 | (Δ[Fe2(SO4)3Ce2(SO4)3])/(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[FeSO4Ce(SO4)2])/(Δt) = (Δ[Fe2(SO4)3Ce2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/16b3efd4ee306ad95c5a3e074dfa12b8.png)
Construct the rate of reaction expression for: FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 ⟶ Fe2(SO4)3Ce2(SO4)3 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 FeSO4Ce(SO4)2 | 2 | -2 Fe2(SO4)3Ce2(SO4)3 | 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 FeSO4Ce(SO4)2 | 2 | -2 | -1/2 (Δ[FeSO4Ce(SO4)2])/(Δt) Fe2(SO4)3Ce2(SO4)3 | 1 | 1 | (Δ[Fe2(SO4)3Ce2(SO4)3])/(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[FeSO4Ce(SO4)2])/(Δt) = (Δ[Fe2(SO4)3Ce2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| FeSO4Ce(SO4)2 | Fe2(SO4)3Ce2(SO4)3 formula | FeSO4Ce(SO4)2 | Fe2(SO4)3Ce2(SO4)3 Hill formula | CeFeO12S3 | Ce2Fe2O24S6
Substance properties
| FeSO4Ce(SO4)2 | Fe2(SO4)3Ce2(SO4)3 molar mass | 484.1 g/mol | 968.3 g/mol
Units
