Fe + NiSO4 = FeSO4 + Ni

Fe iron + NiSO_4 nickel(II) sulfate ⟶ FeSO_4 duretter + Ni nickel

Balance the chemical equation algebraically: Fe + NiSO_4 ⟶ FeSO_4 + Ni Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 NiSO_4 ⟶ c_3 FeSO_4 + c_4 Ni Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, Ni, O and S: Fe: | c_1 = c_3 Ni: | c_2 = c_4 O: | 4 c_2 = 4 c_3 S: | 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_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: | | Fe + NiSO_4 ⟶ FeSO_4 + Ni

+ ⟶ +

iron + nickel(II) sulfate ⟶ duretter + nickel

Construct the equilibrium constant, K, expression for: Fe + NiSO_4 ⟶ FeSO_4 + Ni 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: Fe + NiSO_4 ⟶ FeSO_4 + Ni 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 Fe | 1 | -1 NiSO_4 | 1 | -1 FeSO_4 | 1 | 1 Ni | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe | 1 | -1 | ([Fe])^(-1) NiSO_4 | 1 | -1 | ([NiSO4])^(-1) FeSO_4 | 1 | 1 | [FeSO4] Ni | 1 | 1 | [Ni] 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 = ([Fe])^(-1) ([NiSO4])^(-1) [FeSO4] [Ni] = ([FeSO4] [Ni])/([Fe] [NiSO4])

Construct the rate of reaction expression for: Fe + NiSO_4 ⟶ FeSO_4 + Ni 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: Fe + NiSO_4 ⟶ FeSO_4 + Ni 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 Fe | 1 | -1 NiSO_4 | 1 | -1 FeSO_4 | 1 | 1 Ni | 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 Fe | 1 | -1 | -(Δ[Fe])/(Δt) NiSO_4 | 1 | -1 | -(Δ[NiSO4])/(Δt) FeSO_4 | 1 | 1 | (Δ[FeSO4])/(Δt) Ni | 1 | 1 | (Δ[Ni])/(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[Fe])/(Δt) = -(Δ[NiSO4])/(Δt) = (Δ[FeSO4])/(Δt) = (Δ[Ni])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron | nickel(II) sulfate | duretter | nickel formula | Fe | NiSO_4 | FeSO_4 | Ni Hill formula | Fe | NiO_4S | FeO_4S | Ni name | iron | nickel(II) sulfate | duretter | nickel IUPAC name | iron | nickelous sulfate | iron(+2) cation sulfate | nickel

| iron | nickel(II) sulfate | duretter | nickel molar mass | 55.845 g/mol | 154.75 g/mol | 151.9 g/mol | 58.6934 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 1535 °C | | | 1453 °C boiling point | 2750 °C | | | 2732 °C density | 7.874 g/cm^3 | 4.01 g/cm^3 | 2.841 g/cm^3 | 8.908 g/cm^3 solubility in water | insoluble | | | insoluble odor | | | | odorless