Cu + NiSO4 = CuSO4 + Ni

Cu copper + NiSO_4 nickel(II) sulfate ⟶ CuSO_4 copper(II) sulfate + Ni nickel

Balance the chemical equation algebraically: Cu + NiSO_4 ⟶ CuSO_4 + Ni Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu + c_2 NiSO_4 ⟶ c_3 CuSO_4 + c_4 Ni Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, Ni, O and S: Cu: | 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: | | Cu + NiSO_4 ⟶ CuSO_4 + Ni

+ ⟶ +

copper + nickel(II) sulfate ⟶ copper(II) sulfate + nickel

Construct the equilibrium constant, K, expression for: Cu + NiSO_4 ⟶ CuSO_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: Cu + NiSO_4 ⟶ CuSO_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 Cu | 1 | -1 NiSO_4 | 1 | -1 CuSO_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 Cu | 1 | -1 | ([Cu])^(-1) NiSO_4 | 1 | -1 | ([NiSO4])^(-1) CuSO_4 | 1 | 1 | [CuSO4] 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 = ([Cu])^(-1) ([NiSO4])^(-1) [CuSO4] [Ni] = ([CuSO4] [Ni])/([Cu] [NiSO4])

Construct the rate of reaction expression for: Cu + NiSO_4 ⟶ CuSO_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: Cu + NiSO_4 ⟶ CuSO_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 Cu | 1 | -1 NiSO_4 | 1 | -1 CuSO_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 Cu | 1 | -1 | -(Δ[Cu])/(Δt) NiSO_4 | 1 | -1 | -(Δ[NiSO4])/(Δt) CuSO_4 | 1 | 1 | (Δ[CuSO4])/(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[Cu])/(Δt) = -(Δ[NiSO4])/(Δt) = (Δ[CuSO4])/(Δt) = (Δ[Ni])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper | nickel(II) sulfate | copper(II) sulfate | nickel formula | Cu | NiSO_4 | CuSO_4 | Ni Hill formula | Cu | NiO_4S | CuO_4S | Ni name | copper | nickel(II) sulfate | copper(II) sulfate | nickel IUPAC name | copper | nickelous sulfate | copper sulfate | nickel

| copper | nickel(II) sulfate | copper(II) sulfate | nickel molar mass | 63.546 g/mol | 154.75 g/mol | 159.6 g/mol | 58.6934 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 1083 °C | | 200 °C | 1453 °C boiling point | 2567 °C | | | 2732 °C density | 8.96 g/cm^3 | 4.01 g/cm^3 | 3.603 g/cm^3 | 8.908 g/cm^3 solubility in water | insoluble | | | insoluble odor | odorless | | | odorless