Zn + MgSO4 = Mg + ZnSO4

Zn zinc + MgSO_4 magnesium sulfate ⟶ Mg magnesium + ZnSO_4 zinc sulfate

Balance the chemical equation algebraically: Zn + MgSO_4 ⟶ Mg + ZnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 MgSO_4 ⟶ c_3 Mg + c_4 ZnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, Mg, O and S: Zn: | c_1 = c_4 Mg: | c_2 = c_3 O: | 4 c_2 = 4 c_4 S: | c_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: | | Zn + MgSO_4 ⟶ Mg + ZnSO_4

+ ⟶ +

zinc + magnesium sulfate ⟶ magnesium + zinc sulfate

Construct the equilibrium constant, K, expression for: Zn + MgSO_4 ⟶ Mg + ZnSO_4 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: Zn + MgSO_4 ⟶ Mg + ZnSO_4 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 Zn | 1 | -1 MgSO_4 | 1 | -1 Mg | 1 | 1 ZnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Zn | 1 | -1 | ([Zn])^(-1) MgSO_4 | 1 | -1 | ([MgSO4])^(-1) Mg | 1 | 1 | [Mg] ZnSO_4 | 1 | 1 | [ZnSO4] 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 = ([Zn])^(-1) ([MgSO4])^(-1) [Mg] [ZnSO4] = ([Mg] [ZnSO4])/([Zn] [MgSO4])

Construct the rate of reaction expression for: Zn + MgSO_4 ⟶ Mg + ZnSO_4 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: Zn + MgSO_4 ⟶ Mg + ZnSO_4 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 Zn | 1 | -1 MgSO_4 | 1 | -1 Mg | 1 | 1 ZnSO_4 | 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 Zn | 1 | -1 | -(Δ[Zn])/(Δt) MgSO_4 | 1 | -1 | -(Δ[MgSO4])/(Δt) Mg | 1 | 1 | (Δ[Mg])/(Δt) ZnSO_4 | 1 | 1 | (Δ[ZnSO4])/(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[Zn])/(Δt) = -(Δ[MgSO4])/(Δt) = (Δ[Mg])/(Δt) = (Δ[ZnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| zinc | magnesium sulfate | magnesium | zinc sulfate formula | Zn | MgSO_4 | Mg | ZnSO_4 Hill formula | Zn | MgO_4S | Mg | O_4SZn name | zinc | magnesium sulfate | magnesium | zinc sulfate

| zinc | magnesium sulfate | magnesium | zinc sulfate molar mass | 65.38 g/mol | 120.4 g/mol | 24.305 g/mol | 161.4 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 420 °C | | 648 °C | boiling point | 907 °C | | 1090 °C | density | 7.14 g/cm^3 | | 1.738 g/cm^3 | 1.005 g/cm^3 solubility in water | insoluble | soluble | reacts | soluble odor | odorless | | | odorless