Li2CO3 + MgF2 = MgCO3 + LiF

Li_2CO_3 lithium carbonate + MgF_2 magnesium fluoride ⟶ MgCO_3 magnesium carbonate + LiF lithium fluoride

Balance the chemical equation algebraically: Li_2CO_3 + MgF_2 ⟶ MgCO_3 + LiF Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Li_2CO_3 + c_2 MgF_2 ⟶ c_3 MgCO_3 + c_4 LiF Set the number of atoms in the reactants equal to the number of atoms in the products for C, Li, O, F and Mg: C: | c_1 = c_3 Li: | 2 c_1 = c_4 O: | 3 c_1 = 3 c_3 F: | 2 c_2 = c_4 Mg: | 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Li_2CO_3 + MgF_2 ⟶ MgCO_3 + 2 LiF

+ ⟶ +

lithium carbonate + magnesium fluoride ⟶ magnesium carbonate + lithium fluoride

Construct the equilibrium constant, K, expression for: Li_2CO_3 + MgF_2 ⟶ MgCO_3 + LiF 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: Li_2CO_3 + MgF_2 ⟶ MgCO_3 + 2 LiF 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 Li_2CO_3 | 1 | -1 MgF_2 | 1 | -1 MgCO_3 | 1 | 1 LiF | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Li_2CO_3 | 1 | -1 | ([Li2CO3])^(-1) MgF_2 | 1 | -1 | ([MgF2])^(-1) MgCO_3 | 1 | 1 | [MgCO3] LiF | 2 | 2 | ([LiF])^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 = ([Li2CO3])^(-1) ([MgF2])^(-1) [MgCO3] ([LiF])^2 = ([MgCO3] ([LiF])^2)/([Li2CO3] [MgF2])

Construct the rate of reaction expression for: Li_2CO_3 + MgF_2 ⟶ MgCO_3 + LiF 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: Li_2CO_3 + MgF_2 ⟶ MgCO_3 + 2 LiF 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 Li_2CO_3 | 1 | -1 MgF_2 | 1 | -1 MgCO_3 | 1 | 1 LiF | 2 | 2 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 Li_2CO_3 | 1 | -1 | -(Δ[Li2CO3])/(Δt) MgF_2 | 1 | -1 | -(Δ[MgF2])/(Δt) MgCO_3 | 1 | 1 | (Δ[MgCO3])/(Δt) LiF | 2 | 2 | 1/2 (Δ[LiF])/(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[Li2CO3])/(Δt) = -(Δ[MgF2])/(Δt) = (Δ[MgCO3])/(Δt) = 1/2 (Δ[LiF])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| lithium carbonate | magnesium fluoride | magnesium carbonate | lithium fluoride formula | Li_2CO_3 | MgF_2 | MgCO_3 | LiF Hill formula | CLi_2O_3 | F_2Mg | CMgO_3 | FLi name | lithium carbonate | magnesium fluoride | magnesium carbonate | lithium fluoride IUPAC name | dilithium carbonate | magnesium difluoride | magnesium carbonate | lithium fluoride

| lithium carbonate | magnesium fluoride | magnesium carbonate | lithium fluoride molar mass | 73.9 g/mol | 62.302 g/mol | 84.313 g/mol | 25.94 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 618 °C | 1266 °C | | 845 °C boiling point | | 2260 °C | | 1676 °C density | 2.11 g/cm^3 | 3.15 g/cm^3 | | 2.64 g/cm^3 solubility in water | | slightly soluble | |