Mg + Si = MgSi

Mg magnesium + Si silicon ⟶ MgSi

Balance the chemical equation algebraically: Mg + Si ⟶ MgSi Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Mg + c_2 Si ⟶ c_3 MgSi Set the number of atoms in the reactants equal to the number of atoms in the products for Mg and Si: Mg: | c_1 = c_3 Si: | 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Mg + Si ⟶ MgSi

+ ⟶ MgSi

magnesium + silicon ⟶ MgSi

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

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

| magnesium | silicon | MgSi formula | Mg | Si | MgSi name | magnesium | silicon |

| magnesium | silicon | MgSi molar mass | 24.305 g/mol | 28.085 g/mol | 52.39 g/mol phase | solid (at STP) | solid (at STP) | melting point | 648 °C | 1410 °C | boiling point | 1090 °C | 2355 °C | density | 1.738 g/cm^3 | 2.33 g/cm^3 | solubility in water | reacts | insoluble |