Mg + HI = H2 + MgI2

Mg magnesium + HI hydrogen iodide ⟶ H_2 hydrogen + MgI_2 magnesium iodide

Balance the chemical equation algebraically: Mg + HI ⟶ H_2 + MgI_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Mg + c_2 HI ⟶ c_3 H_2 + c_4 MgI_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Mg, H and I: Mg: | c_1 = c_4 H: | c_2 = 2 c_3 I: | c_2 = 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 = 2 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Mg + 2 HI ⟶ H_2 + MgI_2

+ ⟶ +

magnesium + hydrogen iodide ⟶ hydrogen + magnesium iodide

Construct the equilibrium constant, K, expression for: Mg + HI ⟶ H_2 + MgI_2 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 + 2 HI ⟶ H_2 + MgI_2 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 HI | 2 | -2 H_2 | 1 | 1 MgI_2 | 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) HI | 2 | -2 | ([HI])^(-2) H_2 | 1 | 1 | [H2] MgI_2 | 1 | 1 | [MgI2] 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) ([HI])^(-2) [H2] [MgI2] = ([H2] [MgI2])/([Mg] ([HI])^2)

Construct the rate of reaction expression for: Mg + HI ⟶ H_2 + MgI_2 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 + 2 HI ⟶ H_2 + MgI_2 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 HI | 2 | -2 H_2 | 1 | 1 MgI_2 | 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) HI | 2 | -2 | -1/2 (Δ[HI])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) MgI_2 | 1 | 1 | (Δ[MgI2])/(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) = -1/2 (Δ[HI])/(Δt) = (Δ[H2])/(Δt) = (Δ[MgI2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| magnesium | hydrogen iodide | hydrogen | magnesium iodide formula | Mg | HI | H_2 | MgI_2 Hill formula | Mg | HI | H_2 | I_2Mg name | magnesium | hydrogen iodide | hydrogen | magnesium iodide IUPAC name | magnesium | hydrogen iodide | molecular hydrogen | magnesium diiodide

| magnesium | hydrogen iodide | hydrogen | magnesium iodide molar mass | 24.305 g/mol | 127.912 g/mol | 2.016 g/mol | 278.114 g/mol phase | solid (at STP) | gas (at STP) | gas (at STP) | solid (at STP) melting point | 648 °C | -50.76 °C | -259.2 °C | 637 °C boiling point | 1090 °C | -35.55 °C | -252.8 °C | density | 1.738 g/cm^3 | 0.005228 g/cm^3 (at 25 °C) | 8.99×10^-5 g/cm^3 (at 0 °C) | 4.43 g/cm^3 solubility in water | reacts | very soluble | | dynamic viscosity | | 0.001321 Pa s (at -39 °C) | 8.9×10^-6 Pa s (at 25 °C) | odor | | | odorless | odorless