HCl + MgS = H2S + MgCl2

HCl hydrogen chloride + MgS magnesium sulfide ⟶ H_2S hydrogen sulfide + MgCl_2 magnesium chloride

Balance the chemical equation algebraically: HCl + MgS ⟶ H_2S + MgCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 MgS ⟶ c_3 H_2S + c_4 MgCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Mg and S: Cl: | c_1 = 2 c_4 H: | c_1 = 2 c_3 Mg: | c_2 = c_4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + MgS ⟶ H_2S + MgCl_2

+ ⟶ +

hydrogen chloride + magnesium sulfide ⟶ hydrogen sulfide + magnesium chloride

Construct the equilibrium constant, K, expression for: HCl + MgS ⟶ H_2S + MgCl_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: 2 HCl + MgS ⟶ H_2S + MgCl_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 HCl | 2 | -2 MgS | 1 | -1 H_2S | 1 | 1 MgCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) MgS | 1 | -1 | ([MgS])^(-1) H_2S | 1 | 1 | [H2S] MgCl_2 | 1 | 1 | [MgCl2] 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 = ([HCl])^(-2) ([MgS])^(-1) [H2S] [MgCl2] = ([H2S] [MgCl2])/(([HCl])^2 [MgS])

Construct the rate of reaction expression for: HCl + MgS ⟶ H_2S + MgCl_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: 2 HCl + MgS ⟶ H_2S + MgCl_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 HCl | 2 | -2 MgS | 1 | -1 H_2S | 1 | 1 MgCl_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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) MgS | 1 | -1 | -(Δ[MgS])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) MgCl_2 | 1 | 1 | (Δ[MgCl2])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[MgS])/(Δt) = (Δ[H2S])/(Δt) = (Δ[MgCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | magnesium sulfide | hydrogen sulfide | magnesium chloride formula | HCl | MgS | H_2S | MgCl_2 Hill formula | ClH | MgS | H_2S | Cl_2Mg name | hydrogen chloride | magnesium sulfide | hydrogen sulfide | magnesium chloride IUPAC name | hydrogen chloride | | hydrogen sulfide | magnesium dichloride

| hydrogen chloride | magnesium sulfide | hydrogen sulfide | magnesium chloride molar mass | 36.46 g/mol | 56.36 g/mol | 34.08 g/mol | 95.2 g/mol phase | gas (at STP) | | gas (at STP) | solid (at STP) melting point | -114.17 °C | 2226 °C | -85 °C | 714 °C boiling point | -85 °C | | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | 2.68 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | 2.32 g/cm^3 solubility in water | miscible | reacts | | soluble dynamic viscosity | | | 1.239×10^-5 Pa s (at 25 °C) |