H2O + HSiCl3 = HCl + H10Si10O15

H_2O water + HSiCl3 ⟶ HCl hydrogen chloride + H10Si10O15

Balance the chemical equation algebraically: H_2O + HSiCl3 ⟶ HCl + H10Si10O15 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HSiCl3 ⟶ c_3 HCl + c_4 H10Si10O15 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Si and Cl: H: | 2 c_1 + c_2 = c_3 + 10 c_4 O: | c_1 = 15 c_4 Si: | c_2 = 10 c_4 Cl: | 3 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 15 c_2 = 10 c_3 = 30 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 15 H_2O + 10 HSiCl3 ⟶ 30 HCl + H10Si10O15

+ HSiCl3 ⟶ + H10Si10O15

water + HSiCl3 ⟶ hydrogen chloride + H10Si10O15

Construct the equilibrium constant, K, expression for: H_2O + HSiCl3 ⟶ HCl + H10Si10O15 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: 15 H_2O + 10 HSiCl3 ⟶ 30 HCl + H10Si10O15 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 H_2O | 15 | -15 HSiCl3 | 10 | -10 HCl | 30 | 30 H10Si10O15 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 15 | -15 | ([H2O])^(-15) HSiCl3 | 10 | -10 | ([HSiCl3])^(-10) HCl | 30 | 30 | ([HCl])^30 H10Si10O15 | 1 | 1 | [H10Si10O15] 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 = ([H2O])^(-15) ([HSiCl3])^(-10) ([HCl])^30 [H10Si10O15] = (([HCl])^30 [H10Si10O15])/(([H2O])^15 ([HSiCl3])^10)

Construct the rate of reaction expression for: H_2O + HSiCl3 ⟶ HCl + H10Si10O15 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: 15 H_2O + 10 HSiCl3 ⟶ 30 HCl + H10Si10O15 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 H_2O | 15 | -15 HSiCl3 | 10 | -10 HCl | 30 | 30 H10Si10O15 | 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 H_2O | 15 | -15 | -1/15 (Δ[H2O])/(Δt) HSiCl3 | 10 | -10 | -1/10 (Δ[HSiCl3])/(Δt) HCl | 30 | 30 | 1/30 (Δ[HCl])/(Δt) H10Si10O15 | 1 | 1 | (Δ[H10Si10O15])/(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 = -1/15 (Δ[H2O])/(Δt) = -1/10 (Δ[HSiCl3])/(Δt) = 1/30 (Δ[HCl])/(Δt) = (Δ[H10Si10O15])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | HSiCl3 | hydrogen chloride | H10Si10O15 formula | H_2O | HSiCl3 | HCl | H10Si10O15 Hill formula | H_2O | HCl3Si | ClH | H10O15Si10 name | water | | hydrogen chloride |

| water | HSiCl3 | hydrogen chloride | H10Si10O15 molar mass | 18.015 g/mol | 135.4 g/mol | 36.46 g/mol | 530.91 g/mol phase | liquid (at STP) | | gas (at STP) | melting point | 0 °C | | -114.17 °C | boiling point | 99.9839 °C | | -85 °C | density | 1 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | solubility in water | | | miscible | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | odor | odorless | | |