H2O + SiH4 = H2 + SiO2

H_2O water + SiH_4 silane ⟶ H_2 hydrogen + SiO_2 silicon dioxide

Balance the chemical equation algebraically: H_2O + SiH_4 ⟶ H_2 + SiO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SiH_4 ⟶ c_3 H_2 + c_4 SiO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Si: H: | 2 c_1 + 4 c_2 = 2 c_3 O: | c_1 = 2 c_4 Si: | c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 4 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + SiH_4 ⟶ 4 H_2 + SiO_2

+ ⟶ +

water + silane ⟶ hydrogen + silicon dioxide

Construct the equilibrium constant, K, expression for: H_2O + SiH_4 ⟶ H_2 + SiO_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 H_2O + SiH_4 ⟶ 4 H_2 + SiO_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 H_2O | 2 | -2 SiH_4 | 1 | -1 H_2 | 4 | 4 SiO_2 | 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 | 2 | -2 | ([H2O])^(-2) SiH_4 | 1 | -1 | ([SiH4])^(-1) H_2 | 4 | 4 | ([H2])^4 SiO_2 | 1 | 1 | [SiO2] 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])^(-2) ([SiH4])^(-1) ([H2])^4 [SiO2] = (([H2])^4 [SiO2])/(([H2O])^2 [SiH4])

Construct the rate of reaction expression for: H_2O + SiH_4 ⟶ H_2 + SiO_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 H_2O + SiH_4 ⟶ 4 H_2 + SiO_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 H_2O | 2 | -2 SiH_4 | 1 | -1 H_2 | 4 | 4 SiO_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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) SiH_4 | 1 | -1 | -(Δ[SiH4])/(Δt) H_2 | 4 | 4 | 1/4 (Δ[H2])/(Δt) SiO_2 | 1 | 1 | (Δ[SiO2])/(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[H2O])/(Δt) = -(Δ[SiH4])/(Δt) = 1/4 (Δ[H2])/(Δt) = (Δ[SiO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | silane | hydrogen | silicon dioxide formula | H_2O | SiH_4 | H_2 | SiO_2 Hill formula | H_2O | H_4Si | H_2 | O_2Si name | water | silane | hydrogen | silicon dioxide IUPAC name | water | silane | molecular hydrogen | dioxosilane

| water | silane | hydrogen | silicon dioxide molar mass | 18.015 g/mol | 32.117 g/mol | 2.016 g/mol | 60.083 g/mol phase | liquid (at STP) | gas (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | -185 °C | -259.2 °C | 1713 °C boiling point | 99.9839 °C | -112 °C | -252.8 °C | 2950 °C density | 1 g/cm^3 | 0.001313 g/cm^3 (at 25 °C) | 8.99×10^-5 g/cm^3 (at 0 °C) | 2.196 g/cm^3 solubility in water | | | | insoluble surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | odorless | | odorless | odorless