C + SiO2 = CO2 + Si

C activated charcoal + SiO_2 silicon dioxide ⟶ CO_2 carbon dioxide + Si silicon

Balance the chemical equation algebraically: C + SiO_2 ⟶ CO_2 + Si Add stoichiometric coefficients, c_i, to the reactants and products: c_1 C + c_2 SiO_2 ⟶ c_3 CO_2 + c_4 Si Set the number of atoms in the reactants equal to the number of atoms in the products for C, O and Si: C: | c_1 = c_3 O: | 2 c_2 = 2 c_3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | C + SiO_2 ⟶ CO_2 + Si

+ ⟶ +

activated charcoal + silicon dioxide ⟶ carbon dioxide + silicon

Construct the equilibrium constant, K, expression for: C + SiO_2 ⟶ CO_2 + Si 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: C + SiO_2 ⟶ CO_2 + Si 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 C | 1 | -1 SiO_2 | 1 | -1 CO_2 | 1 | 1 Si | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression C | 1 | -1 | ([C])^(-1) SiO_2 | 1 | -1 | ([SiO2])^(-1) CO_2 | 1 | 1 | [CO2] Si | 1 | 1 | [Si] 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 = ([C])^(-1) ([SiO2])^(-1) [CO2] [Si] = ([CO2] [Si])/([C] [SiO2])

Construct the rate of reaction expression for: C + SiO_2 ⟶ CO_2 + Si 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: C + SiO_2 ⟶ CO_2 + Si 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 C | 1 | -1 SiO_2 | 1 | -1 CO_2 | 1 | 1 Si | 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 C | 1 | -1 | -(Δ[C])/(Δt) SiO_2 | 1 | -1 | -(Δ[SiO2])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) Si | 1 | 1 | (Δ[Si])/(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[C])/(Δt) = -(Δ[SiO2])/(Δt) = (Δ[CO2])/(Δt) = (Δ[Si])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| activated charcoal | silicon dioxide | carbon dioxide | silicon formula | C | SiO_2 | CO_2 | Si Hill formula | C | O_2Si | CO_2 | Si name | activated charcoal | silicon dioxide | carbon dioxide | silicon IUPAC name | carbon | dioxosilane | carbon dioxide | silicon

| activated charcoal | silicon dioxide | carbon dioxide | silicon molar mass | 12.011 g/mol | 60.083 g/mol | 44.009 g/mol | 28.085 g/mol phase | solid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | 3550 °C | 1713 °C | -56.56 °C (at triple point) | 1410 °C boiling point | 4027 °C | 2950 °C | -78.5 °C (at sublimation point) | 2355 °C density | 2.26 g/cm^3 | 2.196 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 2.33 g/cm^3 solubility in water | insoluble | insoluble | | insoluble dynamic viscosity | | | 1.491×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless |