H2 + C = HC4

H_2 hydrogen + C activated charcoal ⟶ HC4

Balance the chemical equation algebraically: H_2 + C ⟶ HC4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 C ⟶ c_3 HC4 Set the number of atoms in the reactants equal to the number of atoms in the products for H and C: H: | 2 c_1 = c_3 C: | c_2 = 4 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 8 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2 + 8 C ⟶ 2 HC4

+ ⟶ HC4

hydrogen + activated charcoal ⟶ HC4

Construct the equilibrium constant, K, expression for: H_2 + C ⟶ HC4 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: H_2 + 8 C ⟶ 2 HC4 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_2 | 1 | -1 C | 8 | -8 HC4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2 | 1 | -1 | ([H2])^(-1) C | 8 | -8 | ([C])^(-8) HC4 | 2 | 2 | ([HC4])^2 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 = ([H2])^(-1) ([C])^(-8) ([HC4])^2 = ([HC4])^2/([H2] ([C])^8)

Construct the rate of reaction expression for: H_2 + C ⟶ HC4 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: H_2 + 8 C ⟶ 2 HC4 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_2 | 1 | -1 C | 8 | -8 HC4 | 2 | 2 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_2 | 1 | -1 | -(Δ[H2])/(Δt) C | 8 | -8 | -1/8 (Δ[C])/(Δt) HC4 | 2 | 2 | 1/2 (Δ[HC4])/(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[H2])/(Δt) = -1/8 (Δ[C])/(Δt) = 1/2 (Δ[HC4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen | activated charcoal | HC4 formula | H_2 | C | HC4 Hill formula | H_2 | C | C4H name | hydrogen | activated charcoal | IUPAC name | molecular hydrogen | carbon |

| hydrogen | activated charcoal | HC4 molar mass | 2.016 g/mol | 12.011 g/mol | 49.052 g/mol phase | gas (at STP) | solid (at STP) | melting point | -259.2 °C | 3550 °C | boiling point | -252.8 °C | 4027 °C | density | 8.99×10^-5 g/cm^3 (at 0 °C) | 2.26 g/cm^3 | solubility in water | | insoluble | dynamic viscosity | 8.9×10^-6 Pa s (at 25 °C) | | odor | odorless | |