C2 C=C

2 cups of C activated charcoal ⟶ C activated charcoal

Balance the chemical equation algebraically: C ⟶ C Add stoichiometric coefficients, c_i, to the reactants and products: c_1 C ⟶ c_2 C Set the number of atoms in the reactants equal to the number of atoms in the products for C: C: | c_1 = c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | C ⟶ C

Find the theoretical yield of the following reaction given 2 cups C: 2 cups of C ⟶ C Convert the specified volume of C into moles using the density at STP (2.26 g/cm^3) and the molar mass (12.011 g/mol): 2 cups ((236.6 cm^3)/(1 cup)) (2.26 g/cm^3) (1/(12.011 g/mol)) = 89.03 mol C Make a table of the molar quantities of the reagents corresponding to 89.03 mol C. Begin by filling in this molar quantity: | C | C 89.03 mol C | 89.03 mol | 89.03 mol Write the balanced equation for the reaction: C ⟶ C Use the ratios of coefficients in the balanced equation to compute the molar quantities of the remaining reagents corresponding to 89.03 mol C: Summarize the results of the previous step in the table: | C | C 89.03 mol C | 89.03 mol | 89.03 mol The theoretical yield of the products will be: Answer: | | 89.03 mol C

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activated charcoal ⟶ activated charcoal

Construct the equilibrium constant, K, expression for: C ⟶ C 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 ⟶ C 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 C | 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) C | 1 | 1 | [C] 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) [C] = ([C])/([C])

Construct the rate of reaction expression for: C ⟶ C 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 ⟶ C 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 C | 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) C | 1 | 1 | (Δ[C])/(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[C])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| activated charcoal | activated charcoal formula | C | C name | activated charcoal | activated charcoal IUPAC name | carbon | carbon

| activated charcoal | activated charcoal molar mass | 12.011 g/mol | 12.011 g/mol phase | solid (at STP) | solid (at STP) melting point | 3550 °C | 3550 °C boiling point | 4027 °C | 4027 °C density | 2.26 g/cm^3 | 2.26 g/cm^3 solubility in water | insoluble | insoluble