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I2 + Na2CO3 + C2H5OH = NaI + H2CO3 + CHI3

Input interpretation

I_2 iodine + Na_2CO_3 soda ash + CH_3CH_2OH ethanol ⟶ NaI sodium iodide + H_2CO_3 carbonic acid + CHI_3 iodoform
I_2 iodine + Na_2CO_3 soda ash + CH_3CH_2OH ethanol ⟶ NaI sodium iodide + H_2CO_3 carbonic acid + CHI_3 iodoform

Balanced equation

Balance the chemical equation algebraically: I_2 + Na_2CO_3 + CH_3CH_2OH ⟶ NaI + H_2CO_3 + CHI_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 I_2 + c_2 Na_2CO_3 + c_3 CH_3CH_2OH ⟶ c_4 NaI + c_5 H_2CO_3 + c_6 CHI_3 Set the number of atoms in the reactants equal to the number of atoms in the products for I, C, Na, O and H: I: | 2 c_1 = c_4 + 3 c_6 C: | c_2 + 2 c_3 = c_5 + c_6 Na: | 2 c_2 = c_4 O: | 3 c_2 + c_3 = 3 c_5 H: | 6 c_3 = 2 c_5 + c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 13/3 c_2 = 11/6 c_3 = 1 c_4 = 11/3 c_5 = 13/6 c_6 = 5/3 Multiply by the least common denominator, 6, to eliminate fractional coefficients: c_1 = 26 c_2 = 11 c_3 = 6 c_4 = 22 c_5 = 13 c_6 = 10 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 26 I_2 + 11 Na_2CO_3 + 6 CH_3CH_2OH ⟶ 22 NaI + 13 H_2CO_3 + 10 CHI_3
Balance the chemical equation algebraically: I_2 + Na_2CO_3 + CH_3CH_2OH ⟶ NaI + H_2CO_3 + CHI_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 I_2 + c_2 Na_2CO_3 + c_3 CH_3CH_2OH ⟶ c_4 NaI + c_5 H_2CO_3 + c_6 CHI_3 Set the number of atoms in the reactants equal to the number of atoms in the products for I, C, Na, O and H: I: | 2 c_1 = c_4 + 3 c_6 C: | c_2 + 2 c_3 = c_5 + c_6 Na: | 2 c_2 = c_4 O: | 3 c_2 + c_3 = 3 c_5 H: | 6 c_3 = 2 c_5 + c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 13/3 c_2 = 11/6 c_3 = 1 c_4 = 11/3 c_5 = 13/6 c_6 = 5/3 Multiply by the least common denominator, 6, to eliminate fractional coefficients: c_1 = 26 c_2 = 11 c_3 = 6 c_4 = 22 c_5 = 13 c_6 = 10 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 26 I_2 + 11 Na_2CO_3 + 6 CH_3CH_2OH ⟶ 22 NaI + 13 H_2CO_3 + 10 CHI_3

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

iodine + soda ash + ethanol ⟶ sodium iodide + carbonic acid + iodoform
iodine + soda ash + ethanol ⟶ sodium iodide + carbonic acid + iodoform

Equilibrium constant

Construct the equilibrium constant, K, expression for: I_2 + Na_2CO_3 + CH_3CH_2OH ⟶ NaI + H_2CO_3 + CHI_3 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: 26 I_2 + 11 Na_2CO_3 + 6 CH_3CH_2OH ⟶ 22 NaI + 13 H_2CO_3 + 10 CHI_3 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 I_2 | 26 | -26 Na_2CO_3 | 11 | -11 CH_3CH_2OH | 6 | -6 NaI | 22 | 22 H_2CO_3 | 13 | 13 CHI_3 | 10 | 10 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression I_2 | 26 | -26 | ([I2])^(-26) Na_2CO_3 | 11 | -11 | ([Na2CO3])^(-11) CH_3CH_2OH | 6 | -6 | ([CH3CH2OH])^(-6) NaI | 22 | 22 | ([NaI])^22 H_2CO_3 | 13 | 13 | ([H2CO3])^13 CHI_3 | 10 | 10 | ([CHI3])^10 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 = ([I2])^(-26) ([Na2CO3])^(-11) ([CH3CH2OH])^(-6) ([NaI])^22 ([H2CO3])^13 ([CHI3])^10 = (([NaI])^22 ([H2CO3])^13 ([CHI3])^10)/(([I2])^26 ([Na2CO3])^11 ([CH3CH2OH])^6)
Construct the equilibrium constant, K, expression for: I_2 + Na_2CO_3 + CH_3CH_2OH ⟶ NaI + H_2CO_3 + CHI_3 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: 26 I_2 + 11 Na_2CO_3 + 6 CH_3CH_2OH ⟶ 22 NaI + 13 H_2CO_3 + 10 CHI_3 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 I_2 | 26 | -26 Na_2CO_3 | 11 | -11 CH_3CH_2OH | 6 | -6 NaI | 22 | 22 H_2CO_3 | 13 | 13 CHI_3 | 10 | 10 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression I_2 | 26 | -26 | ([I2])^(-26) Na_2CO_3 | 11 | -11 | ([Na2CO3])^(-11) CH_3CH_2OH | 6 | -6 | ([CH3CH2OH])^(-6) NaI | 22 | 22 | ([NaI])^22 H_2CO_3 | 13 | 13 | ([H2CO3])^13 CHI_3 | 10 | 10 | ([CHI3])^10 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 = ([I2])^(-26) ([Na2CO3])^(-11) ([CH3CH2OH])^(-6) ([NaI])^22 ([H2CO3])^13 ([CHI3])^10 = (([NaI])^22 ([H2CO3])^13 ([CHI3])^10)/(([I2])^26 ([Na2CO3])^11 ([CH3CH2OH])^6)

Rate of reaction

Construct the rate of reaction expression for: I_2 + Na_2CO_3 + CH_3CH_2OH ⟶ NaI + H_2CO_3 + CHI_3 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: 26 I_2 + 11 Na_2CO_3 + 6 CH_3CH_2OH ⟶ 22 NaI + 13 H_2CO_3 + 10 CHI_3 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 I_2 | 26 | -26 Na_2CO_3 | 11 | -11 CH_3CH_2OH | 6 | -6 NaI | 22 | 22 H_2CO_3 | 13 | 13 CHI_3 | 10 | 10 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 I_2 | 26 | -26 | -1/26 (Δ[I2])/(Δt) Na_2CO_3 | 11 | -11 | -1/11 (Δ[Na2CO3])/(Δt) CH_3CH_2OH | 6 | -6 | -1/6 (Δ[CH3CH2OH])/(Δt) NaI | 22 | 22 | 1/22 (Δ[NaI])/(Δt) H_2CO_3 | 13 | 13 | 1/13 (Δ[H2CO3])/(Δt) CHI_3 | 10 | 10 | 1/10 (Δ[CHI3])/(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 = -1/26 (Δ[I2])/(Δt) = -1/11 (Δ[Na2CO3])/(Δt) = -1/6 (Δ[CH3CH2OH])/(Δt) = 1/22 (Δ[NaI])/(Δt) = 1/13 (Δ[H2CO3])/(Δt) = 1/10 (Δ[CHI3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: I_2 + Na_2CO_3 + CH_3CH_2OH ⟶ NaI + H_2CO_3 + CHI_3 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: 26 I_2 + 11 Na_2CO_3 + 6 CH_3CH_2OH ⟶ 22 NaI + 13 H_2CO_3 + 10 CHI_3 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 I_2 | 26 | -26 Na_2CO_3 | 11 | -11 CH_3CH_2OH | 6 | -6 NaI | 22 | 22 H_2CO_3 | 13 | 13 CHI_3 | 10 | 10 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 I_2 | 26 | -26 | -1/26 (Δ[I2])/(Δt) Na_2CO_3 | 11 | -11 | -1/11 (Δ[Na2CO3])/(Δt) CH_3CH_2OH | 6 | -6 | -1/6 (Δ[CH3CH2OH])/(Δt) NaI | 22 | 22 | 1/22 (Δ[NaI])/(Δt) H_2CO_3 | 13 | 13 | 1/13 (Δ[H2CO3])/(Δt) CHI_3 | 10 | 10 | 1/10 (Δ[CHI3])/(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 = -1/26 (Δ[I2])/(Δt) = -1/11 (Δ[Na2CO3])/(Δt) = -1/6 (Δ[CH3CH2OH])/(Δt) = 1/22 (Δ[NaI])/(Δt) = 1/13 (Δ[H2CO3])/(Δt) = 1/10 (Δ[CHI3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iodine | soda ash | ethanol | sodium iodide | carbonic acid | iodoform formula | I_2 | Na_2CO_3 | CH_3CH_2OH | NaI | H_2CO_3 | CHI_3 Hill formula | I_2 | CNa_2O_3 | C_2H_6O | INa | CH_2O_3 | CHI_3 name | iodine | soda ash | ethanol | sodium iodide | carbonic acid | iodoform IUPAC name | molecular iodine | disodium carbonate | ethanol | sodium iodide | carbonic acid | iodoform
| iodine | soda ash | ethanol | sodium iodide | carbonic acid | iodoform formula | I_2 | Na_2CO_3 | CH_3CH_2OH | NaI | H_2CO_3 | CHI_3 Hill formula | I_2 | CNa_2O_3 | C_2H_6O | INa | CH_2O_3 | CHI_3 name | iodine | soda ash | ethanol | sodium iodide | carbonic acid | iodoform IUPAC name | molecular iodine | disodium carbonate | ethanol | sodium iodide | carbonic acid | iodoform

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