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H2O2 + C4H6 = H2O + CO2

Input interpretation

H_2O_2 hydrogen peroxide + CH_2=CHCH=CH_2 1, 3-butadiene ⟶ H_2O water + CO_2 carbon dioxide
H_2O_2 hydrogen peroxide + CH_2=CHCH=CH_2 1, 3-butadiene ⟶ H_2O water + CO_2 carbon dioxide

Balanced equation

Balance the chemical equation algebraically: H_2O_2 + CH_2=CHCH=CH_2 ⟶ H_2O + CO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 CH_2=CHCH=CH_2 ⟶ c_3 H_2O + c_4 CO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and C: H: | 2 c_1 + 6 c_2 = 2 c_3 O: | 2 c_1 = c_3 + 2 c_4 C: | 4 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 = 11 c_2 = 1 c_3 = 14 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 11 H_2O_2 + CH_2=CHCH=CH_2 ⟶ 14 H_2O + 4 CO_2
Balance the chemical equation algebraically: H_2O_2 + CH_2=CHCH=CH_2 ⟶ H_2O + CO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 CH_2=CHCH=CH_2 ⟶ c_3 H_2O + c_4 CO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and C: H: | 2 c_1 + 6 c_2 = 2 c_3 O: | 2 c_1 = c_3 + 2 c_4 C: | 4 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 = 11 c_2 = 1 c_3 = 14 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 11 H_2O_2 + CH_2=CHCH=CH_2 ⟶ 14 H_2O + 4 CO_2

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen peroxide + 1, 3-butadiene ⟶ water + carbon dioxide
hydrogen peroxide + 1, 3-butadiene ⟶ water + carbon dioxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O_2 + CH_2=CHCH=CH_2 ⟶ H_2O + CO_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: 11 H_2O_2 + CH_2=CHCH=CH_2 ⟶ 14 H_2O + 4 CO_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 | 11 | -11 CH_2=CHCH=CH_2 | 1 | -1 H_2O | 14 | 14 CO_2 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O_2 | 11 | -11 | ([H2O2])^(-11) CH_2=CHCH=CH_2 | 1 | -1 | ([CH2=CHCH=CH2])^(-1) H_2O | 14 | 14 | ([H2O])^14 CO_2 | 4 | 4 | ([CO2])^4 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 = ([H2O2])^(-11) ([CH2=CHCH=CH2])^(-1) ([H2O])^14 ([CO2])^4 = (([H2O])^14 ([CO2])^4)/(([H2O2])^11 [CH2=CHCH=CH2])
Construct the equilibrium constant, K, expression for: H_2O_2 + CH_2=CHCH=CH_2 ⟶ H_2O + CO_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: 11 H_2O_2 + CH_2=CHCH=CH_2 ⟶ 14 H_2O + 4 CO_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 | 11 | -11 CH_2=CHCH=CH_2 | 1 | -1 H_2O | 14 | 14 CO_2 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O_2 | 11 | -11 | ([H2O2])^(-11) CH_2=CHCH=CH_2 | 1 | -1 | ([CH2=CHCH=CH2])^(-1) H_2O | 14 | 14 | ([H2O])^14 CO_2 | 4 | 4 | ([CO2])^4 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 = ([H2O2])^(-11) ([CH2=CHCH=CH2])^(-1) ([H2O])^14 ([CO2])^4 = (([H2O])^14 ([CO2])^4)/(([H2O2])^11 [CH2=CHCH=CH2])

Rate of reaction

Construct the rate of reaction expression for: H_2O_2 + CH_2=CHCH=CH_2 ⟶ H_2O + CO_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: 11 H_2O_2 + CH_2=CHCH=CH_2 ⟶ 14 H_2O + 4 CO_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 | 11 | -11 CH_2=CHCH=CH_2 | 1 | -1 H_2O | 14 | 14 CO_2 | 4 | 4 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 | 11 | -11 | -1/11 (Δ[H2O2])/(Δt) CH_2=CHCH=CH_2 | 1 | -1 | -(Δ[CH2=CHCH=CH2])/(Δt) H_2O | 14 | 14 | 1/14 (Δ[H2O])/(Δt) CO_2 | 4 | 4 | 1/4 (Δ[CO2])/(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 = -1/11 (Δ[H2O2])/(Δt) = -(Δ[CH2=CHCH=CH2])/(Δt) = 1/14 (Δ[H2O])/(Δt) = 1/4 (Δ[CO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O_2 + CH_2=CHCH=CH_2 ⟶ H_2O + CO_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: 11 H_2O_2 + CH_2=CHCH=CH_2 ⟶ 14 H_2O + 4 CO_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 | 11 | -11 CH_2=CHCH=CH_2 | 1 | -1 H_2O | 14 | 14 CO_2 | 4 | 4 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 | 11 | -11 | -1/11 (Δ[H2O2])/(Δt) CH_2=CHCH=CH_2 | 1 | -1 | -(Δ[CH2=CHCH=CH2])/(Δt) H_2O | 14 | 14 | 1/14 (Δ[H2O])/(Δt) CO_2 | 4 | 4 | 1/4 (Δ[CO2])/(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 = -1/11 (Δ[H2O2])/(Δt) = -(Δ[CH2=CHCH=CH2])/(Δt) = 1/14 (Δ[H2O])/(Δt) = 1/4 (Δ[CO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen peroxide | 1, 3-butadiene | water | carbon dioxide formula | H_2O_2 | CH_2=CHCH=CH_2 | H_2O | CO_2 Hill formula | H_2O_2 | C_4H_6 | H_2O | CO_2 name | hydrogen peroxide | 1, 3-butadiene | water | carbon dioxide IUPAC name | hydrogen peroxide | buta-1, 3-diene | water | carbon dioxide
| hydrogen peroxide | 1, 3-butadiene | water | carbon dioxide formula | H_2O_2 | CH_2=CHCH=CH_2 | H_2O | CO_2 Hill formula | H_2O_2 | C_4H_6 | H_2O | CO_2 name | hydrogen peroxide | 1, 3-butadiene | water | carbon dioxide IUPAC name | hydrogen peroxide | buta-1, 3-diene | water | carbon dioxide

Substance properties

| hydrogen peroxide | 1, 3-butadiene | water | carbon dioxide molar mass | 34.014 g/mol | 54.09 g/mol | 18.015 g/mol | 44.009 g/mol phase | liquid (at STP) | gas (at STP) | liquid (at STP) | gas (at STP) melting point | -0.43 °C | -109 °C | 0 °C | -56.56 °C (at triple point) boiling point | 150.2 °C | -4.5 °C | 99.9839 °C | -78.5 °C (at sublimation point) density | 1.44 g/cm^3 | 0.62 g/cm^3 (at 20 °C) | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) solubility in water | miscible | insoluble | | surface tension | 0.0804 N/m | 0.0134 N/m | 0.0728 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | 7.54×10^-6 Pa s (at 20 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) odor | | | odorless | odorless
| hydrogen peroxide | 1, 3-butadiene | water | carbon dioxide molar mass | 34.014 g/mol | 54.09 g/mol | 18.015 g/mol | 44.009 g/mol phase | liquid (at STP) | gas (at STP) | liquid (at STP) | gas (at STP) melting point | -0.43 °C | -109 °C | 0 °C | -56.56 °C (at triple point) boiling point | 150.2 °C | -4.5 °C | 99.9839 °C | -78.5 °C (at sublimation point) density | 1.44 g/cm^3 | 0.62 g/cm^3 (at 20 °C) | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) solubility in water | miscible | insoluble | | surface tension | 0.0804 N/m | 0.0134 N/m | 0.0728 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | 7.54×10^-6 Pa s (at 20 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) odor | | | odorless | odorless

Units

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