Search

H2SO4 + KMnO4 + C4H6 = H2O + K2SO4 + MnSO4 + CH3COOH

Input interpretation

H_2SO_4 sulfuric acid + KMnO_4 potassium permanganate + CH_2=CHCH=CH_2 1, 3-butadiene ⟶ H_2O water + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + CH_3CO_2H acetic acid
H_2SO_4 sulfuric acid + KMnO_4 potassium permanganate + CH_2=CHCH=CH_2 1, 3-butadiene ⟶ H_2O water + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + CH_3CO_2H acetic acid

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + CH_2=CHCH=CH_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + CH_3CO_2H Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 CH_2=CHCH=CH_2 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 MnSO_4 + c_7 CH_3CO_2H Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Mn and C: H: | 2 c_1 + 6 c_3 = 2 c_4 + 4 c_7 O: | 4 c_1 + 4 c_2 = c_4 + 4 c_5 + 4 c_6 + 2 c_7 S: | c_1 = c_5 + c_6 K: | c_2 = 2 c_5 Mn: | c_2 = c_6 C: | 4 c_3 = 2 c_7 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 2 c_3 = 5/3 c_4 = 4/3 c_5 = 1 c_6 = 2 c_7 = 10/3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 9 c_2 = 6 c_3 = 5 c_4 = 4 c_5 = 3 c_6 = 6 c_7 = 10 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 H_2SO_4 + 6 KMnO_4 + 5 CH_2=CHCH=CH_2 ⟶ 4 H_2O + 3 K_2SO_4 + 6 MnSO_4 + 10 CH_3CO_2H
Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + CH_2=CHCH=CH_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + CH_3CO_2H Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 CH_2=CHCH=CH_2 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 MnSO_4 + c_7 CH_3CO_2H Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Mn and C: H: | 2 c_1 + 6 c_3 = 2 c_4 + 4 c_7 O: | 4 c_1 + 4 c_2 = c_4 + 4 c_5 + 4 c_6 + 2 c_7 S: | c_1 = c_5 + c_6 K: | c_2 = 2 c_5 Mn: | c_2 = c_6 C: | 4 c_3 = 2 c_7 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 2 c_3 = 5/3 c_4 = 4/3 c_5 = 1 c_6 = 2 c_7 = 10/3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 9 c_2 = 6 c_3 = 5 c_4 = 4 c_5 = 3 c_6 = 6 c_7 = 10 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 H_2SO_4 + 6 KMnO_4 + 5 CH_2=CHCH=CH_2 ⟶ 4 H_2O + 3 K_2SO_4 + 6 MnSO_4 + 10 CH_3CO_2H

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + potassium permanganate + 1, 3-butadiene ⟶ water + potassium sulfate + manganese(II) sulfate + acetic acid
sulfuric acid + potassium permanganate + 1, 3-butadiene ⟶ water + potassium sulfate + manganese(II) sulfate + acetic acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + CH_2=CHCH=CH_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + CH_3CO_2H 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: 9 H_2SO_4 + 6 KMnO_4 + 5 CH_2=CHCH=CH_2 ⟶ 4 H_2O + 3 K_2SO_4 + 6 MnSO_4 + 10 CH_3CO_2H 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_2SO_4 | 9 | -9 KMnO_4 | 6 | -6 CH_2=CHCH=CH_2 | 5 | -5 H_2O | 4 | 4 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 CH_3CO_2H | 10 | 10 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 9 | -9 | ([H2SO4])^(-9) KMnO_4 | 6 | -6 | ([KMnO4])^(-6) CH_2=CHCH=CH_2 | 5 | -5 | ([CH2=CHCH=CH2])^(-5) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 3 | 3 | ([K2SO4])^3 MnSO_4 | 6 | 6 | ([MnSO4])^6 CH_3CO_2H | 10 | 10 | ([CH3CO2H])^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 = ([H2SO4])^(-9) ([KMnO4])^(-6) ([CH2=CHCH=CH2])^(-5) ([H2O])^4 ([K2SO4])^3 ([MnSO4])^6 ([CH3CO2H])^10 = (([H2O])^4 ([K2SO4])^3 ([MnSO4])^6 ([CH3CO2H])^10)/(([H2SO4])^9 ([KMnO4])^6 ([CH2=CHCH=CH2])^5)
Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + CH_2=CHCH=CH_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + CH_3CO_2H 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: 9 H_2SO_4 + 6 KMnO_4 + 5 CH_2=CHCH=CH_2 ⟶ 4 H_2O + 3 K_2SO_4 + 6 MnSO_4 + 10 CH_3CO_2H 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_2SO_4 | 9 | -9 KMnO_4 | 6 | -6 CH_2=CHCH=CH_2 | 5 | -5 H_2O | 4 | 4 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 CH_3CO_2H | 10 | 10 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 9 | -9 | ([H2SO4])^(-9) KMnO_4 | 6 | -6 | ([KMnO4])^(-6) CH_2=CHCH=CH_2 | 5 | -5 | ([CH2=CHCH=CH2])^(-5) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 3 | 3 | ([K2SO4])^3 MnSO_4 | 6 | 6 | ([MnSO4])^6 CH_3CO_2H | 10 | 10 | ([CH3CO2H])^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 = ([H2SO4])^(-9) ([KMnO4])^(-6) ([CH2=CHCH=CH2])^(-5) ([H2O])^4 ([K2SO4])^3 ([MnSO4])^6 ([CH3CO2H])^10 = (([H2O])^4 ([K2SO4])^3 ([MnSO4])^6 ([CH3CO2H])^10)/(([H2SO4])^9 ([KMnO4])^6 ([CH2=CHCH=CH2])^5)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + CH_2=CHCH=CH_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + CH_3CO_2H 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: 9 H_2SO_4 + 6 KMnO_4 + 5 CH_2=CHCH=CH_2 ⟶ 4 H_2O + 3 K_2SO_4 + 6 MnSO_4 + 10 CH_3CO_2H 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_2SO_4 | 9 | -9 KMnO_4 | 6 | -6 CH_2=CHCH=CH_2 | 5 | -5 H_2O | 4 | 4 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 CH_3CO_2H | 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 H_2SO_4 | 9 | -9 | -1/9 (Δ[H2SO4])/(Δt) KMnO_4 | 6 | -6 | -1/6 (Δ[KMnO4])/(Δt) CH_2=CHCH=CH_2 | 5 | -5 | -1/5 (Δ[CH2=CHCH=CH2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) MnSO_4 | 6 | 6 | 1/6 (Δ[MnSO4])/(Δt) CH_3CO_2H | 10 | 10 | 1/10 (Δ[CH3CO2H])/(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 = -1/9 (Δ[H2SO4])/(Δt) = -1/6 (Δ[KMnO4])/(Δt) = -1/5 (Δ[CH2=CHCH=CH2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/6 (Δ[MnSO4])/(Δt) = 1/10 (Δ[CH3CO2H])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + CH_2=CHCH=CH_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + CH_3CO_2H 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: 9 H_2SO_4 + 6 KMnO_4 + 5 CH_2=CHCH=CH_2 ⟶ 4 H_2O + 3 K_2SO_4 + 6 MnSO_4 + 10 CH_3CO_2H 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_2SO_4 | 9 | -9 KMnO_4 | 6 | -6 CH_2=CHCH=CH_2 | 5 | -5 H_2O | 4 | 4 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 CH_3CO_2H | 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 H_2SO_4 | 9 | -9 | -1/9 (Δ[H2SO4])/(Δt) KMnO_4 | 6 | -6 | -1/6 (Δ[KMnO4])/(Δt) CH_2=CHCH=CH_2 | 5 | -5 | -1/5 (Δ[CH2=CHCH=CH2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) MnSO_4 | 6 | 6 | 1/6 (Δ[MnSO4])/(Δt) CH_3CO_2H | 10 | 10 | 1/10 (Δ[CH3CO2H])/(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 = -1/9 (Δ[H2SO4])/(Δt) = -1/6 (Δ[KMnO4])/(Δt) = -1/5 (Δ[CH2=CHCH=CH2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/6 (Δ[MnSO4])/(Δt) = 1/10 (Δ[CH3CO2H])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium permanganate | 1, 3-butadiene | water | potassium sulfate | manganese(II) sulfate | acetic acid formula | H_2SO_4 | KMnO_4 | CH_2=CHCH=CH_2 | H_2O | K_2SO_4 | MnSO_4 | CH_3CO_2H Hill formula | H_2O_4S | KMnO_4 | C_4H_6 | H_2O | K_2O_4S | MnSO_4 | C_2H_4O_2 name | sulfuric acid | potassium permanganate | 1, 3-butadiene | water | potassium sulfate | manganese(II) sulfate | acetic acid IUPAC name | sulfuric acid | potassium permanganate | buta-1, 3-diene | water | dipotassium sulfate | manganese(+2) cation sulfate | acetic acid
| sulfuric acid | potassium permanganate | 1, 3-butadiene | water | potassium sulfate | manganese(II) sulfate | acetic acid formula | H_2SO_4 | KMnO_4 | CH_2=CHCH=CH_2 | H_2O | K_2SO_4 | MnSO_4 | CH_3CO_2H Hill formula | H_2O_4S | KMnO_4 | C_4H_6 | H_2O | K_2O_4S | MnSO_4 | C_2H_4O_2 name | sulfuric acid | potassium permanganate | 1, 3-butadiene | water | potassium sulfate | manganese(II) sulfate | acetic acid IUPAC name | sulfuric acid | potassium permanganate | buta-1, 3-diene | water | dipotassium sulfate | manganese(+2) cation sulfate | acetic acid

Random Queries

specific heat of solidification of group 14 elements
H2 + KIO3 + S2O4 = H2O + I2 + K + S4O6
KOH + I2 + C3H6O = H2O + KI + CHI3 + CH3COOK
D-gamma-tocopherol
mass fractions of soda ash
freezing point of diphosphorous tetraiodide vs 3-(iodomethyl)pyridine hydriodide
net ionic charge of selenide anion vs tin(II) cation
discovery countries of group 12 elements
chlorine Cl-Cl bond
chemical types of ytterbium(III) chloride hexahydrate