Search

KMnO4 + C3H8O3 = H2O + CO2 + MnO2 + K2CO3

Input interpretation

KMnO_4 potassium permanganate + HOCH_2CH(OH)CH_2OH glycerol ⟶ H_2O water + CO_2 carbon dioxide + MnO_2 manganese dioxide + K_2CO_3 pearl ash
KMnO_4 potassium permanganate + HOCH_2CH(OH)CH_2OH glycerol ⟶ H_2O water + CO_2 carbon dioxide + MnO_2 manganese dioxide + K_2CO_3 pearl ash

Balanced equation

Balance the chemical equation algebraically: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + MnO_2 + K_2CO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 HOCH_2CH(OH)CH_2OH ⟶ c_3 H_2O + c_4 CO_2 + c_5 MnO_2 + c_6 K_2CO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, C and H: K: | c_1 = 2 c_6 Mn: | c_1 = c_5 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 2 c_5 + 3 c_6 C: | 3 c_2 = c_4 + c_6 H: | 8 c_2 = 2 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 7 c_2 = 3/2 c_3 = 6 c_4 = 1 c_5 = 7 c_6 = 7/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 14 c_2 = 3 c_3 = 12 c_4 = 2 c_5 = 14 c_6 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 KMnO_4 + 3 HOCH_2CH(OH)CH_2OH ⟶ 12 H_2O + 2 CO_2 + 14 MnO_2 + 7 K_2CO_3
Balance the chemical equation algebraically: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + MnO_2 + K_2CO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 HOCH_2CH(OH)CH_2OH ⟶ c_3 H_2O + c_4 CO_2 + c_5 MnO_2 + c_6 K_2CO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, C and H: K: | c_1 = 2 c_6 Mn: | c_1 = c_5 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 2 c_5 + 3 c_6 C: | 3 c_2 = c_4 + c_6 H: | 8 c_2 = 2 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 7 c_2 = 3/2 c_3 = 6 c_4 = 1 c_5 = 7 c_6 = 7/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 14 c_2 = 3 c_3 = 12 c_4 = 2 c_5 = 14 c_6 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 KMnO_4 + 3 HOCH_2CH(OH)CH_2OH ⟶ 12 H_2O + 2 CO_2 + 14 MnO_2 + 7 K_2CO_3

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

potassium permanganate + glycerol ⟶ water + carbon dioxide + manganese dioxide + pearl ash
potassium permanganate + glycerol ⟶ water + carbon dioxide + manganese dioxide + pearl ash

Equilibrium constant

Construct the equilibrium constant, K, expression for: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + MnO_2 + K_2CO_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: 14 KMnO_4 + 3 HOCH_2CH(OH)CH_2OH ⟶ 12 H_2O + 2 CO_2 + 14 MnO_2 + 7 K_2CO_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 KMnO_4 | 14 | -14 HOCH_2CH(OH)CH_2OH | 3 | -3 H_2O | 12 | 12 CO_2 | 2 | 2 MnO_2 | 14 | 14 K_2CO_3 | 7 | 7 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 14 | -14 | ([KMnO4])^(-14) HOCH_2CH(OH)CH_2OH | 3 | -3 | ([HOCH2CH(OH)CH2OH])^(-3) H_2O | 12 | 12 | ([H2O])^12 CO_2 | 2 | 2 | ([CO2])^2 MnO_2 | 14 | 14 | ([MnO2])^14 K_2CO_3 | 7 | 7 | ([K2CO3])^7 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 = ([KMnO4])^(-14) ([HOCH2CH(OH)CH2OH])^(-3) ([H2O])^12 ([CO2])^2 ([MnO2])^14 ([K2CO3])^7 = (([H2O])^12 ([CO2])^2 ([MnO2])^14 ([K2CO3])^7)/(([KMnO4])^14 ([HOCH2CH(OH)CH2OH])^3)
Construct the equilibrium constant, K, expression for: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + MnO_2 + K_2CO_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: 14 KMnO_4 + 3 HOCH_2CH(OH)CH_2OH ⟶ 12 H_2O + 2 CO_2 + 14 MnO_2 + 7 K_2CO_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 KMnO_4 | 14 | -14 HOCH_2CH(OH)CH_2OH | 3 | -3 H_2O | 12 | 12 CO_2 | 2 | 2 MnO_2 | 14 | 14 K_2CO_3 | 7 | 7 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 14 | -14 | ([KMnO4])^(-14) HOCH_2CH(OH)CH_2OH | 3 | -3 | ([HOCH2CH(OH)CH2OH])^(-3) H_2O | 12 | 12 | ([H2O])^12 CO_2 | 2 | 2 | ([CO2])^2 MnO_2 | 14 | 14 | ([MnO2])^14 K_2CO_3 | 7 | 7 | ([K2CO3])^7 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 = ([KMnO4])^(-14) ([HOCH2CH(OH)CH2OH])^(-3) ([H2O])^12 ([CO2])^2 ([MnO2])^14 ([K2CO3])^7 = (([H2O])^12 ([CO2])^2 ([MnO2])^14 ([K2CO3])^7)/(([KMnO4])^14 ([HOCH2CH(OH)CH2OH])^3)

Rate of reaction

Construct the rate of reaction expression for: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + MnO_2 + K_2CO_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: 14 KMnO_4 + 3 HOCH_2CH(OH)CH_2OH ⟶ 12 H_2O + 2 CO_2 + 14 MnO_2 + 7 K_2CO_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 KMnO_4 | 14 | -14 HOCH_2CH(OH)CH_2OH | 3 | -3 H_2O | 12 | 12 CO_2 | 2 | 2 MnO_2 | 14 | 14 K_2CO_3 | 7 | 7 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 KMnO_4 | 14 | -14 | -1/14 (Δ[KMnO4])/(Δt) HOCH_2CH(OH)CH_2OH | 3 | -3 | -1/3 (Δ[HOCH2CH(OH)CH2OH])/(Δt) H_2O | 12 | 12 | 1/12 (Δ[H2O])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) MnO_2 | 14 | 14 | 1/14 (Δ[MnO2])/(Δt) K_2CO_3 | 7 | 7 | 1/7 (Δ[K2CO3])/(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 = -1/14 (Δ[KMnO4])/(Δt) = -1/3 (Δ[HOCH2CH(OH)CH2OH])/(Δt) = 1/12 (Δ[H2O])/(Δt) = 1/2 (Δ[CO2])/(Δt) = 1/14 (Δ[MnO2])/(Δt) = 1/7 (Δ[K2CO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + MnO_2 + K_2CO_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: 14 KMnO_4 + 3 HOCH_2CH(OH)CH_2OH ⟶ 12 H_2O + 2 CO_2 + 14 MnO_2 + 7 K_2CO_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 KMnO_4 | 14 | -14 HOCH_2CH(OH)CH_2OH | 3 | -3 H_2O | 12 | 12 CO_2 | 2 | 2 MnO_2 | 14 | 14 K_2CO_3 | 7 | 7 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 KMnO_4 | 14 | -14 | -1/14 (Δ[KMnO4])/(Δt) HOCH_2CH(OH)CH_2OH | 3 | -3 | -1/3 (Δ[HOCH2CH(OH)CH2OH])/(Δt) H_2O | 12 | 12 | 1/12 (Δ[H2O])/(Δt) CO_2 | 2 | 2 | 1/2 (Δ[CO2])/(Δt) MnO_2 | 14 | 14 | 1/14 (Δ[MnO2])/(Δt) K_2CO_3 | 7 | 7 | 1/7 (Δ[K2CO3])/(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 = -1/14 (Δ[KMnO4])/(Δt) = -1/3 (Δ[HOCH2CH(OH)CH2OH])/(Δt) = 1/12 (Δ[H2O])/(Δt) = 1/2 (Δ[CO2])/(Δt) = 1/14 (Δ[MnO2])/(Δt) = 1/7 (Δ[K2CO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium permanganate | glycerol | water | carbon dioxide | manganese dioxide | pearl ash formula | KMnO_4 | HOCH_2CH(OH)CH_2OH | H_2O | CO_2 | MnO_2 | K_2CO_3 Hill formula | KMnO_4 | C_3H_8O_3 | H_2O | CO_2 | MnO_2 | CK_2O_3 name | potassium permanganate | glycerol | water | carbon dioxide | manganese dioxide | pearl ash IUPAC name | potassium permanganate | glycerol | water | carbon dioxide | dioxomanganese | dipotassium carbonate
| potassium permanganate | glycerol | water | carbon dioxide | manganese dioxide | pearl ash formula | KMnO_4 | HOCH_2CH(OH)CH_2OH | H_2O | CO_2 | MnO_2 | K_2CO_3 Hill formula | KMnO_4 | C_3H_8O_3 | H_2O | CO_2 | MnO_2 | CK_2O_3 name | potassium permanganate | glycerol | water | carbon dioxide | manganese dioxide | pearl ash IUPAC name | potassium permanganate | glycerol | water | carbon dioxide | dioxomanganese | dipotassium carbonate

Random Queries

CAS number of ammonium hexabromoplatinate vs 4-bromo-1,2-dimethoxybenzene
boiling point of barium fluoride
melting point of 1,1,3-trichlorotrifluoroacetone vs 2,5-bis(chloromethyl)-p-xylene
KOH + MnO2 + O3 = H2O + KMnO4
CAS number of germanium(IV) selenide
electronegativity of sulfur vs aluminum
volume magnetic susceptibility of sulfur
iron(II) cation vs ferrocyanide anion
color of diamond vs haxonite
S + Ba(OH)2 = H2O + BaSO4 + BaS