Search

KMnO4 + C3H8O3 = H2O + CO2 + K2CO3 + Mn2O3

Input interpretation

KMnO_4 potassium permanganate + HOCH_2CH(OH)CH_2OH glycerol ⟶ H_2O water + CO_2 carbon dioxide + K_2CO_3 pearl ash + Mn_2O_3 manganese(III) oxide
KMnO_4 potassium permanganate + HOCH_2CH(OH)CH_2OH glycerol ⟶ H_2O water + CO_2 carbon dioxide + K_2CO_3 pearl ash + Mn_2O_3 manganese(III) oxide

Balanced equation

Balance the chemical equation algebraically: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + K_2CO_3 + Mn_2O_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 K_2CO_3 + c_6 Mn_2O_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_5 Mn: | c_1 = 2 c_6 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 3 c_5 + 3 c_6 C: | 3 c_2 = c_4 + c_5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 7/2 c_2 = 1 c_3 = 4 c_4 = 5/4 c_5 = 7/4 c_6 = 7/4 Multiply by the least common denominator, 4, to eliminate fractional coefficients: c_1 = 14 c_2 = 4 c_3 = 16 c_4 = 5 c_5 = 7 c_6 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 KMnO_4 + 4 HOCH_2CH(OH)CH_2OH ⟶ 16 H_2O + 5 CO_2 + 7 K_2CO_3 + 7 Mn_2O_3
Balance the chemical equation algebraically: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + K_2CO_3 + Mn_2O_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 K_2CO_3 + c_6 Mn_2O_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_5 Mn: | c_1 = 2 c_6 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 3 c_5 + 3 c_6 C: | 3 c_2 = c_4 + c_5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 7/2 c_2 = 1 c_3 = 4 c_4 = 5/4 c_5 = 7/4 c_6 = 7/4 Multiply by the least common denominator, 4, to eliminate fractional coefficients: c_1 = 14 c_2 = 4 c_3 = 16 c_4 = 5 c_5 = 7 c_6 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 KMnO_4 + 4 HOCH_2CH(OH)CH_2OH ⟶ 16 H_2O + 5 CO_2 + 7 K_2CO_3 + 7 Mn_2O_3

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

potassium permanganate + glycerol ⟶ water + carbon dioxide + pearl ash + manganese(III) oxide
potassium permanganate + glycerol ⟶ water + carbon dioxide + pearl ash + manganese(III) oxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + K_2CO_3 + Mn_2O_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 + 4 HOCH_2CH(OH)CH_2OH ⟶ 16 H_2O + 5 CO_2 + 7 K_2CO_3 + 7 Mn_2O_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 | 4 | -4 H_2O | 16 | 16 CO_2 | 5 | 5 K_2CO_3 | 7 | 7 Mn_2O_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 | 4 | -4 | ([HOCH2CH(OH)CH2OH])^(-4) H_2O | 16 | 16 | ([H2O])^16 CO_2 | 5 | 5 | ([CO2])^5 K_2CO_3 | 7 | 7 | ([K2CO3])^7 Mn_2O_3 | 7 | 7 | ([Mn2O3])^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])^(-4) ([H2O])^16 ([CO2])^5 ([K2CO3])^7 ([Mn2O3])^7 = (([H2O])^16 ([CO2])^5 ([K2CO3])^7 ([Mn2O3])^7)/(([KMnO4])^14 ([HOCH2CH(OH)CH2OH])^4)
Construct the equilibrium constant, K, expression for: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + K_2CO_3 + Mn_2O_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 + 4 HOCH_2CH(OH)CH_2OH ⟶ 16 H_2O + 5 CO_2 + 7 K_2CO_3 + 7 Mn_2O_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 | 4 | -4 H_2O | 16 | 16 CO_2 | 5 | 5 K_2CO_3 | 7 | 7 Mn_2O_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 | 4 | -4 | ([HOCH2CH(OH)CH2OH])^(-4) H_2O | 16 | 16 | ([H2O])^16 CO_2 | 5 | 5 | ([CO2])^5 K_2CO_3 | 7 | 7 | ([K2CO3])^7 Mn_2O_3 | 7 | 7 | ([Mn2O3])^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])^(-4) ([H2O])^16 ([CO2])^5 ([K2CO3])^7 ([Mn2O3])^7 = (([H2O])^16 ([CO2])^5 ([K2CO3])^7 ([Mn2O3])^7)/(([KMnO4])^14 ([HOCH2CH(OH)CH2OH])^4)

Rate of reaction

Construct the rate of reaction expression for: KMnO_4 + HOCH_2CH(OH)CH_2OH ⟶ H_2O + CO_2 + K_2CO_3 + Mn_2O_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 + 4 HOCH_2CH(OH)CH_2OH ⟶ 16 H_2O + 5 CO_2 + 7 K_2CO_3 + 7 Mn_2O_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 | 4 | -4 H_2O | 16 | 16 CO_2 | 5 | 5 K_2CO_3 | 7 | 7 Mn_2O_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 | 4 | -4 | -1/4 (Δ[HOCH2CH(OH)CH2OH])/(Δt) H_2O | 16 | 16 | 1/16 (Δ[H2O])/(Δt) CO_2 | 5 | 5 | 1/5 (Δ[CO2])/(Δt) K_2CO_3 | 7 | 7 | 1/7 (Δ[K2CO3])/(Δt) Mn_2O_3 | 7 | 7 | 1/7 (Δ[Mn2O3])/(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) = -1/4 (Δ[HOCH2CH(OH)CH2OH])/(Δt) = 1/16 (Δ[H2O])/(Δt) = 1/5 (Δ[CO2])/(Δt) = 1/7 (Δ[K2CO3])/(Δt) = 1/7 (Δ[Mn2O3])/(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 + K_2CO_3 + Mn_2O_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 + 4 HOCH_2CH(OH)CH_2OH ⟶ 16 H_2O + 5 CO_2 + 7 K_2CO_3 + 7 Mn_2O_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 | 4 | -4 H_2O | 16 | 16 CO_2 | 5 | 5 K_2CO_3 | 7 | 7 Mn_2O_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 | 4 | -4 | -1/4 (Δ[HOCH2CH(OH)CH2OH])/(Δt) H_2O | 16 | 16 | 1/16 (Δ[H2O])/(Δt) CO_2 | 5 | 5 | 1/5 (Δ[CO2])/(Δt) K_2CO_3 | 7 | 7 | 1/7 (Δ[K2CO3])/(Δt) Mn_2O_3 | 7 | 7 | 1/7 (Δ[Mn2O3])/(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) = -1/4 (Δ[HOCH2CH(OH)CH2OH])/(Δt) = 1/16 (Δ[H2O])/(Δt) = 1/5 (Δ[CO2])/(Δt) = 1/7 (Δ[K2CO3])/(Δt) = 1/7 (Δ[Mn2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium permanganate | glycerol | water | carbon dioxide | pearl ash | manganese(III) oxide formula | KMnO_4 | HOCH_2CH(OH)CH_2OH | H_2O | CO_2 | K_2CO_3 | Mn_2O_3 Hill formula | KMnO_4 | C_3H_8O_3 | H_2O | CO_2 | CK_2O_3 | Mn_2O_3 name | potassium permanganate | glycerol | water | carbon dioxide | pearl ash | manganese(III) oxide IUPAC name | potassium permanganate | glycerol | water | carbon dioxide | dipotassium carbonate | oxo-(oxomanganiooxy)manganese
| potassium permanganate | glycerol | water | carbon dioxide | pearl ash | manganese(III) oxide formula | KMnO_4 | HOCH_2CH(OH)CH_2OH | H_2O | CO_2 | K_2CO_3 | Mn_2O_3 Hill formula | KMnO_4 | C_3H_8O_3 | H_2O | CO_2 | CK_2O_3 | Mn_2O_3 name | potassium permanganate | glycerol | water | carbon dioxide | pearl ash | manganese(III) oxide IUPAC name | potassium permanganate | glycerol | water | carbon dioxide | dipotassium carbonate | oxo-(oxomanganiooxy)manganese

Random Queries

net ionic charge of calcium chloride
electrical type of silver vs copper
density of sodium aluminate
freezing point of iodic acid vs trifluoroacetic acid
structure diagram of nitride anion vs acetate anion
molar mass of neodymium(III) sulfide vs nitronium tetrafluoroborate
melting point of chlorine trifluoride vs hydrogen
flash point of 1-bromo-3-methyl-2-butene
molar mass of sulfur dioxide
Aufbau diagram of synthetic elements