Search

HCl + KMnO4 = H2O + Cl2 + KClMnCl2

Input interpretation

HCl hydrogen chloride + KMnO_4 potassium permanganate ⟶ H_2O water + Cl_2 chlorine + KClMnCl2
HCl hydrogen chloride + KMnO_4 potassium permanganate ⟶ H_2O water + Cl_2 chlorine + KClMnCl2

Balanced equation

Balance the chemical equation algebraically: HCl + KMnO_4 ⟶ H_2O + Cl_2 + KClMnCl2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KMnO_4 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 KClMnCl2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, Mn and O: Cl: | c_1 = 2 c_4 + 3 c_5 H: | c_1 = 2 c_3 K: | c_2 = c_5 Mn: | c_2 = c_5 O: | 4 c_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 = 8 c_2 = 1 c_3 = 4 c_4 = 5/2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 16 c_2 = 2 c_3 = 8 c_4 = 5 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 16 HCl + 2 KMnO_4 ⟶ 8 H_2O + 5 Cl_2 + 2 KClMnCl2
Balance the chemical equation algebraically: HCl + KMnO_4 ⟶ H_2O + Cl_2 + KClMnCl2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KMnO_4 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 KClMnCl2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, Mn and O: Cl: | c_1 = 2 c_4 + 3 c_5 H: | c_1 = 2 c_3 K: | c_2 = c_5 Mn: | c_2 = c_5 O: | 4 c_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 = 8 c_2 = 1 c_3 = 4 c_4 = 5/2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 16 c_2 = 2 c_3 = 8 c_4 = 5 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 16 HCl + 2 KMnO_4 ⟶ 8 H_2O + 5 Cl_2 + 2 KClMnCl2

Structures

+ ⟶ + + KClMnCl2
+ ⟶ + + KClMnCl2

Names

hydrogen chloride + potassium permanganate ⟶ water + chlorine + KClMnCl2
hydrogen chloride + potassium permanganate ⟶ water + chlorine + KClMnCl2

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + KMnO_4 ⟶ H_2O + Cl_2 + KClMnCl2 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: 16 HCl + 2 KMnO_4 ⟶ 8 H_2O + 5 Cl_2 + 2 KClMnCl2 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 HCl | 16 | -16 KMnO_4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 KClMnCl2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 16 | -16 | ([HCl])^(-16) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) H_2O | 8 | 8 | ([H2O])^8 Cl_2 | 5 | 5 | ([Cl2])^5 KClMnCl2 | 2 | 2 | ([KClMnCl2])^2 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 = ([HCl])^(-16) ([KMnO4])^(-2) ([H2O])^8 ([Cl2])^5 ([KClMnCl2])^2 = (([H2O])^8 ([Cl2])^5 ([KClMnCl2])^2)/(([HCl])^16 ([KMnO4])^2)
Construct the equilibrium constant, K, expression for: HCl + KMnO_4 ⟶ H_2O + Cl_2 + KClMnCl2 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: 16 HCl + 2 KMnO_4 ⟶ 8 H_2O + 5 Cl_2 + 2 KClMnCl2 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 HCl | 16 | -16 KMnO_4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 KClMnCl2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 16 | -16 | ([HCl])^(-16) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) H_2O | 8 | 8 | ([H2O])^8 Cl_2 | 5 | 5 | ([Cl2])^5 KClMnCl2 | 2 | 2 | ([KClMnCl2])^2 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 = ([HCl])^(-16) ([KMnO4])^(-2) ([H2O])^8 ([Cl2])^5 ([KClMnCl2])^2 = (([H2O])^8 ([Cl2])^5 ([KClMnCl2])^2)/(([HCl])^16 ([KMnO4])^2)

Rate of reaction

Construct the rate of reaction expression for: HCl + KMnO_4 ⟶ H_2O + Cl_2 + KClMnCl2 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: 16 HCl + 2 KMnO_4 ⟶ 8 H_2O + 5 Cl_2 + 2 KClMnCl2 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 HCl | 16 | -16 KMnO_4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 KClMnCl2 | 2 | 2 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 HCl | 16 | -16 | -1/16 (Δ[HCl])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) Cl_2 | 5 | 5 | 1/5 (Δ[Cl2])/(Δt) KClMnCl2 | 2 | 2 | 1/2 (Δ[KClMnCl2])/(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 = -1/16 (Δ[HCl])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/5 (Δ[Cl2])/(Δt) = 1/2 (Δ[KClMnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + KMnO_4 ⟶ H_2O + Cl_2 + KClMnCl2 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: 16 HCl + 2 KMnO_4 ⟶ 8 H_2O + 5 Cl_2 + 2 KClMnCl2 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 HCl | 16 | -16 KMnO_4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 KClMnCl2 | 2 | 2 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 HCl | 16 | -16 | -1/16 (Δ[HCl])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) Cl_2 | 5 | 5 | 1/5 (Δ[Cl2])/(Δt) KClMnCl2 | 2 | 2 | 1/2 (Δ[KClMnCl2])/(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 = -1/16 (Δ[HCl])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/5 (Δ[Cl2])/(Δt) = 1/2 (Δ[KClMnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | potassium permanganate | water | chlorine | KClMnCl2 formula | HCl | KMnO_4 | H_2O | Cl_2 | KClMnCl2 Hill formula | ClH | KMnO_4 | H_2O | Cl_2 | Cl3KMn name | hydrogen chloride | potassium permanganate | water | chlorine | IUPAC name | hydrogen chloride | potassium permanganate | water | molecular chlorine |
| hydrogen chloride | potassium permanganate | water | chlorine | KClMnCl2 formula | HCl | KMnO_4 | H_2O | Cl_2 | KClMnCl2 Hill formula | ClH | KMnO_4 | H_2O | Cl_2 | Cl3KMn name | hydrogen chloride | potassium permanganate | water | chlorine | IUPAC name | hydrogen chloride | potassium permanganate | water | molecular chlorine |

Substance properties

| hydrogen chloride | potassium permanganate | water | chlorine | KClMnCl2 molar mass | 36.46 g/mol | 158.03 g/mol | 18.015 g/mol | 70.9 g/mol | 200.4 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | -114.17 °C | 240 °C | 0 °C | -101 °C | boiling point | -85 °C | | 99.9839 °C | -34 °C | density | 0.00149 g/cm^3 (at 25 °C) | 1 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | solubility in water | miscible | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | odorless | odorless | |
| hydrogen chloride | potassium permanganate | water | chlorine | KClMnCl2 molar mass | 36.46 g/mol | 158.03 g/mol | 18.015 g/mol | 70.9 g/mol | 200.4 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | -114.17 °C | 240 °C | 0 °C | -101 °C | boiling point | -85 °C | | 99.9839 °C | -34 °C | density | 0.00149 g/cm^3 (at 25 °C) | 1 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | solubility in water | miscible | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | odorless | odorless | |

Units

Random Queries

Hill formula string of trichlorofluoromethane
antimony vs nitrogen vs bismuth
molar heat of fusion of potassium iodide
net ionic charge of chromium(II) cation vs scandium(III) cation
molar mass of antimony pentafluoride
atomic mass of arsenic vs hydrogen
edge rules of hexamethylmelamine
CAS number of dichlorotetrakis(pyridine)iron
Hill formula string of alkenes
most common oxidation states of gold