Search

HCl + KMnO4 + KSCN = H2O + CO2 + SO2 + KCl + NO + MnCl2

Input interpretation

HCl hydrogen chloride + KMnO_4 potassium permanganate + KSCN potassium thiocyanate ⟶ H_2O water + CO_2 carbon dioxide + SO_2 sulfur dioxide + KCl potassium chloride + NO nitric oxide + MnCl_2 manganese(II) chloride
HCl hydrogen chloride + KMnO_4 potassium permanganate + KSCN potassium thiocyanate ⟶ H_2O water + CO_2 carbon dioxide + SO_2 sulfur dioxide + KCl potassium chloride + NO nitric oxide + MnCl_2 manganese(II) chloride

Balanced equation

Balance the chemical equation algebraically: HCl + KMnO_4 + KSCN ⟶ H_2O + CO_2 + SO_2 + KCl + NO + MnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KMnO_4 + c_3 KSCN ⟶ c_4 H_2O + c_5 CO_2 + c_6 SO_2 + c_7 KCl + c_8 NO + c_9 MnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, Mn, O, C, N and S: Cl: | c_1 = c_7 + 2 c_9 H: | c_1 = 2 c_4 K: | c_2 + c_3 = c_7 Mn: | c_2 = c_9 O: | 4 c_2 = c_4 + 2 c_5 + 2 c_6 + c_8 C: | c_3 = c_5 N: | c_3 = c_8 S: | c_3 = c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 38/5 c_2 = 11/5 c_3 = 1 c_4 = 19/5 c_5 = 1 c_6 = 1 c_7 = 16/5 c_8 = 1 c_9 = 11/5 Multiply by the least common denominator, 5, to eliminate fractional coefficients: c_1 = 38 c_2 = 11 c_3 = 5 c_4 = 19 c_5 = 5 c_6 = 5 c_7 = 16 c_8 = 5 c_9 = 11 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 38 HCl + 11 KMnO_4 + 5 KSCN ⟶ 19 H_2O + 5 CO_2 + 5 SO_2 + 16 KCl + 5 NO + 11 MnCl_2
Balance the chemical equation algebraically: HCl + KMnO_4 + KSCN ⟶ H_2O + CO_2 + SO_2 + KCl + NO + MnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KMnO_4 + c_3 KSCN ⟶ c_4 H_2O + c_5 CO_2 + c_6 SO_2 + c_7 KCl + c_8 NO + c_9 MnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, Mn, O, C, N and S: Cl: | c_1 = c_7 + 2 c_9 H: | c_1 = 2 c_4 K: | c_2 + c_3 = c_7 Mn: | c_2 = c_9 O: | 4 c_2 = c_4 + 2 c_5 + 2 c_6 + c_8 C: | c_3 = c_5 N: | c_3 = c_8 S: | c_3 = c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 38/5 c_2 = 11/5 c_3 = 1 c_4 = 19/5 c_5 = 1 c_6 = 1 c_7 = 16/5 c_8 = 1 c_9 = 11/5 Multiply by the least common denominator, 5, to eliminate fractional coefficients: c_1 = 38 c_2 = 11 c_3 = 5 c_4 = 19 c_5 = 5 c_6 = 5 c_7 = 16 c_8 = 5 c_9 = 11 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 38 HCl + 11 KMnO_4 + 5 KSCN ⟶ 19 H_2O + 5 CO_2 + 5 SO_2 + 16 KCl + 5 NO + 11 MnCl_2

Names

hydrogen chloride + potassium permanganate + potassium thiocyanate ⟶ water + carbon dioxide + sulfur dioxide + potassium chloride + nitric oxide + manganese(II) chloride
hydrogen chloride + potassium permanganate + potassium thiocyanate ⟶ water + carbon dioxide + sulfur dioxide + potassium chloride + nitric oxide + manganese(II) chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + KMnO_4 + KSCN ⟶ H_2O + CO_2 + SO_2 + KCl + NO + MnCl_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: 38 HCl + 11 KMnO_4 + 5 KSCN ⟶ 19 H_2O + 5 CO_2 + 5 SO_2 + 16 KCl + 5 NO + 11 MnCl_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 HCl | 38 | -38 KMnO_4 | 11 | -11 KSCN | 5 | -5 H_2O | 19 | 19 CO_2 | 5 | 5 SO_2 | 5 | 5 KCl | 16 | 16 NO | 5 | 5 MnCl_2 | 11 | 11 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 38 | -38 | ([HCl])^(-38) KMnO_4 | 11 | -11 | ([KMnO4])^(-11) KSCN | 5 | -5 | ([KSCN])^(-5) H_2O | 19 | 19 | ([H2O])^19 CO_2 | 5 | 5 | ([CO2])^5 SO_2 | 5 | 5 | ([SO2])^5 KCl | 16 | 16 | ([KCl])^16 NO | 5 | 5 | ([NO])^5 MnCl_2 | 11 | 11 | ([MnCl2])^11 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])^(-38) ([KMnO4])^(-11) ([KSCN])^(-5) ([H2O])^19 ([CO2])^5 ([SO2])^5 ([KCl])^16 ([NO])^5 ([MnCl2])^11 = (([H2O])^19 ([CO2])^5 ([SO2])^5 ([KCl])^16 ([NO])^5 ([MnCl2])^11)/(([HCl])^38 ([KMnO4])^11 ([KSCN])^5)
Construct the equilibrium constant, K, expression for: HCl + KMnO_4 + KSCN ⟶ H_2O + CO_2 + SO_2 + KCl + NO + MnCl_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: 38 HCl + 11 KMnO_4 + 5 KSCN ⟶ 19 H_2O + 5 CO_2 + 5 SO_2 + 16 KCl + 5 NO + 11 MnCl_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 HCl | 38 | -38 KMnO_4 | 11 | -11 KSCN | 5 | -5 H_2O | 19 | 19 CO_2 | 5 | 5 SO_2 | 5 | 5 KCl | 16 | 16 NO | 5 | 5 MnCl_2 | 11 | 11 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 38 | -38 | ([HCl])^(-38) KMnO_4 | 11 | -11 | ([KMnO4])^(-11) KSCN | 5 | -5 | ([KSCN])^(-5) H_2O | 19 | 19 | ([H2O])^19 CO_2 | 5 | 5 | ([CO2])^5 SO_2 | 5 | 5 | ([SO2])^5 KCl | 16 | 16 | ([KCl])^16 NO | 5 | 5 | ([NO])^5 MnCl_2 | 11 | 11 | ([MnCl2])^11 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])^(-38) ([KMnO4])^(-11) ([KSCN])^(-5) ([H2O])^19 ([CO2])^5 ([SO2])^5 ([KCl])^16 ([NO])^5 ([MnCl2])^11 = (([H2O])^19 ([CO2])^5 ([SO2])^5 ([KCl])^16 ([NO])^5 ([MnCl2])^11)/(([HCl])^38 ([KMnO4])^11 ([KSCN])^5)

Rate of reaction

Construct the rate of reaction expression for: HCl + KMnO_4 + KSCN ⟶ H_2O + CO_2 + SO_2 + KCl + NO + MnCl_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: 38 HCl + 11 KMnO_4 + 5 KSCN ⟶ 19 H_2O + 5 CO_2 + 5 SO_2 + 16 KCl + 5 NO + 11 MnCl_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 HCl | 38 | -38 KMnO_4 | 11 | -11 KSCN | 5 | -5 H_2O | 19 | 19 CO_2 | 5 | 5 SO_2 | 5 | 5 KCl | 16 | 16 NO | 5 | 5 MnCl_2 | 11 | 11 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 | 38 | -38 | -1/38 (Δ[HCl])/(Δt) KMnO_4 | 11 | -11 | -1/11 (Δ[KMnO4])/(Δt) KSCN | 5 | -5 | -1/5 (Δ[KSCN])/(Δt) H_2O | 19 | 19 | 1/19 (Δ[H2O])/(Δt) CO_2 | 5 | 5 | 1/5 (Δ[CO2])/(Δt) SO_2 | 5 | 5 | 1/5 (Δ[SO2])/(Δt) KCl | 16 | 16 | 1/16 (Δ[KCl])/(Δt) NO | 5 | 5 | 1/5 (Δ[NO])/(Δt) MnCl_2 | 11 | 11 | 1/11 (Δ[MnCl2])/(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 = -1/38 (Δ[HCl])/(Δt) = -1/11 (Δ[KMnO4])/(Δt) = -1/5 (Δ[KSCN])/(Δt) = 1/19 (Δ[H2O])/(Δt) = 1/5 (Δ[CO2])/(Δt) = 1/5 (Δ[SO2])/(Δt) = 1/16 (Δ[KCl])/(Δt) = 1/5 (Δ[NO])/(Δt) = 1/11 (Δ[MnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + KMnO_4 + KSCN ⟶ H_2O + CO_2 + SO_2 + KCl + NO + MnCl_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: 38 HCl + 11 KMnO_4 + 5 KSCN ⟶ 19 H_2O + 5 CO_2 + 5 SO_2 + 16 KCl + 5 NO + 11 MnCl_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 HCl | 38 | -38 KMnO_4 | 11 | -11 KSCN | 5 | -5 H_2O | 19 | 19 CO_2 | 5 | 5 SO_2 | 5 | 5 KCl | 16 | 16 NO | 5 | 5 MnCl_2 | 11 | 11 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 | 38 | -38 | -1/38 (Δ[HCl])/(Δt) KMnO_4 | 11 | -11 | -1/11 (Δ[KMnO4])/(Δt) KSCN | 5 | -5 | -1/5 (Δ[KSCN])/(Δt) H_2O | 19 | 19 | 1/19 (Δ[H2O])/(Δt) CO_2 | 5 | 5 | 1/5 (Δ[CO2])/(Δt) SO_2 | 5 | 5 | 1/5 (Δ[SO2])/(Δt) KCl | 16 | 16 | 1/16 (Δ[KCl])/(Δt) NO | 5 | 5 | 1/5 (Δ[NO])/(Δt) MnCl_2 | 11 | 11 | 1/11 (Δ[MnCl2])/(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 = -1/38 (Δ[HCl])/(Δt) = -1/11 (Δ[KMnO4])/(Δt) = -1/5 (Δ[KSCN])/(Δt) = 1/19 (Δ[H2O])/(Δt) = 1/5 (Δ[CO2])/(Δt) = 1/5 (Δ[SO2])/(Δt) = 1/16 (Δ[KCl])/(Δt) = 1/5 (Δ[NO])/(Δt) = 1/11 (Δ[MnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | potassium permanganate | potassium thiocyanate | water | carbon dioxide | sulfur dioxide | potassium chloride | nitric oxide | manganese(II) chloride formula | HCl | KMnO_4 | KSCN | H_2O | CO_2 | SO_2 | KCl | NO | MnCl_2 Hill formula | ClH | KMnO_4 | CKNS | H_2O | CO_2 | O_2S | ClK | NO | Cl_2Mn name | hydrogen chloride | potassium permanganate | potassium thiocyanate | water | carbon dioxide | sulfur dioxide | potassium chloride | nitric oxide | manganese(II) chloride IUPAC name | hydrogen chloride | potassium permanganate | potassium isothiocyanate | water | carbon dioxide | sulfur dioxide | potassium chloride | nitric oxide | dichloromanganese
| hydrogen chloride | potassium permanganate | potassium thiocyanate | water | carbon dioxide | sulfur dioxide | potassium chloride | nitric oxide | manganese(II) chloride formula | HCl | KMnO_4 | KSCN | H_2O | CO_2 | SO_2 | KCl | NO | MnCl_2 Hill formula | ClH | KMnO_4 | CKNS | H_2O | CO_2 | O_2S | ClK | NO | Cl_2Mn name | hydrogen chloride | potassium permanganate | potassium thiocyanate | water | carbon dioxide | sulfur dioxide | potassium chloride | nitric oxide | manganese(II) chloride IUPAC name | hydrogen chloride | potassium permanganate | potassium isothiocyanate | water | carbon dioxide | sulfur dioxide | potassium chloride | nitric oxide | dichloromanganese

Random Queries

CAS number of dichlorine hexoxide
common compound names of gadolinium vs holmium
IUPAC name of aluminum cesium sulfate dodecahydrate vs tetrasodium ethylenediaminetetraacetate
stable isotopes of argon
2O = Cu + FeSO4
formula of vanadium(III) cation vs vanadium(I) cation
chemical types of sodium fluoride vs indium(III) fluoride
IUPAC name of beryllium oxide vs hexaamminenickel(II) bromide
barium vs cesium vs sulfur
isomeric SMILES identifier of grignard reagents