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HCl + KMnO4 + SnCl2 = H2O + KCl + MnCl + H2SnCl6

Input interpretation

HCl hydrogen chloride + KMnO_4 potassium permanganate + SnCl_2 stannous chloride ⟶ H_2O water + KCl potassium chloride + MnCl + H2SnCl6
HCl hydrogen chloride + KMnO_4 potassium permanganate + SnCl_2 stannous chloride ⟶ H_2O water + KCl potassium chloride + MnCl + H2SnCl6

Balanced equation

Balance the chemical equation algebraically: HCl + KMnO_4 + SnCl_2 ⟶ H_2O + KCl + MnCl + H2SnCl6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KMnO_4 + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 KCl + c_6 MnCl + c_7 H2SnCl6 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, Mn, O and Sn: Cl: | c_1 + 2 c_3 = c_5 + c_6 + 6 c_7 H: | c_1 = 2 c_4 + 2 c_7 K: | c_2 = c_5 Mn: | c_2 = c_6 O: | 4 c_2 = c_4 Sn: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 14 c_2 = 1 c_3 = 3 c_4 = 4 c_5 = 1 c_6 = 1 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 HCl + KMnO_4 + 3 SnCl_2 ⟶ 4 H_2O + KCl + MnCl + 3 H2SnCl6
Balance the chemical equation algebraically: HCl + KMnO_4 + SnCl_2 ⟶ H_2O + KCl + MnCl + H2SnCl6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KMnO_4 + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 KCl + c_6 MnCl + c_7 H2SnCl6 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, Mn, O and Sn: Cl: | c_1 + 2 c_3 = c_5 + c_6 + 6 c_7 H: | c_1 = 2 c_4 + 2 c_7 K: | c_2 = c_5 Mn: | c_2 = c_6 O: | 4 c_2 = c_4 Sn: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 14 c_2 = 1 c_3 = 3 c_4 = 4 c_5 = 1 c_6 = 1 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 HCl + KMnO_4 + 3 SnCl_2 ⟶ 4 H_2O + KCl + MnCl + 3 H2SnCl6

Structures

+ + ⟶ + + MnCl + H2SnCl6
+ + ⟶ + + MnCl + H2SnCl6

Names

hydrogen chloride + potassium permanganate + stannous chloride ⟶ water + potassium chloride + MnCl + H2SnCl6
hydrogen chloride + potassium permanganate + stannous chloride ⟶ water + potassium chloride + MnCl + H2SnCl6

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + KMnO_4 + SnCl_2 ⟶ H_2O + KCl + MnCl + H2SnCl6 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 HCl + KMnO_4 + 3 SnCl_2 ⟶ 4 H_2O + KCl + MnCl + 3 H2SnCl6 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 | 14 | -14 KMnO_4 | 1 | -1 SnCl_2 | 3 | -3 H_2O | 4 | 4 KCl | 1 | 1 MnCl | 1 | 1 H2SnCl6 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 14 | -14 | ([HCl])^(-14) KMnO_4 | 1 | -1 | ([KMnO4])^(-1) SnCl_2 | 3 | -3 | ([SnCl2])^(-3) H_2O | 4 | 4 | ([H2O])^4 KCl | 1 | 1 | [KCl] MnCl | 1 | 1 | [MnCl] H2SnCl6 | 3 | 3 | ([H2SnCl6])^3 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])^(-14) ([KMnO4])^(-1) ([SnCl2])^(-3) ([H2O])^4 [KCl] [MnCl] ([H2SnCl6])^3 = (([H2O])^4 [KCl] [MnCl] ([H2SnCl6])^3)/(([HCl])^14 [KMnO4] ([SnCl2])^3)
Construct the equilibrium constant, K, expression for: HCl + KMnO_4 + SnCl_2 ⟶ H_2O + KCl + MnCl + H2SnCl6 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 HCl + KMnO_4 + 3 SnCl_2 ⟶ 4 H_2O + KCl + MnCl + 3 H2SnCl6 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 | 14 | -14 KMnO_4 | 1 | -1 SnCl_2 | 3 | -3 H_2O | 4 | 4 KCl | 1 | 1 MnCl | 1 | 1 H2SnCl6 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 14 | -14 | ([HCl])^(-14) KMnO_4 | 1 | -1 | ([KMnO4])^(-1) SnCl_2 | 3 | -3 | ([SnCl2])^(-3) H_2O | 4 | 4 | ([H2O])^4 KCl | 1 | 1 | [KCl] MnCl | 1 | 1 | [MnCl] H2SnCl6 | 3 | 3 | ([H2SnCl6])^3 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])^(-14) ([KMnO4])^(-1) ([SnCl2])^(-3) ([H2O])^4 [KCl] [MnCl] ([H2SnCl6])^3 = (([H2O])^4 [KCl] [MnCl] ([H2SnCl6])^3)/(([HCl])^14 [KMnO4] ([SnCl2])^3)

Rate of reaction

Construct the rate of reaction expression for: HCl + KMnO_4 + SnCl_2 ⟶ H_2O + KCl + MnCl + H2SnCl6 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 HCl + KMnO_4 + 3 SnCl_2 ⟶ 4 H_2O + KCl + MnCl + 3 H2SnCl6 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 | 14 | -14 KMnO_4 | 1 | -1 SnCl_2 | 3 | -3 H_2O | 4 | 4 KCl | 1 | 1 MnCl | 1 | 1 H2SnCl6 | 3 | 3 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 | 14 | -14 | -1/14 (Δ[HCl])/(Δt) KMnO_4 | 1 | -1 | -(Δ[KMnO4])/(Δt) SnCl_2 | 3 | -3 | -1/3 (Δ[SnCl2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) MnCl | 1 | 1 | (Δ[MnCl])/(Δt) H2SnCl6 | 3 | 3 | 1/3 (Δ[H2SnCl6])/(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[HCl])/(Δt) = -(Δ[KMnO4])/(Δt) = -1/3 (Δ[SnCl2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = (Δ[MnCl])/(Δt) = 1/3 (Δ[H2SnCl6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + KMnO_4 + SnCl_2 ⟶ H_2O + KCl + MnCl + H2SnCl6 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 HCl + KMnO_4 + 3 SnCl_2 ⟶ 4 H_2O + KCl + MnCl + 3 H2SnCl6 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 | 14 | -14 KMnO_4 | 1 | -1 SnCl_2 | 3 | -3 H_2O | 4 | 4 KCl | 1 | 1 MnCl | 1 | 1 H2SnCl6 | 3 | 3 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 | 14 | -14 | -1/14 (Δ[HCl])/(Δt) KMnO_4 | 1 | -1 | -(Δ[KMnO4])/(Δt) SnCl_2 | 3 | -3 | -1/3 (Δ[SnCl2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) MnCl | 1 | 1 | (Δ[MnCl])/(Δt) H2SnCl6 | 3 | 3 | 1/3 (Δ[H2SnCl6])/(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[HCl])/(Δt) = -(Δ[KMnO4])/(Δt) = -1/3 (Δ[SnCl2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = (Δ[MnCl])/(Δt) = 1/3 (Δ[H2SnCl6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | potassium permanganate | stannous chloride | water | potassium chloride | MnCl | H2SnCl6 formula | HCl | KMnO_4 | SnCl_2 | H_2O | KCl | MnCl | H2SnCl6 Hill formula | ClH | KMnO_4 | Cl_2Sn | H_2O | ClK | ClMn | H2Cl6Sn name | hydrogen chloride | potassium permanganate | stannous chloride | water | potassium chloride | | IUPAC name | hydrogen chloride | potassium permanganate | dichlorotin | water | potassium chloride | |
| hydrogen chloride | potassium permanganate | stannous chloride | water | potassium chloride | MnCl | H2SnCl6 formula | HCl | KMnO_4 | SnCl_2 | H_2O | KCl | MnCl | H2SnCl6 Hill formula | ClH | KMnO_4 | Cl_2Sn | H_2O | ClK | ClMn | H2Cl6Sn name | hydrogen chloride | potassium permanganate | stannous chloride | water | potassium chloride | | IUPAC name | hydrogen chloride | potassium permanganate | dichlorotin | water | potassium chloride | |

Substance properties

| hydrogen chloride | potassium permanganate | stannous chloride | water | potassium chloride | MnCl | H2SnCl6 molar mass | 36.46 g/mol | 158.03 g/mol | 189.6 g/mol | 18.015 g/mol | 74.55 g/mol | 90.39 g/mol | 333.4 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | | melting point | -114.17 °C | 240 °C | 246 °C | 0 °C | 770 °C | | boiling point | -85 °C | | 652 °C | 99.9839 °C | 1420 °C | | density | 0.00149 g/cm^3 (at 25 °C) | 1 g/cm^3 | 3.354 g/cm^3 | 1 g/cm^3 | 1.98 g/cm^3 | | solubility in water | miscible | | | | soluble | | surface tension | | | | 0.0728 N/m | | | dynamic viscosity | | | 7 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | | | odor | | odorless | odorless | odorless | odorless | |
| hydrogen chloride | potassium permanganate | stannous chloride | water | potassium chloride | MnCl | H2SnCl6 molar mass | 36.46 g/mol | 158.03 g/mol | 189.6 g/mol | 18.015 g/mol | 74.55 g/mol | 90.39 g/mol | 333.4 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | | melting point | -114.17 °C | 240 °C | 246 °C | 0 °C | 770 °C | | boiling point | -85 °C | | 652 °C | 99.9839 °C | 1420 °C | | density | 0.00149 g/cm^3 (at 25 °C) | 1 g/cm^3 | 3.354 g/cm^3 | 1 g/cm^3 | 1.98 g/cm^3 | | solubility in water | miscible | | | | soluble | | surface tension | | | | 0.0728 N/m | | | dynamic viscosity | | | 7 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | | | odor | | odorless | odorless | odorless | odorless | |

Units

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