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H2O + HClO3 + MnS = H2SO4 + HCl + HMnO4

Input interpretation

H_2O water + HClO3 + MnS manganese sulfide ⟶ H_2SO_4 sulfuric acid + HCl hydrogen chloride + HMnO4
H_2O water + HClO3 + MnS manganese sulfide ⟶ H_2SO_4 sulfuric acid + HCl hydrogen chloride + HMnO4

Balanced equation

Balance the chemical equation algebraically: H_2O + HClO3 + MnS ⟶ H_2SO_4 + HCl + HMnO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HClO3 + c_3 MnS ⟶ c_4 H_2SO_4 + c_5 HCl + c_6 HMnO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Mn and S: H: | 2 c_1 + c_2 = 2 c_4 + c_5 + c_6 O: | c_1 + 3 c_2 = 4 c_4 + 4 c_6 Cl: | c_2 = c_5 Mn: | c_3 = c_6 S: | c_3 = c_4 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 = 3/2 c_2 = 13/6 c_3 = 1 c_4 = 1 c_5 = 13/6 c_6 = 1 Multiply by the least common denominator, 6, to eliminate fractional coefficients: c_1 = 9 c_2 = 13 c_3 = 6 c_4 = 6 c_5 = 13 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: |   | 9 H_2O + 13 HClO3 + 6 MnS ⟶ 6 H_2SO_4 + 13 HCl + 6 HMnO4
Balance the chemical equation algebraically: H_2O + HClO3 + MnS ⟶ H_2SO_4 + HCl + HMnO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HClO3 + c_3 MnS ⟶ c_4 H_2SO_4 + c_5 HCl + c_6 HMnO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Mn and S: H: | 2 c_1 + c_2 = 2 c_4 + c_5 + c_6 O: | c_1 + 3 c_2 = 4 c_4 + 4 c_6 Cl: | c_2 = c_5 Mn: | c_3 = c_6 S: | c_3 = c_4 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 = 3/2 c_2 = 13/6 c_3 = 1 c_4 = 1 c_5 = 13/6 c_6 = 1 Multiply by the least common denominator, 6, to eliminate fractional coefficients: c_1 = 9 c_2 = 13 c_3 = 6 c_4 = 6 c_5 = 13 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 H_2O + 13 HClO3 + 6 MnS ⟶ 6 H_2SO_4 + 13 HCl + 6 HMnO4

Structures

 + HClO3 + ⟶ + + HMnO4
+ HClO3 + ⟶ + + HMnO4

Names

water + HClO3 + manganese sulfide ⟶ sulfuric acid + hydrogen chloride + HMnO4
water + HClO3 + manganese sulfide ⟶ sulfuric acid + hydrogen chloride + HMnO4

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + HClO3 + MnS ⟶ H_2SO_4 + HCl + HMnO4 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: 9 H_2O + 13 HClO3 + 6 MnS ⟶ 6 H_2SO_4 + 13 HCl + 6 HMnO4 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 H_2O | 9 | -9 HClO3 | 13 | -13 MnS | 6 | -6 H_2SO_4 | 6 | 6 HCl | 13 | 13 HMnO4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 9 | -9 | ([H2O])^(-9) HClO3 | 13 | -13 | ([HClO3])^(-13) MnS | 6 | -6 | ([MnS])^(-6) H_2SO_4 | 6 | 6 | ([H2SO4])^6 HCl | 13 | 13 | ([HCl])^13 HMnO4 | 6 | 6 | ([HMnO4])^6 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 = ([H2O])^(-9) ([HClO3])^(-13) ([MnS])^(-6) ([H2SO4])^6 ([HCl])^13 ([HMnO4])^6 = (([H2SO4])^6 ([HCl])^13 ([HMnO4])^6)/(([H2O])^9 ([HClO3])^13 ([MnS])^6)
Construct the equilibrium constant, K, expression for: H_2O + HClO3 + MnS ⟶ H_2SO_4 + HCl + HMnO4 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: 9 H_2O + 13 HClO3 + 6 MnS ⟶ 6 H_2SO_4 + 13 HCl + 6 HMnO4 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 H_2O | 9 | -9 HClO3 | 13 | -13 MnS | 6 | -6 H_2SO_4 | 6 | 6 HCl | 13 | 13 HMnO4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 9 | -9 | ([H2O])^(-9) HClO3 | 13 | -13 | ([HClO3])^(-13) MnS | 6 | -6 | ([MnS])^(-6) H_2SO_4 | 6 | 6 | ([H2SO4])^6 HCl | 13 | 13 | ([HCl])^13 HMnO4 | 6 | 6 | ([HMnO4])^6 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 = ([H2O])^(-9) ([HClO3])^(-13) ([MnS])^(-6) ([H2SO4])^6 ([HCl])^13 ([HMnO4])^6 = (([H2SO4])^6 ([HCl])^13 ([HMnO4])^6)/(([H2O])^9 ([HClO3])^13 ([MnS])^6)

Rate of reaction

Construct the rate of reaction expression for: H_2O + HClO3 + MnS ⟶ H_2SO_4 + HCl + HMnO4 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: 9 H_2O + 13 HClO3 + 6 MnS ⟶ 6 H_2SO_4 + 13 HCl + 6 HMnO4 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 H_2O | 9 | -9 HClO3 | 13 | -13 MnS | 6 | -6 H_2SO_4 | 6 | 6 HCl | 13 | 13 HMnO4 | 6 | 6 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 H_2O | 9 | -9 | -1/9 (Δ[H2O])/(Δt) HClO3 | 13 | -13 | -1/13 (Δ[HClO3])/(Δt) MnS | 6 | -6 | -1/6 (Δ[MnS])/(Δt) H_2SO_4 | 6 | 6 | 1/6 (Δ[H2SO4])/(Δt) HCl | 13 | 13 | 1/13 (Δ[HCl])/(Δt) HMnO4 | 6 | 6 | 1/6 (Δ[HMnO4])/(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 = -1/9 (Δ[H2O])/(Δt) = -1/13 (Δ[HClO3])/(Δt) = -1/6 (Δ[MnS])/(Δt) = 1/6 (Δ[H2SO4])/(Δt) = 1/13 (Δ[HCl])/(Δt) = 1/6 (Δ[HMnO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + HClO3 + MnS ⟶ H_2SO_4 + HCl + HMnO4 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: 9 H_2O + 13 HClO3 + 6 MnS ⟶ 6 H_2SO_4 + 13 HCl + 6 HMnO4 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 H_2O | 9 | -9 HClO3 | 13 | -13 MnS | 6 | -6 H_2SO_4 | 6 | 6 HCl | 13 | 13 HMnO4 | 6 | 6 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 H_2O | 9 | -9 | -1/9 (Δ[H2O])/(Δt) HClO3 | 13 | -13 | -1/13 (Δ[HClO3])/(Δt) MnS | 6 | -6 | -1/6 (Δ[MnS])/(Δt) H_2SO_4 | 6 | 6 | 1/6 (Δ[H2SO4])/(Δt) HCl | 13 | 13 | 1/13 (Δ[HCl])/(Δt) HMnO4 | 6 | 6 | 1/6 (Δ[HMnO4])/(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 = -1/9 (Δ[H2O])/(Δt) = -1/13 (Δ[HClO3])/(Δt) = -1/6 (Δ[MnS])/(Δt) = 1/6 (Δ[H2SO4])/(Δt) = 1/13 (Δ[HCl])/(Δt) = 1/6 (Δ[HMnO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | water | HClO3 | manganese sulfide | sulfuric acid | hydrogen chloride | HMnO4 formula | H_2O | HClO3 | MnS | H_2SO_4 | HCl | HMnO4 Hill formula | H_2O | HClO3 | MnS | H_2O_4S | ClH | HMnO4 name | water | | manganese sulfide | sulfuric acid | hydrogen chloride |
| water | HClO3 | manganese sulfide | sulfuric acid | hydrogen chloride | HMnO4 formula | H_2O | HClO3 | MnS | H_2SO_4 | HCl | HMnO4 Hill formula | H_2O | HClO3 | MnS | H_2O_4S | ClH | HMnO4 name | water | | manganese sulfide | sulfuric acid | hydrogen chloride |

Substance properties

 | water | HClO3 | manganese sulfide | sulfuric acid | hydrogen chloride | HMnO4 molar mass | 18.015 g/mol | 84.45 g/mol | 87 g/mol | 98.07 g/mol | 36.46 g/mol | 119.94 g/mol phase | liquid (at STP) | | solid (at STP) | liquid (at STP) | gas (at STP) |  melting point | 0 °C | | 1141 °C | 10.371 °C | -114.17 °C |  boiling point | 99.9839 °C | | | 279.6 °C | -85 °C |  density | 1 g/cm^3 | | 3.3 g/cm^3 | 1.8305 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) |  solubility in water | | | | very soluble | miscible |  surface tension | 0.0728 N/m | | | 0.0735 N/m | |  dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 2.64×10^-5 Pa s (at 1250 °C) | 0.021 Pa s (at 25 °C) | |  odor | odorless | | | odorless | |
| water | HClO3 | manganese sulfide | sulfuric acid | hydrogen chloride | HMnO4 molar mass | 18.015 g/mol | 84.45 g/mol | 87 g/mol | 98.07 g/mol | 36.46 g/mol | 119.94 g/mol phase | liquid (at STP) | | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | 0 °C | | 1141 °C | 10.371 °C | -114.17 °C | boiling point | 99.9839 °C | | | 279.6 °C | -85 °C | density | 1 g/cm^3 | | 3.3 g/cm^3 | 1.8305 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | solubility in water | | | | very soluble | miscible | surface tension | 0.0728 N/m | | | 0.0735 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 2.64×10^-5 Pa s (at 1250 °C) | 0.021 Pa s (at 25 °C) | | odor | odorless | | | odorless | |

Units