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H2O + MnS = H2S + Mn(OH)2

Input interpretation

H_2O water + MnS manganese sulfide ⟶ H_2S hydrogen sulfide + Mn(OH)_2 manganese hydroxide
H_2O water + MnS manganese sulfide ⟶ H_2S hydrogen sulfide + Mn(OH)_2 manganese hydroxide

Balanced equation

Balance the chemical equation algebraically: H_2O + MnS ⟶ H_2S + Mn(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 MnS ⟶ c_3 H_2S + c_4 Mn(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Mn and S: H: | 2 c_1 = 2 c_3 + 2 c_4 O: | c_1 = 2 c_4 Mn: | c_2 = c_4 S: | 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 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + MnS ⟶ H_2S + Mn(OH)_2
Balance the chemical equation algebraically: H_2O + MnS ⟶ H_2S + Mn(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 MnS ⟶ c_3 H_2S + c_4 Mn(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Mn and S: H: | 2 c_1 = 2 c_3 + 2 c_4 O: | c_1 = 2 c_4 Mn: | c_2 = c_4 S: | 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 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + MnS ⟶ H_2S + Mn(OH)_2

Structures

+ ⟶ +
+ ⟶ +

Names

water + manganese sulfide ⟶ hydrogen sulfide + manganese hydroxide
water + manganese sulfide ⟶ hydrogen sulfide + manganese hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + MnS ⟶ H_2S + Mn(OH)_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: 2 H_2O + MnS ⟶ H_2S + Mn(OH)_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 H_2O | 2 | -2 MnS | 1 | -1 H_2S | 1 | 1 Mn(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) MnS | 1 | -1 | ([MnS])^(-1) H_2S | 1 | 1 | [H2S] Mn(OH)_2 | 1 | 1 | [Mn(OH)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 = ([H2O])^(-2) ([MnS])^(-1) [H2S] [Mn(OH)2] = ([H2S] [Mn(OH)2])/(([H2O])^2 [MnS])
Construct the equilibrium constant, K, expression for: H_2O + MnS ⟶ H_2S + Mn(OH)_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: 2 H_2O + MnS ⟶ H_2S + Mn(OH)_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 H_2O | 2 | -2 MnS | 1 | -1 H_2S | 1 | 1 Mn(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) MnS | 1 | -1 | ([MnS])^(-1) H_2S | 1 | 1 | [H2S] Mn(OH)_2 | 1 | 1 | [Mn(OH)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 = ([H2O])^(-2) ([MnS])^(-1) [H2S] [Mn(OH)2] = ([H2S] [Mn(OH)2])/(([H2O])^2 [MnS])

Rate of reaction

Construct the rate of reaction expression for: H_2O + MnS ⟶ H_2S + Mn(OH)_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: 2 H_2O + MnS ⟶ H_2S + Mn(OH)_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 H_2O | 2 | -2 MnS | 1 | -1 H_2S | 1 | 1 Mn(OH)_2 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[H2O])/(Δt) MnS | 1 | -1 | -(Δ[MnS])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) Mn(OH)_2 | 1 | 1 | (Δ[Mn(OH)2])/(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 = -1/2 (Δ[H2O])/(Δt) = -(Δ[MnS])/(Δt) = (Δ[H2S])/(Δt) = (Δ[Mn(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + MnS ⟶ H_2S + Mn(OH)_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: 2 H_2O + MnS ⟶ H_2S + Mn(OH)_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 H_2O | 2 | -2 MnS | 1 | -1 H_2S | 1 | 1 Mn(OH)_2 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[H2O])/(Δt) MnS | 1 | -1 | -(Δ[MnS])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) Mn(OH)_2 | 1 | 1 | (Δ[Mn(OH)2])/(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 = -1/2 (Δ[H2O])/(Δt) = -(Δ[MnS])/(Δt) = (Δ[H2S])/(Δt) = (Δ[Mn(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | manganese sulfide | hydrogen sulfide | manganese hydroxide formula | H_2O | MnS | H_2S | Mn(OH)_2 Hill formula | H_2O | MnS | H_2S | H_2MnO_2 name | water | manganese sulfide | hydrogen sulfide | manganese hydroxide IUPAC name | water | | hydrogen sulfide | manganous dihydroxide
| water | manganese sulfide | hydrogen sulfide | manganese hydroxide formula | H_2O | MnS | H_2S | Mn(OH)_2 Hill formula | H_2O | MnS | H_2S | H_2MnO_2 name | water | manganese sulfide | hydrogen sulfide | manganese hydroxide IUPAC name | water | | hydrogen sulfide | manganous dihydroxide

Substance properties

| water | manganese sulfide | hydrogen sulfide | manganese hydroxide molar mass | 18.015 g/mol | 87 g/mol | 34.08 g/mol | 88.952 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 0 °C | 1141 °C | -85 °C | boiling point | 99.9839 °C | | -60 °C | density | 1 g/cm^3 | 3.3 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 2.64×10^-5 Pa s (at 1250 °C) | 1.239×10^-5 Pa s (at 25 °C) | odor | odorless | | |
| water | manganese sulfide | hydrogen sulfide | manganese hydroxide molar mass | 18.015 g/mol | 87 g/mol | 34.08 g/mol | 88.952 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 0 °C | 1141 °C | -85 °C | boiling point | 99.9839 °C | | -60 °C | density | 1 g/cm^3 | 3.3 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 2.64×10^-5 Pa s (at 1250 °C) | 1.239×10^-5 Pa s (at 25 °C) | odor | odorless | | |

Units

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