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H2S + HBrO3 = H2O + S + HBr

Input interpretation

H_2S (hydrogen sulfide) + HO_3Br (bromic acid) ⟶ H_2O (water) + S (mixed sulfur) + HBr (hydrogen bromide)
H_2S (hydrogen sulfide) + HO_3Br (bromic acid) ⟶ H_2O (water) + S (mixed sulfur) + HBr (hydrogen bromide)

Balanced equation

Balance the chemical equation algebraically: H_2S + HO_3Br ⟶ H_2O + S + HBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 HO_3Br ⟶ c_3 H_2O + c_4 S + c_5 HBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, Br and O: H: | 2 c_1 + c_2 = 2 c_3 + c_5 S: | c_1 = c_4 Br: | c_2 = c_5 O: | 3 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 = 3 c_2 = 1 c_3 = 3 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2S + HO_3Br ⟶ 3 H_2O + 3 S + HBr
Balance the chemical equation algebraically: H_2S + HO_3Br ⟶ H_2O + S + HBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 HO_3Br ⟶ c_3 H_2O + c_4 S + c_5 HBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, Br and O: H: | 2 c_1 + c_2 = 2 c_3 + c_5 S: | c_1 = c_4 Br: | c_2 = c_5 O: | 3 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 = 3 c_2 = 1 c_3 = 3 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2S + HO_3Br ⟶ 3 H_2O + 3 S + HBr

Structures

+ ⟶ + +
+ ⟶ + +

Names

hydrogen sulfide + bromic acid ⟶ water + mixed sulfur + hydrogen bromide
hydrogen sulfide + bromic acid ⟶ water + mixed sulfur + hydrogen bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2S + HO_3Br ⟶ H_2O + S + HBr 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: 3 H_2S + HO_3Br ⟶ 3 H_2O + 3 S + HBr 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_2S | 3 | -3 HO_3Br | 1 | -1 H_2O | 3 | 3 S | 3 | 3 HBr | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 3 | -3 | ([H2S])^(-3) HO_3Br | 1 | -1 | ([H1O3Br1])^(-1) H_2O | 3 | 3 | ([H2O])^3 S | 3 | 3 | ([S])^3 HBr | 1 | 1 | [HBr] 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 = ([H2S])^(-3) ([H1O3Br1])^(-1) ([H2O])^3 ([S])^3 [HBr] = (([H2O])^3 ([S])^3 [HBr])/(([H2S])^3 [H1O3Br1])
Construct the equilibrium constant, K, expression for: H_2S + HO_3Br ⟶ H_2O + S + HBr 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: 3 H_2S + HO_3Br ⟶ 3 H_2O + 3 S + HBr 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_2S | 3 | -3 HO_3Br | 1 | -1 H_2O | 3 | 3 S | 3 | 3 HBr | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 3 | -3 | ([H2S])^(-3) HO_3Br | 1 | -1 | ([H1O3Br1])^(-1) H_2O | 3 | 3 | ([H2O])^3 S | 3 | 3 | ([S])^3 HBr | 1 | 1 | [HBr] 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 = ([H2S])^(-3) ([H1O3Br1])^(-1) ([H2O])^3 ([S])^3 [HBr] = (([H2O])^3 ([S])^3 [HBr])/(([H2S])^3 [H1O3Br1])

Rate of reaction

Construct the rate of reaction expression for: H_2S + HO_3Br ⟶ H_2O + S + HBr 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: 3 H_2S + HO_3Br ⟶ 3 H_2O + 3 S + HBr 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_2S | 3 | -3 HO_3Br | 1 | -1 H_2O | 3 | 3 S | 3 | 3 HBr | 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_2S | 3 | -3 | -1/3 (Δ[H2S])/(Δt) HO_3Br | 1 | -1 | -(Δ[H1O3Br1])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) S | 3 | 3 | 1/3 (Δ[S])/(Δt) HBr | 1 | 1 | (Δ[HBr])/(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 = -1/3 (Δ[H2S])/(Δt) = -(Δ[H1O3Br1])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = (Δ[HBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2S + HO_3Br ⟶ H_2O + S + HBr 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: 3 H_2S + HO_3Br ⟶ 3 H_2O + 3 S + HBr 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_2S | 3 | -3 HO_3Br | 1 | -1 H_2O | 3 | 3 S | 3 | 3 HBr | 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_2S | 3 | -3 | -1/3 (Δ[H2S])/(Δt) HO_3Br | 1 | -1 | -(Δ[H1O3Br1])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) S | 3 | 3 | 1/3 (Δ[S])/(Δt) HBr | 1 | 1 | (Δ[HBr])/(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 = -1/3 (Δ[H2S])/(Δt) = -(Δ[H1O3Br1])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = (Δ[HBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen sulfide | bromic acid | water | mixed sulfur | hydrogen bromide formula | H_2S | HO_3Br | H_2O | S | HBr Hill formula | H_2S | BrHO_3 | H_2O | S | BrH name | hydrogen sulfide | bromic acid | water | mixed sulfur | hydrogen bromide IUPAC name | hydrogen sulfide | bromic acid | water | sulfur | hydrogen bromide
| hydrogen sulfide | bromic acid | water | mixed sulfur | hydrogen bromide formula | H_2S | HO_3Br | H_2O | S | HBr Hill formula | H_2S | BrHO_3 | H_2O | S | BrH name | hydrogen sulfide | bromic acid | water | mixed sulfur | hydrogen bromide IUPAC name | hydrogen sulfide | bromic acid | water | sulfur | hydrogen bromide

Substance properties

| hydrogen sulfide | bromic acid | water | mixed sulfur | hydrogen bromide molar mass | 34.08 g/mol | 128.91 g/mol | 18.015 g/mol | 32.06 g/mol | 80.912 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) melting point | -85 °C | | 0 °C | 112.8 °C | -86.8 °C boiling point | -60 °C | | 99.9839 °C | 444.7 °C | -66.38 °C density | 0.001393 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 2.07 g/cm^3 | 0.003307 g/cm^3 (at 25 °C) solubility in water | | | | | miscible surface tension | | | 0.0728 N/m | | 0.0271 N/m dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 8.4×10^-4 Pa s (at -75 °C) odor | | | odorless | |
| hydrogen sulfide | bromic acid | water | mixed sulfur | hydrogen bromide molar mass | 34.08 g/mol | 128.91 g/mol | 18.015 g/mol | 32.06 g/mol | 80.912 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) melting point | -85 °C | | 0 °C | 112.8 °C | -86.8 °C boiling point | -60 °C | | 99.9839 °C | 444.7 °C | -66.38 °C density | 0.001393 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 2.07 g/cm^3 | 0.003307 g/cm^3 (at 25 °C) solubility in water | | | | | miscible surface tension | | | 0.0728 N/m | | 0.0271 N/m dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 8.4×10^-4 Pa s (at -75 °C) odor | | | odorless | |

Units

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