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H2O + K2S + KBrO4 = S + KOH + KBr

Input interpretation

H_2O water + K2S + KBrO4 ⟶ S mixed sulfur + KOH potassium hydroxide + KBr potassium bromide
H_2O water + K2S + KBrO4 ⟶ S mixed sulfur + KOH potassium hydroxide + KBr potassium bromide

Balanced equation

Balance the chemical equation algebraically: H_2O + K2S + KBrO4 ⟶ S + KOH + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 K2S + c_3 KBrO4 ⟶ c_4 S + c_5 KOH + c_6 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, S and Br: H: | 2 c_1 = c_5 O: | c_1 + 4 c_3 = c_5 K: | 2 c_2 + c_3 = c_5 + c_6 S: | c_2 = c_4 Br: | 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 = 4 c_2 = 4 c_3 = 1 c_4 = 4 c_5 = 8 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 4 K2S + KBrO4 ⟶ 4 S + 8 KOH + KBr
Balance the chemical equation algebraically: H_2O + K2S + KBrO4 ⟶ S + KOH + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 K2S + c_3 KBrO4 ⟶ c_4 S + c_5 KOH + c_6 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, S and Br: H: | 2 c_1 = c_5 O: | c_1 + 4 c_3 = c_5 K: | 2 c_2 + c_3 = c_5 + c_6 S: | c_2 = c_4 Br: | 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 = 4 c_2 = 4 c_3 = 1 c_4 = 4 c_5 = 8 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 4 K2S + KBrO4 ⟶ 4 S + 8 KOH + KBr

Structures

+ K2S + KBrO4 ⟶ + +
+ K2S + KBrO4 ⟶ + +

Names

water + K2S + KBrO4 ⟶ mixed sulfur + potassium hydroxide + potassium bromide
water + K2S + KBrO4 ⟶ mixed sulfur + potassium hydroxide + potassium bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + K2S + KBrO4 ⟶ S + KOH + KBr 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: 4 H_2O + 4 K2S + KBrO4 ⟶ 4 S + 8 KOH + KBr 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 | 4 | -4 K2S | 4 | -4 KBrO4 | 1 | -1 S | 4 | 4 KOH | 8 | 8 KBr | 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 | 4 | -4 | ([H2O])^(-4) K2S | 4 | -4 | ([K2S])^(-4) KBrO4 | 1 | -1 | ([KBrO4])^(-1) S | 4 | 4 | ([S])^4 KOH | 8 | 8 | ([KOH])^8 KBr | 1 | 1 | [KBr] 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])^(-4) ([K2S])^(-4) ([KBrO4])^(-1) ([S])^4 ([KOH])^8 [KBr] = (([S])^4 ([KOH])^8 [KBr])/(([H2O])^4 ([K2S])^4 [KBrO4])
Construct the equilibrium constant, K, expression for: H_2O + K2S + KBrO4 ⟶ S + KOH + KBr 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: 4 H_2O + 4 K2S + KBrO4 ⟶ 4 S + 8 KOH + KBr 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 | 4 | -4 K2S | 4 | -4 KBrO4 | 1 | -1 S | 4 | 4 KOH | 8 | 8 KBr | 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 | 4 | -4 | ([H2O])^(-4) K2S | 4 | -4 | ([K2S])^(-4) KBrO4 | 1 | -1 | ([KBrO4])^(-1) S | 4 | 4 | ([S])^4 KOH | 8 | 8 | ([KOH])^8 KBr | 1 | 1 | [KBr] 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])^(-4) ([K2S])^(-4) ([KBrO4])^(-1) ([S])^4 ([KOH])^8 [KBr] = (([S])^4 ([KOH])^8 [KBr])/(([H2O])^4 ([K2S])^4 [KBrO4])

Rate of reaction

Construct the rate of reaction expression for: H_2O + K2S + KBrO4 ⟶ S + KOH + KBr 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: 4 H_2O + 4 K2S + KBrO4 ⟶ 4 S + 8 KOH + KBr 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 | 4 | -4 K2S | 4 | -4 KBrO4 | 1 | -1 S | 4 | 4 KOH | 8 | 8 KBr | 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 | 4 | -4 | -1/4 (Δ[H2O])/(Δt) K2S | 4 | -4 | -1/4 (Δ[K2S])/(Δt) KBrO4 | 1 | -1 | -(Δ[KBrO4])/(Δt) S | 4 | 4 | 1/4 (Δ[S])/(Δt) KOH | 8 | 8 | 1/8 (Δ[KOH])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/4 (Δ[K2S])/(Δt) = -(Δ[KBrO4])/(Δt) = 1/4 (Δ[S])/(Δt) = 1/8 (Δ[KOH])/(Δt) = (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + K2S + KBrO4 ⟶ S + KOH + KBr 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: 4 H_2O + 4 K2S + KBrO4 ⟶ 4 S + 8 KOH + KBr 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 | 4 | -4 K2S | 4 | -4 KBrO4 | 1 | -1 S | 4 | 4 KOH | 8 | 8 KBr | 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 | 4 | -4 | -1/4 (Δ[H2O])/(Δt) K2S | 4 | -4 | -1/4 (Δ[K2S])/(Δt) KBrO4 | 1 | -1 | -(Δ[KBrO4])/(Δt) S | 4 | 4 | 1/4 (Δ[S])/(Δt) KOH | 8 | 8 | 1/8 (Δ[KOH])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/4 (Δ[K2S])/(Δt) = -(Δ[KBrO4])/(Δt) = 1/4 (Δ[S])/(Δt) = 1/8 (Δ[KOH])/(Δt) = (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | K2S | KBrO4 | mixed sulfur | potassium hydroxide | potassium bromide formula | H_2O | K2S | KBrO4 | S | KOH | KBr Hill formula | H_2O | K2S | BrKO4 | S | HKO | BrK name | water | | | mixed sulfur | potassium hydroxide | potassium bromide IUPAC name | water | | | sulfur | potassium hydroxide | potassium bromide
| water | K2S | KBrO4 | mixed sulfur | potassium hydroxide | potassium bromide formula | H_2O | K2S | KBrO4 | S | KOH | KBr Hill formula | H_2O | K2S | BrKO4 | S | HKO | BrK name | water | | | mixed sulfur | potassium hydroxide | potassium bromide IUPAC name | water | | | sulfur | potassium hydroxide | potassium bromide

Substance properties

| water | K2S | KBrO4 | mixed sulfur | potassium hydroxide | potassium bromide molar mass | 18.015 g/mol | 110.26 g/mol | 183 g/mol | 32.06 g/mol | 56.105 g/mol | 119 g/mol phase | liquid (at STP) | | | solid (at STP) | solid (at STP) | solid (at STP) melting point | 0 °C | | | 112.8 °C | 406 °C | 734 °C boiling point | 99.9839 °C | | | 444.7 °C | 1327 °C | 1435 °C density | 1 g/cm^3 | | | 2.07 g/cm^3 | 2.044 g/cm^3 | 2.75 g/cm^3 solubility in water | | | | | soluble | soluble surface tension | 0.0728 N/m | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | | 0.001 Pa s (at 550 °C) | odor | odorless | | | | |
| water | K2S | KBrO4 | mixed sulfur | potassium hydroxide | potassium bromide molar mass | 18.015 g/mol | 110.26 g/mol | 183 g/mol | 32.06 g/mol | 56.105 g/mol | 119 g/mol phase | liquid (at STP) | | | solid (at STP) | solid (at STP) | solid (at STP) melting point | 0 °C | | | 112.8 °C | 406 °C | 734 °C boiling point | 99.9839 °C | | | 444.7 °C | 1327 °C | 1435 °C density | 1 g/cm^3 | | | 2.07 g/cm^3 | 2.044 g/cm^3 | 2.75 g/cm^3 solubility in water | | | | | soluble | soluble surface tension | 0.0728 N/m | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | | 0.001 Pa s (at 550 °C) | odor | odorless | | | | |

Units

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