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KOH + Br2 + K2S2O3 = H2O + K2SO4 + KBr

Input interpretation

KOH potassium hydroxide + Br_2 bromine + K_2S_2O_3 potassium thiosulfate ⟶ H_2O water + K_2SO_4 potassium sulfate + KBr potassium bromide
KOH potassium hydroxide + Br_2 bromine + K_2S_2O_3 potassium thiosulfate ⟶ H_2O water + K_2SO_4 potassium sulfate + KBr potassium bromide

Balanced equation

Balance the chemical equation algebraically: KOH + Br_2 + K_2S_2O_3 ⟶ H_2O + K_2SO_4 + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 Br_2 + c_3 K_2S_2O_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Br and S: H: | c_1 = 2 c_4 K: | c_1 + 2 c_3 = 2 c_5 + c_6 O: | c_1 + 3 c_3 = c_4 + 4 c_5 Br: | 2 c_2 = c_6 S: | 2 c_3 = c_5 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 = 10 c_2 = 4 c_3 = 1 c_4 = 5 c_5 = 2 c_6 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 KOH + 4 Br_2 + K_2S_2O_3 ⟶ 5 H_2O + 2 K_2SO_4 + 8 KBr
Balance the chemical equation algebraically: KOH + Br_2 + K_2S_2O_3 ⟶ H_2O + K_2SO_4 + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 Br_2 + c_3 K_2S_2O_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Br and S: H: | c_1 = 2 c_4 K: | c_1 + 2 c_3 = 2 c_5 + c_6 O: | c_1 + 3 c_3 = c_4 + 4 c_5 Br: | 2 c_2 = c_6 S: | 2 c_3 = c_5 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 = 10 c_2 = 4 c_3 = 1 c_4 = 5 c_5 = 2 c_6 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 KOH + 4 Br_2 + K_2S_2O_3 ⟶ 5 H_2O + 2 K_2SO_4 + 8 KBr

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

potassium hydroxide + bromine + potassium thiosulfate ⟶ water + potassium sulfate + potassium bromide
potassium hydroxide + bromine + potassium thiosulfate ⟶ water + potassium sulfate + potassium bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + Br_2 + K_2S_2O_3 ⟶ H_2O + K_2SO_4 + 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: 10 KOH + 4 Br_2 + K_2S_2O_3 ⟶ 5 H_2O + 2 K_2SO_4 + 8 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 KOH | 10 | -10 Br_2 | 4 | -4 K_2S_2O_3 | 1 | -1 H_2O | 5 | 5 K_2SO_4 | 2 | 2 KBr | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 10 | -10 | ([KOH])^(-10) Br_2 | 4 | -4 | ([Br2])^(-4) K_2S_2O_3 | 1 | -1 | ([K2S2O3])^(-1) H_2O | 5 | 5 | ([H2O])^5 K_2SO_4 | 2 | 2 | ([K2SO4])^2 KBr | 8 | 8 | ([KBr])^8 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 = ([KOH])^(-10) ([Br2])^(-4) ([K2S2O3])^(-1) ([H2O])^5 ([K2SO4])^2 ([KBr])^8 = (([H2O])^5 ([K2SO4])^2 ([KBr])^8)/(([KOH])^10 ([Br2])^4 [K2S2O3])
Construct the equilibrium constant, K, expression for: KOH + Br_2 + K_2S_2O_3 ⟶ H_2O + K_2SO_4 + 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: 10 KOH + 4 Br_2 + K_2S_2O_3 ⟶ 5 H_2O + 2 K_2SO_4 + 8 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 KOH | 10 | -10 Br_2 | 4 | -4 K_2S_2O_3 | 1 | -1 H_2O | 5 | 5 K_2SO_4 | 2 | 2 KBr | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 10 | -10 | ([KOH])^(-10) Br_2 | 4 | -4 | ([Br2])^(-4) K_2S_2O_3 | 1 | -1 | ([K2S2O3])^(-1) H_2O | 5 | 5 | ([H2O])^5 K_2SO_4 | 2 | 2 | ([K2SO4])^2 KBr | 8 | 8 | ([KBr])^8 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 = ([KOH])^(-10) ([Br2])^(-4) ([K2S2O3])^(-1) ([H2O])^5 ([K2SO4])^2 ([KBr])^8 = (([H2O])^5 ([K2SO4])^2 ([KBr])^8)/(([KOH])^10 ([Br2])^4 [K2S2O3])

Rate of reaction

Construct the rate of reaction expression for: KOH + Br_2 + K_2S_2O_3 ⟶ H_2O + K_2SO_4 + 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: 10 KOH + 4 Br_2 + K_2S_2O_3 ⟶ 5 H_2O + 2 K_2SO_4 + 8 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 KOH | 10 | -10 Br_2 | 4 | -4 K_2S_2O_3 | 1 | -1 H_2O | 5 | 5 K_2SO_4 | 2 | 2 KBr | 8 | 8 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 KOH | 10 | -10 | -1/10 (Δ[KOH])/(Δt) Br_2 | 4 | -4 | -1/4 (Δ[Br2])/(Δt) K_2S_2O_3 | 1 | -1 | -(Δ[K2S2O3])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) K_2SO_4 | 2 | 2 | 1/2 (Δ[K2SO4])/(Δt) KBr | 8 | 8 | 1/8 (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 = -1/10 (Δ[KOH])/(Δt) = -1/4 (Δ[Br2])/(Δt) = -(Δ[K2S2O3])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/2 (Δ[K2SO4])/(Δt) = 1/8 (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + Br_2 + K_2S_2O_3 ⟶ H_2O + K_2SO_4 + 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: 10 KOH + 4 Br_2 + K_2S_2O_3 ⟶ 5 H_2O + 2 K_2SO_4 + 8 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 KOH | 10 | -10 Br_2 | 4 | -4 K_2S_2O_3 | 1 | -1 H_2O | 5 | 5 K_2SO_4 | 2 | 2 KBr | 8 | 8 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 KOH | 10 | -10 | -1/10 (Δ[KOH])/(Δt) Br_2 | 4 | -4 | -1/4 (Δ[Br2])/(Δt) K_2S_2O_3 | 1 | -1 | -(Δ[K2S2O3])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) K_2SO_4 | 2 | 2 | 1/2 (Δ[K2SO4])/(Δt) KBr | 8 | 8 | 1/8 (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 = -1/10 (Δ[KOH])/(Δt) = -1/4 (Δ[Br2])/(Δt) = -(Δ[K2S2O3])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/2 (Δ[K2SO4])/(Δt) = 1/8 (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | bromine | potassium thiosulfate | water | potassium sulfate | potassium bromide formula | KOH | Br_2 | K_2S_2O_3 | H_2O | K_2SO_4 | KBr Hill formula | HKO | Br_2 | K_2O_3S_2 | H_2O | K_2O_4S | BrK name | potassium hydroxide | bromine | potassium thiosulfate | water | potassium sulfate | potassium bromide IUPAC name | potassium hydroxide | molecular bromine | | water | dipotassium sulfate | potassium bromide
| potassium hydroxide | bromine | potassium thiosulfate | water | potassium sulfate | potassium bromide formula | KOH | Br_2 | K_2S_2O_3 | H_2O | K_2SO_4 | KBr Hill formula | HKO | Br_2 | K_2O_3S_2 | H_2O | K_2O_4S | BrK name | potassium hydroxide | bromine | potassium thiosulfate | water | potassium sulfate | potassium bromide IUPAC name | potassium hydroxide | molecular bromine | | water | dipotassium sulfate | potassium bromide

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