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H2SO4 + KI + KBrO3 = H2O + K2SO4 + I2 + KBr

Input interpretation

H_2SO_4 sulfuric acid + KI potassium iodide + KBrO_3 potassium bromate ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + KBr potassium bromide
H_2SO_4 sulfuric acid + KI potassium iodide + KBrO_3 potassium bromate ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + KBr potassium bromide

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KI + KBrO_3 ⟶ H_2O + K_2SO_4 + I_2 + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 KBrO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K and Br: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 3 c_3 = c_4 + 4 c_5 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | c_2 + c_3 = 2 c_5 + c_7 Br: | c_3 = c_7 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 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 3 c_6 = 3 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + 6 KI + KBrO_3 ⟶ 3 H_2O + 3 K_2SO_4 + 3 I_2 + KBr
Balance the chemical equation algebraically: H_2SO_4 + KI + KBrO_3 ⟶ H_2O + K_2SO_4 + I_2 + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 KBrO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K and Br: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 3 c_3 = c_4 + 4 c_5 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | c_2 + c_3 = 2 c_5 + c_7 Br: | c_3 = c_7 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 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 3 c_6 = 3 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + 6 KI + KBrO_3 ⟶ 3 H_2O + 3 K_2SO_4 + 3 I_2 + KBr

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + potassium iodide + potassium bromate ⟶ water + potassium sulfate + iodine + potassium bromide
sulfuric acid + potassium iodide + potassium bromate ⟶ water + potassium sulfate + iodine + potassium bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + KBrO_3 ⟶ H_2O + K_2SO_4 + I_2 + 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: 3 H_2SO_4 + 6 KI + KBrO_3 ⟶ 3 H_2O + 3 K_2SO_4 + 3 I_2 + 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_2SO_4 | 3 | -3 KI | 6 | -6 KBrO_3 | 1 | -1 H_2O | 3 | 3 K_2SO_4 | 3 | 3 I_2 | 3 | 3 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_2SO_4 | 3 | -3 | ([H2SO4])^(-3) KI | 6 | -6 | ([KI])^(-6) KBrO_3 | 1 | -1 | ([KBrO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 K_2SO_4 | 3 | 3 | ([K2SO4])^3 I_2 | 3 | 3 | ([I2])^3 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 = ([H2SO4])^(-3) ([KI])^(-6) ([KBrO3])^(-1) ([H2O])^3 ([K2SO4])^3 ([I2])^3 [KBr] = (([H2O])^3 ([K2SO4])^3 ([I2])^3 [KBr])/(([H2SO4])^3 ([KI])^6 [KBrO3])
Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + KBrO_3 ⟶ H_2O + K_2SO_4 + I_2 + 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: 3 H_2SO_4 + 6 KI + KBrO_3 ⟶ 3 H_2O + 3 K_2SO_4 + 3 I_2 + 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_2SO_4 | 3 | -3 KI | 6 | -6 KBrO_3 | 1 | -1 H_2O | 3 | 3 K_2SO_4 | 3 | 3 I_2 | 3 | 3 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_2SO_4 | 3 | -3 | ([H2SO4])^(-3) KI | 6 | -6 | ([KI])^(-6) KBrO_3 | 1 | -1 | ([KBrO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 K_2SO_4 | 3 | 3 | ([K2SO4])^3 I_2 | 3 | 3 | ([I2])^3 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 = ([H2SO4])^(-3) ([KI])^(-6) ([KBrO3])^(-1) ([H2O])^3 ([K2SO4])^3 ([I2])^3 [KBr] = (([H2O])^3 ([K2SO4])^3 ([I2])^3 [KBr])/(([H2SO4])^3 ([KI])^6 [KBrO3])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KI + KBrO_3 ⟶ H_2O + K_2SO_4 + I_2 + 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: 3 H_2SO_4 + 6 KI + KBrO_3 ⟶ 3 H_2O + 3 K_2SO_4 + 3 I_2 + 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_2SO_4 | 3 | -3 KI | 6 | -6 KBrO_3 | 1 | -1 H_2O | 3 | 3 K_2SO_4 | 3 | 3 I_2 | 3 | 3 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_2SO_4 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) KI | 6 | -6 | -1/6 (Δ[KI])/(Δt) KBrO_3 | 1 | -1 | -(Δ[KBrO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -1/6 (Δ[KI])/(Δt) = -(Δ[KBrO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/3 (Δ[I2])/(Δt) = (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KI + KBrO_3 ⟶ H_2O + K_2SO_4 + I_2 + 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: 3 H_2SO_4 + 6 KI + KBrO_3 ⟶ 3 H_2O + 3 K_2SO_4 + 3 I_2 + 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_2SO_4 | 3 | -3 KI | 6 | -6 KBrO_3 | 1 | -1 H_2O | 3 | 3 K_2SO_4 | 3 | 3 I_2 | 3 | 3 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_2SO_4 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) KI | 6 | -6 | -1/6 (Δ[KI])/(Δt) KBrO_3 | 1 | -1 | -(Δ[KBrO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -1/6 (Δ[KI])/(Δt) = -(Δ[KBrO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/3 (Δ[I2])/(Δt) = (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium iodide | potassium bromate | water | potassium sulfate | iodine | potassium bromide formula | H_2SO_4 | KI | KBrO_3 | H_2O | K_2SO_4 | I_2 | KBr Hill formula | H_2O_4S | IK | BrKO_3 | H_2O | K_2O_4S | I_2 | BrK name | sulfuric acid | potassium iodide | potassium bromate | water | potassium sulfate | iodine | potassium bromide IUPAC name | sulfuric acid | potassium iodide | potassium bromate | water | dipotassium sulfate | molecular iodine | potassium bromide
| sulfuric acid | potassium iodide | potassium bromate | water | potassium sulfate | iodine | potassium bromide formula | H_2SO_4 | KI | KBrO_3 | H_2O | K_2SO_4 | I_2 | KBr Hill formula | H_2O_4S | IK | BrKO_3 | H_2O | K_2O_4S | I_2 | BrK name | sulfuric acid | potassium iodide | potassium bromate | water | potassium sulfate | iodine | potassium bromide IUPAC name | sulfuric acid | potassium iodide | potassium bromate | water | dipotassium sulfate | molecular iodine | potassium bromide

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