H2SO4 + KCl + KClO3 = H2O + Cl2 + K2SO4

Input interpretation

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H_2SO_4 sulfuric acid + KCl potassium chloride + KClO_3 potassium chlorate ⟶ H_2O water + Cl_2 chlorine + K_2SO_4 potassium sulfate

Balanced equation

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Balance the chemical equation algebraically: H_2SO_4 + KCl + KClO_3 ⟶ H_2O + Cl_2 + K_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KCl + c_3 KClO_3 ⟶ c_4 H_2O + c_5 Cl_2 + c_6 K_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cl and K: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 3 c_3 = c_4 + 4 c_6 S: | c_1 = c_6 Cl: | c_2 + c_3 = 2 c_5 K: | c_2 + c_3 = 2 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 = 3 c_2 = 5 c_3 = 1 c_4 = 3 c_5 = 3 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + 5 KCl + KClO_3 ⟶ 3 H_2O + 3 Cl_2 + 3 K_2SO_4

+ + ⟶ + +

Names

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sulfuric acid + potassium chloride + potassium chlorate ⟶ water + chlorine + potassium sulfate

Equilibrium constant

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Construct the equilibrium constant, K, expression for: H_2SO_4 + KCl + KClO_3 ⟶ H_2O + Cl_2 + K_2SO_4 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 + 5 KCl + KClO_3 ⟶ 3 H_2O + 3 Cl_2 + 3 K_2SO_4 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 KCl | 5 | -5 KClO_3 | 1 | -1 H_2O | 3 | 3 Cl_2 | 3 | 3 K_2SO_4 | 3 | 3 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) KCl | 5 | -5 | ([KCl])^(-5) KClO_3 | 1 | -1 | ([KClO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 Cl_2 | 3 | 3 | ([Cl2])^3 K_2SO_4 | 3 | 3 | ([K2SO4])^3 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) ([KCl])^(-5) ([KClO3])^(-1) ([H2O])^3 ([Cl2])^3 ([K2SO4])^3 = (([H2O])^3 ([Cl2])^3 ([K2SO4])^3)/(([H2SO4])^3 ([KCl])^5 [KClO3])

Rate of reaction

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Construct the rate of reaction expression for: H_2SO_4 + KCl + KClO_3 ⟶ H_2O + Cl_2 + K_2SO_4 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 + 5 KCl + KClO_3 ⟶ 3 H_2O + 3 Cl_2 + 3 K_2SO_4 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 KCl | 5 | -5 KClO_3 | 1 | -1 H_2O | 3 | 3 Cl_2 | 3 | 3 K_2SO_4 | 3 | 3 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) KCl | 5 | -5 | -1/5 (Δ[KCl])/(Δt) KClO_3 | 1 | -1 | -(Δ[KClO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) Cl_2 | 3 | 3 | 1/3 (Δ[Cl2])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(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) = -1/5 (Δ[KCl])/(Δt) = -(Δ[KClO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[Cl2])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)