H2O2 + NaClO = H2O + O2 + NaCl

Input interpretation

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H_2O_2 hydrogen peroxide + NaOCl sodium hypochlorite ⟶ H_2O water + O_2 oxygen + NaCl sodium chloride

Balanced equation

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Balance the chemical equation algebraically: H_2O_2 + NaOCl ⟶ H_2O + O_2 + NaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 NaOCl ⟶ c_3 H_2O + c_4 O_2 + c_5 NaCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl and Na: H: | 2 c_1 = 2 c_3 O: | 2 c_1 + c_2 = c_3 + 2 c_4 Cl: | c_2 = c_5 Na: | c_2 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_3 = 1 c_4 = c_2/2 + 1/2 c_5 = c_2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 1 and solve for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O_2 + NaOCl ⟶ H_2O + O_2 + NaCl

+ ⟶ + +

Names

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hydrogen peroxide + sodium hypochlorite ⟶ water + oxygen + sodium chloride

Equilibrium constant

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Construct the equilibrium constant, K, expression for: H_2O_2 + NaOCl ⟶ H_2O + O_2 + NaCl 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: H_2O_2 + NaOCl ⟶ H_2O + O_2 + NaCl 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_2 | 1 | -1 NaOCl | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 NaCl | 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_2 | 1 | -1 | ([H2O2])^(-1) NaOCl | 1 | -1 | ([NaOCl])^(-1) H_2O | 1 | 1 | [H2O] O_2 | 1 | 1 | [O2] NaCl | 1 | 1 | [NaCl] 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 = ([H2O2])^(-1) ([NaOCl])^(-1) [H2O] [O2] [NaCl] = ([H2O] [O2] [NaCl])/([H2O2] [NaOCl])

Rate of reaction

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Construct the rate of reaction expression for: H_2O_2 + NaOCl ⟶ H_2O + O_2 + NaCl 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: H_2O_2 + NaOCl ⟶ H_2O + O_2 + NaCl 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_2 | 1 | -1 NaOCl | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 NaCl | 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_2 | 1 | -1 | -(Δ[H2O2])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(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 = -(Δ[H2O2])/(Δt) = -(Δ[NaOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = (Δ[NaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)