H2SO4 + K2S + NaClO = H2O + K2SO4 + S + NaCl

H_2SO_4 sulfuric acid + K2S + NaOCl sodium hypochlorite ⟶ H_2O water + K_2SO_4 potassium sulfate + S mixed sulfur + NaCl sodium chloride

Balance the chemical equation algebraically: H_2SO_4 + K2S + NaOCl ⟶ H_2O + K_2SO_4 + S + NaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 K2S + c_3 NaOCl ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 S + c_7 NaCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Cl and Na: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + c_3 = c_4 + 4 c_5 S: | c_1 + c_2 = c_5 + c_6 K: | 2 c_2 = 2 c_5 Cl: | c_3 = c_7 Na: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_3 = 4 c_2 - 3 c_4 = 1 c_5 = c_2 c_6 = 1 c_7 = 4 c_2 - 3 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 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + K2S + NaOCl ⟶ H_2O + K_2SO_4 + S + NaCl

+ K2S + ⟶ + + +

sulfuric acid + K2S + sodium hypochlorite ⟶ water + potassium sulfate + mixed sulfur + sodium chloride

Construct the equilibrium constant, K, expression for: H_2SO_4 + K2S + NaOCl ⟶ H_2O + K_2SO_4 + S + 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_2SO_4 + K2S + NaOCl ⟶ H_2O + K_2SO_4 + S + 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_2SO_4 | 1 | -1 K2S | 1 | -1 NaOCl | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 S | 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_2SO_4 | 1 | -1 | ([H2SO4])^(-1) K2S | 1 | -1 | ([K2S])^(-1) NaOCl | 1 | -1 | ([NaOCl])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] S | 1 | 1 | [S] 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 = ([H2SO4])^(-1) ([K2S])^(-1) ([NaOCl])^(-1) [H2O] [K2SO4] [S] [NaCl] = ([H2O] [K2SO4] [S] [NaCl])/([H2SO4] [K2S] [NaOCl])

Construct the rate of reaction expression for: H_2SO_4 + K2S + NaOCl ⟶ H_2O + K_2SO_4 + S + 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_2SO_4 + K2S + NaOCl ⟶ H_2O + K_2SO_4 + S + 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_2SO_4 | 1 | -1 K2S | 1 | -1 NaOCl | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 S | 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) K2S | 1 | -1 | -(Δ[K2S])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) S | 1 | 1 | (Δ[S])/(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[H2SO4])/(Δt) = -(Δ[K2S])/(Δt) = -(Δ[NaOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[S])/(Δt) = (Δ[NaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | K2S | sodium hypochlorite | water | potassium sulfate | mixed sulfur | sodium chloride formula | H_2SO_4 | K2S | NaOCl | H_2O | K_2SO_4 | S | NaCl Hill formula | H_2O_4S | K2S | ClNaO | H_2O | K_2O_4S | S | ClNa name | sulfuric acid | | sodium hypochlorite | water | potassium sulfate | mixed sulfur | sodium chloride IUPAC name | sulfuric acid | | sodium hypochlorite | water | dipotassium sulfate | sulfur | sodium chloride

| sulfuric acid | K2S | sodium hypochlorite | water | potassium sulfate | mixed sulfur | sodium chloride molar mass | 98.07 g/mol | 110.26 g/mol | 74.44 g/mol | 18.015 g/mol | 174.25 g/mol | 32.06 g/mol | 58.44 g/mol phase | liquid (at STP) | | liquid (at STP) | liquid (at STP) | | solid (at STP) | solid (at STP) melting point | 10.371 °C | | -6 °C | 0 °C | | 112.8 °C | 801 °C boiling point | 279.6 °C | | | 99.9839 °C | | 444.7 °C | 1413 °C density | 1.8305 g/cm^3 | | 1.11 g/cm^3 | 1 g/cm^3 | | 2.07 g/cm^3 | 2.16 g/cm^3 solubility in water | very soluble | | miscible | | soluble | | soluble surface tension | 0.0735 N/m | | | 0.0728 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | | odor | odorless | | | odorless | | | odorless