KOH + H2O2 + CrCl = H2O + KCl + K2CrO4

KOH potassium hydroxide + H_2O_2 hydrogen peroxide + CrCl ⟶ H_2O water + KCl potassium chloride + K_2CrO_4 potassium chromate

Balance the chemical equation algebraically: KOH + H_2O_2 + CrCl ⟶ H_2O + KCl + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 H_2O_2 + c_3 CrCl ⟶ c_4 H_2O + c_5 KCl + c_6 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Cr and Cl: H: | c_1 + 2 c_2 = 2 c_4 K: | c_1 = c_5 + 2 c_6 O: | c_1 + 2 c_2 = c_4 + 4 c_6 Cr: | c_3 = c_6 Cl: | 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 = 3 c_2 = 5/2 c_3 = 1 c_4 = 4 c_5 = 1 c_6 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 6 c_2 = 5 c_3 = 2 c_4 = 8 c_5 = 2 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KOH + 5 H_2O_2 + 2 CrCl ⟶ 8 H_2O + 2 KCl + 2 K_2CrO_4

+ + CrCl ⟶ + +

potassium hydroxide + hydrogen peroxide + CrCl ⟶ water + potassium chloride + potassium chromate

Construct the equilibrium constant, K, expression for: KOH + H_2O_2 + CrCl ⟶ H_2O + KCl + K_2CrO_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: 6 KOH + 5 H_2O_2 + 2 CrCl ⟶ 8 H_2O + 2 KCl + 2 K_2CrO_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 KOH | 6 | -6 H_2O_2 | 5 | -5 CrCl | 2 | -2 H_2O | 8 | 8 KCl | 2 | 2 K_2CrO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 6 | -6 | ([KOH])^(-6) H_2O_2 | 5 | -5 | ([H2O2])^(-5) CrCl | 2 | -2 | ([CrCl])^(-2) H_2O | 8 | 8 | ([H2O])^8 KCl | 2 | 2 | ([KCl])^2 K_2CrO_4 | 2 | 2 | ([K2CrO4])^2 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])^(-6) ([H2O2])^(-5) ([CrCl])^(-2) ([H2O])^8 ([KCl])^2 ([K2CrO4])^2 = (([H2O])^8 ([KCl])^2 ([K2CrO4])^2)/(([KOH])^6 ([H2O2])^5 ([CrCl])^2)

Construct the rate of reaction expression for: KOH + H_2O_2 + CrCl ⟶ H_2O + KCl + K_2CrO_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: 6 KOH + 5 H_2O_2 + 2 CrCl ⟶ 8 H_2O + 2 KCl + 2 K_2CrO_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 KOH | 6 | -6 H_2O_2 | 5 | -5 CrCl | 2 | -2 H_2O | 8 | 8 KCl | 2 | 2 K_2CrO_4 | 2 | 2 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 | 6 | -6 | -1/6 (Δ[KOH])/(Δt) H_2O_2 | 5 | -5 | -1/5 (Δ[H2O2])/(Δt) CrCl | 2 | -2 | -1/2 (Δ[CrCl])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) KCl | 2 | 2 | 1/2 (Δ[KCl])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(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 = -1/6 (Δ[KOH])/(Δt) = -1/5 (Δ[H2O2])/(Δt) = -1/2 (Δ[CrCl])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/2 (Δ[KCl])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium hydroxide | hydrogen peroxide | CrCl | water | potassium chloride | potassium chromate formula | KOH | H_2O_2 | CrCl | H_2O | KCl | K_2CrO_4 Hill formula | HKO | H_2O_2 | ClCr | H_2O | ClK | CrK_2O_4 name | potassium hydroxide | hydrogen peroxide | | water | potassium chloride | potassium chromate IUPAC name | potassium hydroxide | hydrogen peroxide | | water | potassium chloride | dipotassium dioxido-dioxochromium

| potassium hydroxide | hydrogen peroxide | CrCl | water | potassium chloride | potassium chromate molar mass | 56.105 g/mol | 34.014 g/mol | 87.45 g/mol | 18.015 g/mol | 74.55 g/mol | 194.19 g/mol phase | solid (at STP) | liquid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 406 °C | -0.43 °C | | 0 °C | 770 °C | 971 °C boiling point | 1327 °C | 150.2 °C | | 99.9839 °C | 1420 °C | density | 2.044 g/cm^3 | 1.44 g/cm^3 | | 1 g/cm^3 | 1.98 g/cm^3 | 2.73 g/cm^3 solubility in water | soluble | miscible | | | soluble | soluble surface tension | | 0.0804 N/m | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | odorless | odorless