NaOH + H2O2 + CrBr3 = H2O + NaBr + Na2CrO4

NaOH sodium hydroxide + H_2O_2 hydrogen peroxide + Br_3Cr chromium tribromide ⟶ H_2O water + NaBr sodium bromide + Na_2CrO_4 sodium chromate

Balance the chemical equation algebraically: NaOH + H_2O_2 + Br_3Cr ⟶ H_2O + NaBr + Na_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 H_2O_2 + c_3 Br_3Cr ⟶ c_4 H_2O + c_5 NaBr + c_6 Na_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Br and Cr: H: | c_1 + 2 c_2 = 2 c_4 Na: | c_1 = c_5 + 2 c_6 O: | c_1 + 2 c_2 = c_4 + 4 c_6 Br: | 3 c_3 = c_5 Cr: | c_3 = 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 = 5 c_2 = 3/2 c_3 = 1 c_4 = 4 c_5 = 3 c_6 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 10 c_2 = 3 c_3 = 2 c_4 = 8 c_5 = 6 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 NaOH + 3 H_2O_2 + 2 Br_3Cr ⟶ 8 H_2O + 6 NaBr + 2 Na_2CrO_4

+ + ⟶ + +

sodium hydroxide + hydrogen peroxide + chromium tribromide ⟶ water + sodium bromide + sodium chromate

Construct the equilibrium constant, K, expression for: NaOH + H_2O_2 + Br_3Cr ⟶ H_2O + NaBr + Na_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: 10 NaOH + 3 H_2O_2 + 2 Br_3Cr ⟶ 8 H_2O + 6 NaBr + 2 Na_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 NaOH | 10 | -10 H_2O_2 | 3 | -3 Br_3Cr | 2 | -2 H_2O | 8 | 8 NaBr | 6 | 6 Na_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 NaOH | 10 | -10 | ([NaOH])^(-10) H_2O_2 | 3 | -3 | ([H2O2])^(-3) Br_3Cr | 2 | -2 | ([Br3Cr])^(-2) H_2O | 8 | 8 | ([H2O])^8 NaBr | 6 | 6 | ([NaBr])^6 Na_2CrO_4 | 2 | 2 | ([Na2CrO4])^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 = ([NaOH])^(-10) ([H2O2])^(-3) ([Br3Cr])^(-2) ([H2O])^8 ([NaBr])^6 ([Na2CrO4])^2 = (([H2O])^8 ([NaBr])^6 ([Na2CrO4])^2)/(([NaOH])^10 ([H2O2])^3 ([Br3Cr])^2)

Construct the rate of reaction expression for: NaOH + H_2O_2 + Br_3Cr ⟶ H_2O + NaBr + Na_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: 10 NaOH + 3 H_2O_2 + 2 Br_3Cr ⟶ 8 H_2O + 6 NaBr + 2 Na_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 NaOH | 10 | -10 H_2O_2 | 3 | -3 Br_3Cr | 2 | -2 H_2O | 8 | 8 NaBr | 6 | 6 Na_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 NaOH | 10 | -10 | -1/10 (Δ[NaOH])/(Δt) H_2O_2 | 3 | -3 | -1/3 (Δ[H2O2])/(Δt) Br_3Cr | 2 | -2 | -1/2 (Δ[Br3Cr])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) NaBr | 6 | 6 | 1/6 (Δ[NaBr])/(Δt) Na_2CrO_4 | 2 | 2 | 1/2 (Δ[Na2CrO4])/(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 = -1/10 (Δ[NaOH])/(Δt) = -1/3 (Δ[H2O2])/(Δt) = -1/2 (Δ[Br3Cr])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/6 (Δ[NaBr])/(Δt) = 1/2 (Δ[Na2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium hydroxide | hydrogen peroxide | chromium tribromide | water | sodium bromide | sodium chromate formula | NaOH | H_2O_2 | Br_3Cr | H_2O | NaBr | Na_2CrO_4 Hill formula | HNaO | H_2O_2 | Br_3Cr | H_2O | BrNa | CrNa_2O_4 name | sodium hydroxide | hydrogen peroxide | chromium tribromide | water | sodium bromide | sodium chromate IUPAC name | sodium hydroxide | hydrogen peroxide | chromium(+3) cation tribromide | water | sodium bromide | disodium dioxido(dioxo)chromium

| sodium hydroxide | hydrogen peroxide | chromium tribromide | water | sodium bromide | sodium chromate molar mass | 39.997 g/mol | 34.014 g/mol | 291.71 g/mol | 18.015 g/mol | 102.89 g/mol | 161.97 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | -0.43 °C | 1130 °C | 0 °C | 755 °C | 780 °C boiling point | 1390 °C | 150.2 °C | | 99.9839 °C | 1396 °C | density | 2.13 g/cm^3 | 1.44 g/cm^3 | 4.68 g/cm^3 | 1 g/cm^3 | 3.2 g/cm^3 | 2.698 g/cm^3 solubility in water | soluble | miscible | slightly soluble | | soluble | surface tension | 0.07435 N/m | 0.0804 N/m | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | |