KOH + I2 + AsH3 = H2O + KI + K3AsO

KOH potassium hydroxide + I_2 iodine + AsH_3 arsine ⟶ H_2O water + KI potassium iodide + K3AsO

Balance the chemical equation algebraically: KOH + I_2 + AsH_3 ⟶ H_2O + KI + K3AsO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 I_2 + c_3 AsH_3 ⟶ c_4 H_2O + c_5 KI + c_6 K3AsO Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, I and As: H: | c_1 + 3 c_3 = 2 c_4 K: | c_1 = c_5 + 3 c_6 O: | c_1 = c_4 + c_6 I: | 2 c_2 = c_5 As: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5 c_2 = 1 c_3 = 1 c_4 = 4 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 KOH + I_2 + AsH_3 ⟶ 4 H_2O + 2 KI + K3AsO

+ + ⟶ + + K3AsO

potassium hydroxide + iodine + arsine ⟶ water + potassium iodide + K3AsO

Construct the equilibrium constant, K, expression for: KOH + I_2 + AsH_3 ⟶ H_2O + KI + K3AsO 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: 5 KOH + I_2 + AsH_3 ⟶ 4 H_2O + 2 KI + K3AsO 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 | 5 | -5 I_2 | 1 | -1 AsH_3 | 1 | -1 H_2O | 4 | 4 KI | 2 | 2 K3AsO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 5 | -5 | ([KOH])^(-5) I_2 | 1 | -1 | ([I2])^(-1) AsH_3 | 1 | -1 | ([AsH3])^(-1) H_2O | 4 | 4 | ([H2O])^4 KI | 2 | 2 | ([KI])^2 K3AsO | 1 | 1 | [K3AsO] 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])^(-5) ([I2])^(-1) ([AsH3])^(-1) ([H2O])^4 ([KI])^2 [K3AsO] = (([H2O])^4 ([KI])^2 [K3AsO])/(([KOH])^5 [I2] [AsH3])

Construct the rate of reaction expression for: KOH + I_2 + AsH_3 ⟶ H_2O + KI + K3AsO 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: 5 KOH + I_2 + AsH_3 ⟶ 4 H_2O + 2 KI + K3AsO 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 | 5 | -5 I_2 | 1 | -1 AsH_3 | 1 | -1 H_2O | 4 | 4 KI | 2 | 2 K3AsO | 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 KOH | 5 | -5 | -1/5 (Δ[KOH])/(Δt) I_2 | 1 | -1 | -(Δ[I2])/(Δt) AsH_3 | 1 | -1 | -(Δ[AsH3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) KI | 2 | 2 | 1/2 (Δ[KI])/(Δt) K3AsO | 1 | 1 | (Δ[K3AsO])/(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 = -1/5 (Δ[KOH])/(Δt) = -(Δ[I2])/(Δt) = -(Δ[AsH3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/2 (Δ[KI])/(Δt) = (Δ[K3AsO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium hydroxide | iodine | arsine | water | potassium iodide | K3AsO formula | KOH | I_2 | AsH_3 | H_2O | KI | K3AsO Hill formula | HKO | I_2 | AsH_3 | H_2O | IK | AsK3O name | potassium hydroxide | iodine | arsine | water | potassium iodide | IUPAC name | potassium hydroxide | molecular iodine | arsane | water | potassium iodide |

| potassium hydroxide | iodine | arsine | water | potassium iodide | K3AsO molar mass | 56.105 g/mol | 253.80894 g/mol | 77.946 g/mol | 18.015 g/mol | 166.0028 g/mol | 208.215 g/mol phase | solid (at STP) | solid (at STP) | gas (at STP) | liquid (at STP) | solid (at STP) | melting point | 406 °C | 113 °C | -111.2 °C | 0 °C | 681 °C | boiling point | 1327 °C | 184 °C | -62.5 °C | 99.9839 °C | 1330 °C | density | 2.044 g/cm^3 | 4.94 g/cm^3 | 0.003186 g/cm^3 (at 25 °C) | 1 g/cm^3 | 3.123 g/cm^3 | solubility in water | soluble | | | | | surface tension | | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 0.00227 Pa s (at 116 °C) | 1.47×10^-5 Pa s (at 0 °C) | 8.9×10^-4 Pa s (at 25 °C) | 0.0010227 Pa s (at 732.9 °C) | odor | | | | odorless | |