H2O + AgNO3 + CHI3 = HNO3 + CO + AgI

H_2O water + AgNO_3 silver nitrate + CHI_3 iodoform ⟶ HNO_3 nitric acid + CO carbon monoxide + AgI silver(I) iodide

Balance the chemical equation algebraically: H_2O + AgNO_3 + CHI_3 ⟶ HNO_3 + CO + AgI Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 AgNO_3 + c_3 CHI_3 ⟶ c_4 HNO_3 + c_5 CO + c_6 AgI Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Ag, N, C and I: H: | 2 c_1 + c_3 = c_4 O: | c_1 + 3 c_2 = 3 c_4 + c_5 Ag: | c_2 = c_6 N: | c_2 = c_4 C: | c_3 = c_5 I: | 3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 c_4 = 3 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + 3 AgNO_3 + CHI_3 ⟶ 3 HNO_3 + CO + 3 AgI

+ + ⟶ + +

water + silver nitrate + iodoform ⟶ nitric acid + carbon monoxide + silver(I) iodide

Construct the equilibrium constant, K, expression for: H_2O + AgNO_3 + CHI_3 ⟶ HNO_3 + CO + AgI 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 + 3 AgNO_3 + CHI_3 ⟶ 3 HNO_3 + CO + 3 AgI 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 | 1 | -1 AgNO_3 | 3 | -3 CHI_3 | 1 | -1 HNO_3 | 3 | 3 CO | 1 | 1 AgI | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) AgNO_3 | 3 | -3 | ([AgNO3])^(-3) CHI_3 | 1 | -1 | ([CHI3])^(-1) HNO_3 | 3 | 3 | ([HNO3])^3 CO | 1 | 1 | [CO] AgI | 3 | 3 | ([AgI])^3 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 = ([H2O])^(-1) ([AgNO3])^(-3) ([CHI3])^(-1) ([HNO3])^3 [CO] ([AgI])^3 = (([HNO3])^3 [CO] ([AgI])^3)/([H2O] ([AgNO3])^3 [CHI3])

Construct the rate of reaction expression for: H_2O + AgNO_3 + CHI_3 ⟶ HNO_3 + CO + AgI 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 + 3 AgNO_3 + CHI_3 ⟶ 3 HNO_3 + CO + 3 AgI 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 | 1 | -1 AgNO_3 | 3 | -3 CHI_3 | 1 | -1 HNO_3 | 3 | 3 CO | 1 | 1 AgI | 3 | 3 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 | 1 | -1 | -(Δ[H2O])/(Δt) AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) CHI_3 | 1 | -1 | -(Δ[CHI3])/(Δt) HNO_3 | 3 | 3 | 1/3 (Δ[HNO3])/(Δt) CO | 1 | 1 | (Δ[CO])/(Δt) AgI | 3 | 3 | 1/3 (Δ[AgI])/(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[H2O])/(Δt) = -1/3 (Δ[AgNO3])/(Δt) = -(Δ[CHI3])/(Δt) = 1/3 (Δ[HNO3])/(Δt) = (Δ[CO])/(Δt) = 1/3 (Δ[AgI])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | silver nitrate | iodoform | nitric acid | carbon monoxide | silver(I) iodide formula | H_2O | AgNO_3 | CHI_3 | HNO_3 | CO | AgI name | water | silver nitrate | iodoform | nitric acid | carbon monoxide | silver(I) iodide IUPAC name | water | silver nitrate | iodoform | nitric acid | carbon monoxide | silver iodide