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K2Cr2O7 + HI = H2O + I2 + KI + CrI3

Input interpretation

K_2Cr_2O_7 potassium dichromate + HI hydrogen iodide ⟶ H_2O water + I_2 iodine + KI potassium iodide + Cr_1I_3 chromium(III) iodide
K_2Cr_2O_7 potassium dichromate + HI hydrogen iodide ⟶ H_2O water + I_2 iodine + KI potassium iodide + Cr_1I_3 chromium(III) iodide

Balanced equation

Balance the chemical equation algebraically: K_2Cr_2O_7 + HI ⟶ H_2O + I_2 + KI + Cr_1I_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2Cr_2O_7 + c_2 HI ⟶ c_3 H_2O + c_4 I_2 + c_5 KI + c_6 Cr_1I_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cr, K, O, H and I: Cr: | 2 c_1 = c_6 K: | 2 c_1 = c_5 O: | 7 c_1 = c_3 H: | c_2 = 2 c_3 I: | c_2 = 2 c_4 + c_5 + 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 = 14 c_3 = 7 c_4 = 3 c_5 = 2 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K_2Cr_2O_7 + 14 HI ⟶ 7 H_2O + 3 I_2 + 2 KI + 2 Cr_1I_3
Balance the chemical equation algebraically: K_2Cr_2O_7 + HI ⟶ H_2O + I_2 + KI + Cr_1I_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2Cr_2O_7 + c_2 HI ⟶ c_3 H_2O + c_4 I_2 + c_5 KI + c_6 Cr_1I_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cr, K, O, H and I: Cr: | 2 c_1 = c_6 K: | 2 c_1 = c_5 O: | 7 c_1 = c_3 H: | c_2 = 2 c_3 I: | c_2 = 2 c_4 + c_5 + 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 = 14 c_3 = 7 c_4 = 3 c_5 = 2 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K_2Cr_2O_7 + 14 HI ⟶ 7 H_2O + 3 I_2 + 2 KI + 2 Cr_1I_3

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

potassium dichromate + hydrogen iodide ⟶ water + iodine + potassium iodide + chromium(III) iodide
potassium dichromate + hydrogen iodide ⟶ water + iodine + potassium iodide + chromium(III) iodide

Equilibrium constant

Construct the equilibrium constant, K, expression for: K_2Cr_2O_7 + HI ⟶ H_2O + I_2 + KI + Cr_1I_3 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: K_2Cr_2O_7 + 14 HI ⟶ 7 H_2O + 3 I_2 + 2 KI + 2 Cr_1I_3 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 K_2Cr_2O_7 | 1 | -1 HI | 14 | -14 H_2O | 7 | 7 I_2 | 3 | 3 KI | 2 | 2 Cr_1I_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2Cr_2O_7 | 1 | -1 | ([K2Cr2O7])^(-1) HI | 14 | -14 | ([HI])^(-14) H_2O | 7 | 7 | ([H2O])^7 I_2 | 3 | 3 | ([I2])^3 KI | 2 | 2 | ([KI])^2 Cr_1I_3 | 2 | 2 | ([Cr1I3])^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 = ([K2Cr2O7])^(-1) ([HI])^(-14) ([H2O])^7 ([I2])^3 ([KI])^2 ([Cr1I3])^2 = (([H2O])^7 ([I2])^3 ([KI])^2 ([Cr1I3])^2)/([K2Cr2O7] ([HI])^14)
Construct the equilibrium constant, K, expression for: K_2Cr_2O_7 + HI ⟶ H_2O + I_2 + KI + Cr_1I_3 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: K_2Cr_2O_7 + 14 HI ⟶ 7 H_2O + 3 I_2 + 2 KI + 2 Cr_1I_3 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 K_2Cr_2O_7 | 1 | -1 HI | 14 | -14 H_2O | 7 | 7 I_2 | 3 | 3 KI | 2 | 2 Cr_1I_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2Cr_2O_7 | 1 | -1 | ([K2Cr2O7])^(-1) HI | 14 | -14 | ([HI])^(-14) H_2O | 7 | 7 | ([H2O])^7 I_2 | 3 | 3 | ([I2])^3 KI | 2 | 2 | ([KI])^2 Cr_1I_3 | 2 | 2 | ([Cr1I3])^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 = ([K2Cr2O7])^(-1) ([HI])^(-14) ([H2O])^7 ([I2])^3 ([KI])^2 ([Cr1I3])^2 = (([H2O])^7 ([I2])^3 ([KI])^2 ([Cr1I3])^2)/([K2Cr2O7] ([HI])^14)

Rate of reaction

Construct the rate of reaction expression for: K_2Cr_2O_7 + HI ⟶ H_2O + I_2 + KI + Cr_1I_3 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: K_2Cr_2O_7 + 14 HI ⟶ 7 H_2O + 3 I_2 + 2 KI + 2 Cr_1I_3 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 K_2Cr_2O_7 | 1 | -1 HI | 14 | -14 H_2O | 7 | 7 I_2 | 3 | 3 KI | 2 | 2 Cr_1I_3 | 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 K_2Cr_2O_7 | 1 | -1 | -(Δ[K2Cr2O7])/(Δt) HI | 14 | -14 | -1/14 (Δ[HI])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(Δt) KI | 2 | 2 | 1/2 (Δ[KI])/(Δt) Cr_1I_3 | 2 | 2 | 1/2 (Δ[Cr1I3])/(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[K2Cr2O7])/(Δt) = -1/14 (Δ[HI])/(Δt) = 1/7 (Δ[H2O])/(Δt) = 1/3 (Δ[I2])/(Δt) = 1/2 (Δ[KI])/(Δt) = 1/2 (Δ[Cr1I3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: K_2Cr_2O_7 + HI ⟶ H_2O + I_2 + KI + Cr_1I_3 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: K_2Cr_2O_7 + 14 HI ⟶ 7 H_2O + 3 I_2 + 2 KI + 2 Cr_1I_3 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 K_2Cr_2O_7 | 1 | -1 HI | 14 | -14 H_2O | 7 | 7 I_2 | 3 | 3 KI | 2 | 2 Cr_1I_3 | 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 K_2Cr_2O_7 | 1 | -1 | -(Δ[K2Cr2O7])/(Δt) HI | 14 | -14 | -1/14 (Δ[HI])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) I_2 | 3 | 3 | 1/3 (Δ[I2])/(Δt) KI | 2 | 2 | 1/2 (Δ[KI])/(Δt) Cr_1I_3 | 2 | 2 | 1/2 (Δ[Cr1I3])/(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[K2Cr2O7])/(Δt) = -1/14 (Δ[HI])/(Δt) = 1/7 (Δ[H2O])/(Δt) = 1/3 (Δ[I2])/(Δt) = 1/2 (Δ[KI])/(Δt) = 1/2 (Δ[Cr1I3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium dichromate | hydrogen iodide | water | iodine | potassium iodide | chromium(III) iodide formula | K_2Cr_2O_7 | HI | H_2O | I_2 | KI | Cr_1I_3 Hill formula | Cr_2K_2O_7 | HI | H_2O | I_2 | IK | CrI_3 name | potassium dichromate | hydrogen iodide | water | iodine | potassium iodide | chromium(III) iodide IUPAC name | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | hydrogen iodide | water | molecular iodine | potassium iodide | triiodochromium
| potassium dichromate | hydrogen iodide | water | iodine | potassium iodide | chromium(III) iodide formula | K_2Cr_2O_7 | HI | H_2O | I_2 | KI | Cr_1I_3 Hill formula | Cr_2K_2O_7 | HI | H_2O | I_2 | IK | CrI_3 name | potassium dichromate | hydrogen iodide | water | iodine | potassium iodide | chromium(III) iodide IUPAC name | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | hydrogen iodide | water | molecular iodine | potassium iodide | triiodochromium

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