Input interpretation
HI hydrogen iodide + HIO4 ⟶ I2H2O
Balanced equation
Balance the chemical equation algebraically: HI + HIO4 ⟶ I2H2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HI + c_2 HIO4 ⟶ c_3 I2H2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, I and O: H: | c_1 + c_2 = 2 c_3 I: | c_1 + c_2 = 2 c_3 O: | 4 c_2 = c_3 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 = 7 c_2 = 1 c_3 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 7 HI + HIO4 ⟶ 4 I2H2O
Structures
+ HIO4 ⟶ I2H2O
Names
hydrogen iodide + HIO4 ⟶ I2H2O
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HI + HIO4 ⟶ I2H2O 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: 7 HI + HIO4 ⟶ 4 I2H2O 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 HI | 7 | -7 HIO4 | 1 | -1 I2H2O | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HI | 7 | -7 | ([HI])^(-7) HIO4 | 1 | -1 | ([HIO4])^(-1) I2H2O | 4 | 4 | ([I2H2O])^4 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 = ([HI])^(-7) ([HIO4])^(-1) ([I2H2O])^4 = ([I2H2O])^4/(([HI])^7 [HIO4])](../image_source/82c278cf3d442b9c21b59c1366e2c9a2.png)
Construct the equilibrium constant, K, expression for: HI + HIO4 ⟶ I2H2O 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: 7 HI + HIO4 ⟶ 4 I2H2O 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 HI | 7 | -7 HIO4 | 1 | -1 I2H2O | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HI | 7 | -7 | ([HI])^(-7) HIO4 | 1 | -1 | ([HIO4])^(-1) I2H2O | 4 | 4 | ([I2H2O])^4 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 = ([HI])^(-7) ([HIO4])^(-1) ([I2H2O])^4 = ([I2H2O])^4/(([HI])^7 [HIO4])
Rate of reaction
![Construct the rate of reaction expression for: HI + HIO4 ⟶ I2H2O 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: 7 HI + HIO4 ⟶ 4 I2H2O 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 HI | 7 | -7 HIO4 | 1 | -1 I2H2O | 4 | 4 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 HI | 7 | -7 | -1/7 (Δ[HI])/(Δt) HIO4 | 1 | -1 | -(Δ[HIO4])/(Δt) I2H2O | 4 | 4 | 1/4 (Δ[I2H2O])/(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 = -1/7 (Δ[HI])/(Δt) = -(Δ[HIO4])/(Δt) = 1/4 (Δ[I2H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/cf8c875272445c829b8cb7030a76875a.png)
Construct the rate of reaction expression for: HI + HIO4 ⟶ I2H2O 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: 7 HI + HIO4 ⟶ 4 I2H2O 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 HI | 7 | -7 HIO4 | 1 | -1 I2H2O | 4 | 4 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 HI | 7 | -7 | -1/7 (Δ[HI])/(Δt) HIO4 | 1 | -1 | -(Δ[HIO4])/(Δt) I2H2O | 4 | 4 | 1/4 (Δ[I2H2O])/(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 = -1/7 (Δ[HI])/(Δt) = -(Δ[HIO4])/(Δt) = 1/4 (Δ[I2H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| hydrogen iodide | HIO4 | I2H2O formula | HI | HIO4 | I2H2O Hill formula | HI | HIO4 | H2I2O name | hydrogen iodide | |
Substance properties
| hydrogen iodide | HIO4 | I2H2O molar mass | 127.912 g/mol | 191.91 g/mol | 271.824 g/mol phase | gas (at STP) | | melting point | -50.76 °C | | boiling point | -35.55 °C | | density | 0.005228 g/cm^3 (at 25 °C) | | solubility in water | very soluble | | dynamic viscosity | 0.001321 Pa s (at -39 °C) | |
Units
