Input interpretation
H2I2 ⟶ HI hydrogen iodide
Balanced equation
Balance the chemical equation algebraically: H2I2 ⟶ HI Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H2I2 ⟶ c_2 HI Set the number of atoms in the reactants equal to the number of atoms in the products for H and I: H: | 2 c_1 = c_2 I: | 2 c_1 = c_2 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H2I2 ⟶ 2 HI
Structures
H2I2 ⟶
Names
H2I2 ⟶ hydrogen iodide
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H2I2 ⟶ HI 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: H2I2 ⟶ 2 HI 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 H2I2 | 1 | -1 HI | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H2I2 | 1 | -1 | ([H2I2])^(-1) HI | 2 | 2 | ([HI])^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 = ([H2I2])^(-1) ([HI])^2 = ([HI])^2/([H2I2])](../image_source/9f635cc197a293958ddf3e9c37f8ab07.png)
Construct the equilibrium constant, K, expression for: H2I2 ⟶ HI 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: H2I2 ⟶ 2 HI 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 H2I2 | 1 | -1 HI | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H2I2 | 1 | -1 | ([H2I2])^(-1) HI | 2 | 2 | ([HI])^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 = ([H2I2])^(-1) ([HI])^2 = ([HI])^2/([H2I2])
Rate of reaction
![Construct the rate of reaction expression for: H2I2 ⟶ HI 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: H2I2 ⟶ 2 HI 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 H2I2 | 1 | -1 HI | 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 H2I2 | 1 | -1 | -(Δ[H2I2])/(Δt) HI | 2 | 2 | 1/2 (Δ[HI])/(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[H2I2])/(Δt) = 1/2 (Δ[HI])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/20cb886f52b998d6021dea5ec7e5a60f.png)
Construct the rate of reaction expression for: H2I2 ⟶ HI 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: H2I2 ⟶ 2 HI 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 H2I2 | 1 | -1 HI | 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 H2I2 | 1 | -1 | -(Δ[H2I2])/(Δt) HI | 2 | 2 | 1/2 (Δ[HI])/(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[H2I2])/(Δt) = 1/2 (Δ[HI])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| H2I2 | hydrogen iodide formula | H2I2 | HI name | | hydrogen iodide
Substance properties
| H2I2 | hydrogen iodide molar mass | 255.825 g/mol | 127.912 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
