Input interpretation
H_2O water + I2O7 ⟶ HIO4
Balanced equation
Balance the chemical equation algebraically: H_2O + I2O7 ⟶ HIO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 I2O7 ⟶ c_3 HIO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and I: H: | 2 c_1 = c_3 O: | c_1 + 7 c_2 = 4 c_3 I: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + I2O7 ⟶ 2 HIO4
Structures
+ I2O7 ⟶ HIO4
Names
water + I2O7 ⟶ HIO4
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2O + I2O7 ⟶ HIO4 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 + I2O7 ⟶ 2 HIO4 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 I2O7 | 1 | -1 HIO4 | 2 | 2 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) I2O7 | 1 | -1 | ([I2O7])^(-1) HIO4 | 2 | 2 | ([HIO4])^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 = ([H2O])^(-1) ([I2O7])^(-1) ([HIO4])^2 = ([HIO4])^2/([H2O] [I2O7])](../image_source/eceb0cb448b0c9aca89e5621d38ecc21.png)
Construct the equilibrium constant, K, expression for: H_2O + I2O7 ⟶ HIO4 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 + I2O7 ⟶ 2 HIO4 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 I2O7 | 1 | -1 HIO4 | 2 | 2 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) I2O7 | 1 | -1 | ([I2O7])^(-1) HIO4 | 2 | 2 | ([HIO4])^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 = ([H2O])^(-1) ([I2O7])^(-1) ([HIO4])^2 = ([HIO4])^2/([H2O] [I2O7])
Rate of reaction
![Construct the rate of reaction expression for: H_2O + I2O7 ⟶ HIO4 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 + I2O7 ⟶ 2 HIO4 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 I2O7 | 1 | -1 HIO4 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) I2O7 | 1 | -1 | -(Δ[I2O7])/(Δt) HIO4 | 2 | 2 | 1/2 (Δ[HIO4])/(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) = -(Δ[I2O7])/(Δt) = 1/2 (Δ[HIO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/d7adc9d13fc45b9fcfff4476970feecf.png)
Construct the rate of reaction expression for: H_2O + I2O7 ⟶ HIO4 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 + I2O7 ⟶ 2 HIO4 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 I2O7 | 1 | -1 HIO4 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) I2O7 | 1 | -1 | -(Δ[I2O7])/(Δt) HIO4 | 2 | 2 | 1/2 (Δ[HIO4])/(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) = -(Δ[I2O7])/(Δt) = 1/2 (Δ[HIO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| water | I2O7 | HIO4 formula | H_2O | I2O7 | HIO4 name | water | |
Substance properties
| water | I2O7 | HIO4 molar mass | 18.015 g/mol | 365.8 g/mol | 191.91 g/mol phase | liquid (at STP) | | melting point | 0 °C | | boiling point | 99.9839 °C | | density | 1 g/cm^3 | | surface tension | 0.0728 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | |
Units
