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HI + CH3OH = H2O + CH3I

Input interpretation

HI hydrogen iodide + CH_3OH methanol ⟶ H_2O water + CH_3I methyl iodide
HI hydrogen iodide + CH_3OH methanol ⟶ H_2O water + CH_3I methyl iodide

Balanced equation

Balance the chemical equation algebraically: HI + CH_3OH ⟶ H_2O + CH_3I Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HI + c_2 CH_3OH ⟶ c_3 H_2O + c_4 CH_3I Set the number of atoms in the reactants equal to the number of atoms in the products for H, I, C and O: H: | c_1 + 4 c_2 = 2 c_3 + 3 c_4 I: | c_1 = c_4 C: | c_2 = c_4 O: | 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | HI + CH_3OH ⟶ H_2O + CH_3I
Balance the chemical equation algebraically: HI + CH_3OH ⟶ H_2O + CH_3I Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HI + c_2 CH_3OH ⟶ c_3 H_2O + c_4 CH_3I Set the number of atoms in the reactants equal to the number of atoms in the products for H, I, C and O: H: | c_1 + 4 c_2 = 2 c_3 + 3 c_4 I: | c_1 = c_4 C: | c_2 = c_4 O: | 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | HI + CH_3OH ⟶ H_2O + CH_3I

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen iodide + methanol ⟶ water + methyl iodide
hydrogen iodide + methanol ⟶ water + methyl iodide

Equilibrium constant

Construct the equilibrium constant, K, expression for: HI + CH_3OH ⟶ H_2O + CH_3I 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: HI + CH_3OH ⟶ H_2O + CH_3I 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 | 1 | -1 CH_3OH | 1 | -1 H_2O | 1 | 1 CH_3I | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HI | 1 | -1 | ([HI])^(-1) CH_3OH | 1 | -1 | ([CH3OH])^(-1) H_2O | 1 | 1 | [H2O] CH_3I | 1 | 1 | [CH3I] 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])^(-1) ([CH3OH])^(-1) [H2O] [CH3I] = ([H2O] [CH3I])/([HI] [CH3OH])
Construct the equilibrium constant, K, expression for: HI + CH_3OH ⟶ H_2O + CH_3I 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: HI + CH_3OH ⟶ H_2O + CH_3I 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 | 1 | -1 CH_3OH | 1 | -1 H_2O | 1 | 1 CH_3I | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HI | 1 | -1 | ([HI])^(-1) CH_3OH | 1 | -1 | ([CH3OH])^(-1) H_2O | 1 | 1 | [H2O] CH_3I | 1 | 1 | [CH3I] 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])^(-1) ([CH3OH])^(-1) [H2O] [CH3I] = ([H2O] [CH3I])/([HI] [CH3OH])

Rate of reaction

Construct the rate of reaction expression for: HI + CH_3OH ⟶ H_2O + CH_3I 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: HI + CH_3OH ⟶ H_2O + CH_3I 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 | 1 | -1 CH_3OH | 1 | -1 H_2O | 1 | 1 CH_3I | 1 | 1 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 | 1 | -1 | -(Δ[HI])/(Δt) CH_3OH | 1 | -1 | -(Δ[CH3OH])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CH_3I | 1 | 1 | (Δ[CH3I])/(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[HI])/(Δt) = -(Δ[CH3OH])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CH3I])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HI + CH_3OH ⟶ H_2O + CH_3I 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: HI + CH_3OH ⟶ H_2O + CH_3I 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 | 1 | -1 CH_3OH | 1 | -1 H_2O | 1 | 1 CH_3I | 1 | 1 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 | 1 | -1 | -(Δ[HI])/(Δt) CH_3OH | 1 | -1 | -(Δ[CH3OH])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CH_3I | 1 | 1 | (Δ[CH3I])/(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[HI])/(Δt) = -(Δ[CH3OH])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CH3I])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen iodide | methanol | water | methyl iodide formula | HI | CH_3OH | H_2O | CH_3I Hill formula | HI | CH_4O | H_2O | CH_3I name | hydrogen iodide | methanol | water | methyl iodide IUPAC name | hydrogen iodide | methanol | water | iodomethane
| hydrogen iodide | methanol | water | methyl iodide formula | HI | CH_3OH | H_2O | CH_3I Hill formula | HI | CH_4O | H_2O | CH_3I name | hydrogen iodide | methanol | water | methyl iodide IUPAC name | hydrogen iodide | methanol | water | iodomethane

Substance properties

| hydrogen iodide | methanol | water | methyl iodide molar mass | 127.912 g/mol | 32.042 g/mol | 18.015 g/mol | 141.939 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | liquid (at STP) melting point | -50.76 °C | -98 °C | 0 °C | -66.4 °C boiling point | -35.55 °C | 64.7 °C | 99.9839 °C | 42.43 °C density | 0.005228 g/cm^3 (at 25 °C) | 0.791 g/cm^3 | 1 g/cm^3 | 2.2789 g/cm^3 solubility in water | very soluble | miscible | | surface tension | | | 0.0728 N/m | 0.0258 N/m dynamic viscosity | 0.001321 Pa s (at -39 °C) | 5.44×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | 4.69×10^-4 Pa s (at 25 °C) odor | | pungent | odorless |
| hydrogen iodide | methanol | water | methyl iodide molar mass | 127.912 g/mol | 32.042 g/mol | 18.015 g/mol | 141.939 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | liquid (at STP) melting point | -50.76 °C | -98 °C | 0 °C | -66.4 °C boiling point | -35.55 °C | 64.7 °C | 99.9839 °C | 42.43 °C density | 0.005228 g/cm^3 (at 25 °C) | 0.791 g/cm^3 | 1 g/cm^3 | 2.2789 g/cm^3 solubility in water | very soluble | miscible | | surface tension | | | 0.0728 N/m | 0.0258 N/m dynamic viscosity | 0.001321 Pa s (at -39 °C) | 5.44×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | 4.69×10^-4 Pa s (at 25 °C) odor | | pungent | odorless |

Units

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