H2Cl2 = HCl

H2Cl2 ⟶ HCl (hydrogen chloride)

Balance the chemical equation algebraically: H2Cl2 ⟶ HCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H2Cl2 ⟶ c_2 HCl Set the number of atoms in the reactants equal to the number of atoms in the products for H and Cl: H: | 2 c_1 = c_2 Cl: | 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: | | H2Cl2 ⟶ 2 HCl

H2Cl2 ⟶

H2Cl2 ⟶ hydrogen chloride

Construct the equilibrium constant, K, expression for: H2Cl2 ⟶ HCl 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: H2Cl2 ⟶ 2 HCl 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 H2Cl2 | 1 | -1 HCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H2Cl2 | 1 | -1 | ([H2Cl2])^(-1) HCl | 2 | 2 | ([HCl])^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 = ([H2Cl2])^(-1) ([HCl])^2 = ([HCl])^2/([H2Cl2])

Construct the rate of reaction expression for: H2Cl2 ⟶ HCl 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: H2Cl2 ⟶ 2 HCl 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 H2Cl2 | 1 | -1 HCl | 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 H2Cl2 | 1 | -1 | -(Δ[H2Cl2])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(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[H2Cl2])/(Δt) = 1/2 (Δ[HCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| H2Cl2 | hydrogen chloride formula | H2Cl2 | HCl Hill formula | H2Cl2 | ClH name | | hydrogen chloride

| H2Cl2 | hydrogen chloride molar mass | 72.92 g/mol | 36.46 g/mol phase | | gas (at STP) melting point | | -114.17 °C boiling point | | -85 °C density | | 0.00149 g/cm^3 (at 25 °C) solubility in water | | miscible