HCl + CuSO4 = H2SO4 + CuCl2

hydrogen chloride + copper(II) sulfate ⟶ sulfuric acid + copper(II) chloride

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

+ ⟶ +

hydrogen chloride + copper(II) sulfate ⟶ sulfuric acid + copper(II) chloride

| hydrogen chloride | copper(II) sulfate | sulfuric acid | copper(II) chloride molecular enthalpy | -92.3 kJ/mol | -771.4 kJ/mol | -814 kJ/mol | -220.1 kJ/mol total enthalpy | -184.6 kJ/mol | -771.4 kJ/mol | -814 kJ/mol | -220.1 kJ/mol | H_initial = -956 kJ/mol | | H_final = -1034 kJ/mol | ΔH_rxn^0 | -1034 kJ/mol - -956 kJ/mol = -78.1 kJ/mol (exothermic) | | |

| hydrogen chloride | copper(II) sulfate | sulfuric acid | copper(II) chloride molecular free energy | -95.3 kJ/mol | -662.2 kJ/mol | -690 kJ/mol | -175.7 kJ/mol total free energy | -190.6 kJ/mol | -662.2 kJ/mol | -690 kJ/mol | -175.7 kJ/mol | G_initial = -852.8 kJ/mol | | G_final = -865.7 kJ/mol | ΔG_rxn^0 | -865.7 kJ/mol - -852.8 kJ/mol = -12.9 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: + ⟶ + 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: 2 + ⟶ + 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 | 2 | -2 | 1 | -1 | 1 | 1 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression | 2 | -2 | ([HCl])^(-2) | 1 | -1 | ([CuSO4])^(-1) | 1 | 1 | [H2SO4] | 1 | 1 | [CuCl2] 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 = ([HCl])^(-2) ([CuSO4])^(-1) [H2SO4] [CuCl2] = ([H2SO4] [CuCl2])/(([HCl])^2 [CuSO4])

Construct the rate of reaction expression for: + ⟶ + 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: 2 + ⟶ + 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 | 2 | -2 | 1 | -1 | 1 | 1 | 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) | 1 | -1 | -(Δ[CuSO4])/(Δt) | 1 | 1 | (Δ[H2SO4])/(Δt) | 1 | 1 | (Δ[CuCl2])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[CuSO4])/(Δt) = (Δ[H2SO4])/(Δt) = (Δ[CuCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | copper(II) sulfate | sulfuric acid | copper(II) chloride Hill formula | ClH | CuO_4S | H_2O_4S | Cl_2Cu name | hydrogen chloride | copper(II) sulfate | sulfuric acid | copper(II) chloride IUPAC name | hydrogen chloride | copper sulfate | sulfuric acid | dichlorocopper

| hydrogen chloride | copper(II) sulfate | sulfuric acid | copper(II) chloride molar mass | 36.46 g/mol | 159.6 g/mol | 98.07 g/mol | 134.4 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 200 °C | 10.371 °C | 620 °C boiling point | -85 °C | | 279.6 °C | density | 0.00149 g/cm^3 (at 25 °C) | 3.603 g/cm^3 | 1.8305 g/cm^3 | 3.386 g/cm^3 solubility in water | miscible | | very soluble | surface tension | | | 0.0735 N/m | dynamic viscosity | | | 0.021 Pa s (at 25 °C) | odor | | | odorless |