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H2SO4 + CaCl2 = HCl + CaSO4

Input interpretation

H_2SO_4 sulfuric acid + CaCl_2 calcium chloride ⟶ HCl hydrogen chloride + CaSO_4 calcium sulfate
H_2SO_4 sulfuric acid + CaCl_2 calcium chloride ⟶ HCl hydrogen chloride + CaSO_4 calcium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + CaCl_2 ⟶ HCl + CaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CaCl_2 ⟶ c_3 HCl + c_4 CaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Ca and Cl: H: | 2 c_1 = c_3 O: | 4 c_1 = 4 c_4 S: | c_1 = c_4 Ca: | c_2 = c_4 Cl: | 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 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + CaCl_2 ⟶ 2 HCl + CaSO_4
Balance the chemical equation algebraically: H_2SO_4 + CaCl_2 ⟶ HCl + CaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CaCl_2 ⟶ c_3 HCl + c_4 CaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Ca and Cl: H: | 2 c_1 = c_3 O: | 4 c_1 = 4 c_4 S: | c_1 = c_4 Ca: | c_2 = c_4 Cl: | 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 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + CaCl_2 ⟶ 2 HCl + CaSO_4

Structures

+ ⟶ +
+ ⟶ +

Names

sulfuric acid + calcium chloride ⟶ hydrogen chloride + calcium sulfate
sulfuric acid + calcium chloride ⟶ hydrogen chloride + calcium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + CaCl_2 ⟶ HCl + CaSO_4 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_2SO_4 + CaCl_2 ⟶ 2 HCl + CaSO_4 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_2SO_4 | 1 | -1 CaCl_2 | 1 | -1 HCl | 2 | 2 CaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) CaCl_2 | 1 | -1 | ([CaCl2])^(-1) HCl | 2 | 2 | ([HCl])^2 CaSO_4 | 1 | 1 | [CaSO4] 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 = ([H2SO4])^(-1) ([CaCl2])^(-1) ([HCl])^2 [CaSO4] = (([HCl])^2 [CaSO4])/([H2SO4] [CaCl2])
Construct the equilibrium constant, K, expression for: H_2SO_4 + CaCl_2 ⟶ HCl + CaSO_4 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_2SO_4 + CaCl_2 ⟶ 2 HCl + CaSO_4 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_2SO_4 | 1 | -1 CaCl_2 | 1 | -1 HCl | 2 | 2 CaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) CaCl_2 | 1 | -1 | ([CaCl2])^(-1) HCl | 2 | 2 | ([HCl])^2 CaSO_4 | 1 | 1 | [CaSO4] 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 = ([H2SO4])^(-1) ([CaCl2])^(-1) ([HCl])^2 [CaSO4] = (([HCl])^2 [CaSO4])/([H2SO4] [CaCl2])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + CaCl_2 ⟶ HCl + CaSO_4 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_2SO_4 + CaCl_2 ⟶ 2 HCl + CaSO_4 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_2SO_4 | 1 | -1 CaCl_2 | 1 | -1 HCl | 2 | 2 CaSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) CaCl_2 | 1 | -1 | -(Δ[CaCl2])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) CaSO_4 | 1 | 1 | (Δ[CaSO4])/(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[H2SO4])/(Δt) = -(Δ[CaCl2])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[CaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + CaCl_2 ⟶ HCl + CaSO_4 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_2SO_4 + CaCl_2 ⟶ 2 HCl + CaSO_4 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_2SO_4 | 1 | -1 CaCl_2 | 1 | -1 HCl | 2 | 2 CaSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) CaCl_2 | 1 | -1 | -(Δ[CaCl2])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) CaSO_4 | 1 | 1 | (Δ[CaSO4])/(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[H2SO4])/(Δt) = -(Δ[CaCl2])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[CaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | calcium chloride | hydrogen chloride | calcium sulfate formula | H_2SO_4 | CaCl_2 | HCl | CaSO_4 Hill formula | H_2O_4S | CaCl_2 | ClH | CaO_4S name | sulfuric acid | calcium chloride | hydrogen chloride | calcium sulfate IUPAC name | sulfuric acid | calcium dichloride | hydrogen chloride | calcium sulfate
| sulfuric acid | calcium chloride | hydrogen chloride | calcium sulfate formula | H_2SO_4 | CaCl_2 | HCl | CaSO_4 Hill formula | H_2O_4S | CaCl_2 | ClH | CaO_4S name | sulfuric acid | calcium chloride | hydrogen chloride | calcium sulfate IUPAC name | sulfuric acid | calcium dichloride | hydrogen chloride | calcium sulfate

Substance properties

| sulfuric acid | calcium chloride | hydrogen chloride | calcium sulfate molar mass | 98.07 g/mol | 111 g/mol | 36.46 g/mol | 136.13 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 10.371 °C | 772 °C | -114.17 °C | boiling point | 279.6 °C | | -85 °C | density | 1.8305 g/cm^3 | 2.15 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | solubility in water | very soluble | soluble | miscible | slightly soluble surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | | odor | odorless | | | odorless
| sulfuric acid | calcium chloride | hydrogen chloride | calcium sulfate molar mass | 98.07 g/mol | 111 g/mol | 36.46 g/mol | 136.13 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 10.371 °C | 772 °C | -114.17 °C | boiling point | 279.6 °C | | -85 °C | density | 1.8305 g/cm^3 | 2.15 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | solubility in water | very soluble | soluble | miscible | slightly soluble surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | | odor | odorless | | | odorless

Units

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