Input interpretation
SO_2 sulfur dioxide + Ca(OH)_2 calcium hydroxide ⟶ H_2O water + CaSO3
Balanced equation
Balance the chemical equation algebraically: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SO_2 + c_2 Ca(OH)_2 ⟶ c_3 H_2O + c_4 CaSO3 Set the number of atoms in the reactants equal to the number of atoms in the products for O, S, Ca and H: O: | 2 c_1 + 2 c_2 = c_3 + 3 c_4 S: | c_1 = c_4 Ca: | c_2 = c_4 H: | 2 c_2 = 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: | | SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3
Structures
+ ⟶ + CaSO3
Names
sulfur dioxide + calcium hydroxide ⟶ water + CaSO3
Equilibrium constant
![Construct the equilibrium constant, K, expression for: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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 SO_2 | 1 | -1 Ca(OH)_2 | 1 | -1 H_2O | 1 | 1 CaSO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SO_2 | 1 | -1 | ([SO2])^(-1) Ca(OH)_2 | 1 | -1 | ([Ca(OH)2])^(-1) H_2O | 1 | 1 | [H2O] CaSO3 | 1 | 1 | [CaSO3] 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 = ([SO2])^(-1) ([Ca(OH)2])^(-1) [H2O] [CaSO3] = ([H2O] [CaSO3])/([SO2] [Ca(OH)2])](../image_source/99ca0e0a5d90d5b8bca230c363982186.png)
Construct the equilibrium constant, K, expression for: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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 SO_2 | 1 | -1 Ca(OH)_2 | 1 | -1 H_2O | 1 | 1 CaSO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SO_2 | 1 | -1 | ([SO2])^(-1) Ca(OH)_2 | 1 | -1 | ([Ca(OH)2])^(-1) H_2O | 1 | 1 | [H2O] CaSO3 | 1 | 1 | [CaSO3] 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 = ([SO2])^(-1) ([Ca(OH)2])^(-1) [H2O] [CaSO3] = ([H2O] [CaSO3])/([SO2] [Ca(OH)2])
Rate of reaction
![Construct the rate of reaction expression for: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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 SO_2 | 1 | -1 Ca(OH)_2 | 1 | -1 H_2O | 1 | 1 CaSO3 | 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 SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) Ca(OH)_2 | 1 | -1 | -(Δ[Ca(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CaSO3 | 1 | 1 | (Δ[CaSO3])/(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[SO2])/(Δt) = -(Δ[Ca(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CaSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/fc839454a866e11d4b95a466d6eb7d79.png)
Construct the rate of reaction expression for: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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: SO_2 + Ca(OH)_2 ⟶ H_2O + CaSO3 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 SO_2 | 1 | -1 Ca(OH)_2 | 1 | -1 H_2O | 1 | 1 CaSO3 | 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 SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) Ca(OH)_2 | 1 | -1 | -(Δ[Ca(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CaSO3 | 1 | 1 | (Δ[CaSO3])/(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[SO2])/(Δt) = -(Δ[Ca(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CaSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| sulfur dioxide | calcium hydroxide | water | CaSO3 formula | SO_2 | Ca(OH)_2 | H_2O | CaSO3 Hill formula | O_2S | CaH_2O_2 | H_2O | CaO3S name | sulfur dioxide | calcium hydroxide | water | IUPAC name | sulfur dioxide | calcium dihydroxide | water |