SnSO4 = SO2 + SnO2

SnSO_4 stannous sulfate ⟶ SO_2 sulfur dioxide + SnO_2 stannic oxide

Balance the chemical equation algebraically: SnSO_4 ⟶ SO_2 + SnO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SnSO_4 ⟶ c_2 SO_2 + c_3 SnO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for O, S and Sn: O: | 4 c_1 = 2 c_2 + 2 c_3 S: | c_1 = c_2 Sn: | c_1 = 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SnSO_4 ⟶ SO_2 + SnO_2

⟶ +

stannous sulfate ⟶ sulfur dioxide + stannic oxide

Construct the equilibrium constant, K, expression for: SnSO_4 ⟶ SO_2 + SnO_2 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: SnSO_4 ⟶ SO_2 + SnO_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 SnSO_4 | 1 | -1 SO_2 | 1 | 1 SnO_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnSO_4 | 1 | -1 | ([SnSO4])^(-1) SO_2 | 1 | 1 | [SO2] SnO_2 | 1 | 1 | [SnO2] 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 = ([SnSO4])^(-1) [SO2] [SnO2] = ([SO2] [SnO2])/([SnSO4])

Construct the rate of reaction expression for: SnSO_4 ⟶ SO_2 + SnO_2 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: SnSO_4 ⟶ SO_2 + SnO_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 SnSO_4 | 1 | -1 SO_2 | 1 | 1 SnO_2 | 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 SnSO_4 | 1 | -1 | -(Δ[SnSO4])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) SnO_2 | 1 | 1 | (Δ[SnO2])/(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[SnSO4])/(Δt) = (Δ[SO2])/(Δt) = (Δ[SnO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| stannous sulfate | sulfur dioxide | stannic oxide formula | SnSO_4 | SO_2 | SnO_2 Hill formula | O_4SSn | O_2S | O_2Sn name | stannous sulfate | sulfur dioxide | stannic oxide IUPAC name | tin(+2) cation sulfate | sulfur dioxide |

| stannous sulfate | sulfur dioxide | stannic oxide molar mass | 214.77 g/mol | 64.06 g/mol | 150.708 g/mol phase | | gas (at STP) | solid (at STP) melting point | | -73 °C | 1624.85 °C boiling point | | -10 °C | 2500 °C density | 4.15 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | 6.95 g/cm^3 solubility in water | soluble | | insoluble surface tension | | 0.02859 N/m | dynamic viscosity | | 1.282×10^-5 Pa s (at 25 °C) |