O2 + SnS2 = SO2 + SnO2

O_2 oxygen + SnS_2 tin(IV) sulfide ⟶ SO_2 sulfur dioxide + SnO_2 stannic oxide

Balance the chemical equation algebraically: O_2 + SnS_2 ⟶ SO_2 + SnO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 SnS_2 ⟶ c_3 SO_2 + c_4 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: | 2 c_1 = 2 c_3 + 2 c_4 S: | 2 c_2 = c_3 Sn: | c_2 = c_4 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 = 3 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 O_2 + SnS_2 ⟶ 2 SO_2 + SnO_2

+ ⟶ +

oxygen + tin(IV) sulfide ⟶ sulfur dioxide + stannic oxide

Construct the equilibrium constant, K, expression for: O_2 + SnS_2 ⟶ 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: 3 O_2 + SnS_2 ⟶ 2 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 O_2 | 3 | -3 SnS_2 | 1 | -1 SO_2 | 2 | 2 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 O_2 | 3 | -3 | ([O2])^(-3) SnS_2 | 1 | -1 | ([SnS2])^(-1) SO_2 | 2 | 2 | ([SO2])^2 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 = ([O2])^(-3) ([SnS2])^(-1) ([SO2])^2 [SnO2] = (([SO2])^2 [SnO2])/(([O2])^3 [SnS2])

Construct the rate of reaction expression for: O_2 + SnS_2 ⟶ 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: 3 O_2 + SnS_2 ⟶ 2 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 O_2 | 3 | -3 SnS_2 | 1 | -1 SO_2 | 2 | 2 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 O_2 | 3 | -3 | -1/3 (Δ[O2])/(Δt) SnS_2 | 1 | -1 | -(Δ[SnS2])/(Δt) SO_2 | 2 | 2 | 1/2 (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 = -1/3 (Δ[O2])/(Δt) = -(Δ[SnS2])/(Δt) = 1/2 (Δ[SO2])/(Δt) = (Δ[SnO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | tin(IV) sulfide | sulfur dioxide | stannic oxide formula | O_2 | SnS_2 | SO_2 | SnO_2 Hill formula | O_2 | S_2Sn | O_2S | O_2Sn name | oxygen | tin(IV) sulfide | sulfur dioxide | stannic oxide IUPAC name | molecular oxygen | tin(+4) cation disulfide | sulfur dioxide |

| oxygen | tin(IV) sulfide | sulfur dioxide | stannic oxide molar mass | 31.998 g/mol | 182.8 g/mol | 64.06 g/mol | 150.708 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -218 °C | 600 °C | -73 °C | 1624.85 °C boiling point | -183 °C | | -10 °C | 2500 °C density | 0.001429 g/cm^3 (at 0 °C) | 4.5 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | 6.95 g/cm^3 solubility in water | | insoluble | | insoluble surface tension | 0.01347 N/m | | 0.02859 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | 1.282×10^-5 Pa s (at 25 °C) | odor | odorless | | |