SnSiO3CaOC = SnCaSiO3CO

SnSiO3CaOC ⟶ SnCaSiO3CO

Balance the chemical equation algebraically: SnSiO3CaOC ⟶ SnCaSiO3CO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SnSiO3CaOC ⟶ c_2 SnCaSiO3CO Set the number of atoms in the reactants equal to the number of atoms in the products for Sn, Si, O, Ca and C: Sn: | c_1 = c_2 Si: | c_1 = c_2 O: | 4 c_1 = 4 c_2 Ca: | c_1 = c_2 C: | c_1 = c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SnSiO3CaOC ⟶ SnCaSiO3CO

SnSiO3CaOC ⟶ SnCaSiO3CO

SnSiO3CaOC ⟶ SnCaSiO3CO

Construct the equilibrium constant, K, expression for: SnSiO3CaOC ⟶ SnCaSiO3CO 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: SnSiO3CaOC ⟶ SnCaSiO3CO 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 SnSiO3CaOC | 1 | -1 SnCaSiO3CO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnSiO3CaOC | 1 | -1 | ([SnSiO3CaOC])^(-1) SnCaSiO3CO | 1 | 1 | [SnCaSiO3CO] 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 = ([SnSiO3CaOC])^(-1) [SnCaSiO3CO] = ([SnCaSiO3CO])/([SnSiO3CaOC])

Construct the rate of reaction expression for: SnSiO3CaOC ⟶ SnCaSiO3CO 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: SnSiO3CaOC ⟶ SnCaSiO3CO 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 SnSiO3CaOC | 1 | -1 SnCaSiO3CO | 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 SnSiO3CaOC | 1 | -1 | -(Δ[SnSiO3CaOC])/(Δt) SnCaSiO3CO | 1 | 1 | (Δ[SnCaSiO3CO])/(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[SnSiO3CaOC])/(Δt) = (Δ[SnCaSiO3CO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| SnSiO3CaOC | SnCaSiO3CO formula | SnSiO3CaOC | SnCaSiO3CO Hill formula | CCaO4SiSn | CCaO4SiSn

| SnSiO3CaOC | SnCaSiO3CO molar mass | 262.88 g/mol | 262.88 g/mol