Na2SCaCO3 = Na2CO3CaS

Na2SCaCO3 ⟶ Na2CO3CaS

Balance the chemical equation algebraically: Na2SCaCO3 ⟶ Na2CO3CaS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Na2SCaCO3 ⟶ c_2 Na2CO3CaS Set the number of atoms in the reactants equal to the number of atoms in the products for Na, S, Ca, C and O: Na: | 2 c_1 = 2 c_2 S: | c_1 = c_2 Ca: | c_1 = c_2 C: | c_1 = c_2 O: | 3 c_1 = 3 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: | | Na2SCaCO3 ⟶ Na2CO3CaS

Na2SCaCO3 ⟶ Na2CO3CaS

Na2SCaCO3 ⟶ Na2CO3CaS

Construct the equilibrium constant, K, expression for: Na2SCaCO3 ⟶ Na2CO3CaS 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: Na2SCaCO3 ⟶ Na2CO3CaS 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 Na2SCaCO3 | 1 | -1 Na2CO3CaS | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Na2SCaCO3 | 1 | -1 | ([Na2SCaCO3])^(-1) Na2CO3CaS | 1 | 1 | [Na2CO3CaS] 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 = ([Na2SCaCO3])^(-1) [Na2CO3CaS] = ([Na2CO3CaS])/([Na2SCaCO3])

Construct the rate of reaction expression for: Na2SCaCO3 ⟶ Na2CO3CaS 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: Na2SCaCO3 ⟶ Na2CO3CaS 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 Na2SCaCO3 | 1 | -1 Na2CO3CaS | 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 Na2SCaCO3 | 1 | -1 | -(Δ[Na2SCaCO3])/(Δt) Na2CO3CaS | 1 | 1 | (Δ[Na2CO3CaS])/(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[Na2SCaCO3])/(Δt) = (Δ[Na2CO3CaS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| Na2SCaCO3 | Na2CO3CaS formula | Na2SCaCO3 | Na2CO3CaS Hill formula | CCaNa2O3S | CCaNa2O3S

| Na2SCaCO3 | Na2CO3CaS molar mass | 178.13 g/mol | 178.13 g/mol