Input interpretation
HCl hydrogen chloride + NaI sodium iodide + Na_2TeO_3 sodium tellurite ⟶ H_2O water + I_2 iodine + NaCl sodium chloride + Te tellurium
Balanced equation
Balance the chemical equation algebraically: HCl + NaI + Na_2TeO_3 ⟶ H_2O + I_2 + NaCl + Te Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaI + c_3 Na_2TeO_3 ⟶ c_4 H_2O + c_5 I_2 + c_6 NaCl + c_7 Te Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, I, Na, O and Te: Cl: | c_1 = c_6 H: | c_1 = 2 c_4 I: | c_2 = 2 c_5 Na: | c_2 + 2 c_3 = c_6 O: | 3 c_3 = c_4 Te: | c_3 = c_7 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 4 c_3 = 1 c_4 = 3 c_5 = 2 c_6 = 6 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 4 NaI + Na_2TeO_3 ⟶ 3 H_2O + 2 I_2 + 6 NaCl + Te
Names
hydrogen chloride + sodium iodide + sodium tellurite ⟶ water + iodine + sodium chloride + tellurium
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + NaI + Na_2TeO_3 ⟶ H_2O + I_2 + NaCl + Te 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: 6 HCl + 4 NaI + Na_2TeO_3 ⟶ 3 H_2O + 2 I_2 + 6 NaCl + Te 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 HCl | 6 | -6 NaI | 4 | -4 Na_2TeO_3 | 1 | -1 H_2O | 3 | 3 I_2 | 2 | 2 NaCl | 6 | 6 Te | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) NaI | 4 | -4 | ([NaI])^(-4) Na_2TeO_3 | 1 | -1 | ([Na2TeO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 I_2 | 2 | 2 | ([I2])^2 NaCl | 6 | 6 | ([NaCl])^6 Te | 1 | 1 | [Te] 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 = ([HCl])^(-6) ([NaI])^(-4) ([Na2TeO3])^(-1) ([H2O])^3 ([I2])^2 ([NaCl])^6 [Te] = (([H2O])^3 ([I2])^2 ([NaCl])^6 [Te])/(([HCl])^6 ([NaI])^4 [Na2TeO3])](../image_source/493a603238c11e0a887998e32c2b3c52.png)
Construct the equilibrium constant, K, expression for: HCl + NaI + Na_2TeO_3 ⟶ H_2O + I_2 + NaCl + Te 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: 6 HCl + 4 NaI + Na_2TeO_3 ⟶ 3 H_2O + 2 I_2 + 6 NaCl + Te 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 HCl | 6 | -6 NaI | 4 | -4 Na_2TeO_3 | 1 | -1 H_2O | 3 | 3 I_2 | 2 | 2 NaCl | 6 | 6 Te | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) NaI | 4 | -4 | ([NaI])^(-4) Na_2TeO_3 | 1 | -1 | ([Na2TeO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 I_2 | 2 | 2 | ([I2])^2 NaCl | 6 | 6 | ([NaCl])^6 Te | 1 | 1 | [Te] 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 = ([HCl])^(-6) ([NaI])^(-4) ([Na2TeO3])^(-1) ([H2O])^3 ([I2])^2 ([NaCl])^6 [Te] = (([H2O])^3 ([I2])^2 ([NaCl])^6 [Te])/(([HCl])^6 ([NaI])^4 [Na2TeO3])
Rate of reaction
![Construct the rate of reaction expression for: HCl + NaI + Na_2TeO_3 ⟶ H_2O + I_2 + NaCl + Te 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: 6 HCl + 4 NaI + Na_2TeO_3 ⟶ 3 H_2O + 2 I_2 + 6 NaCl + Te 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 HCl | 6 | -6 NaI | 4 | -4 Na_2TeO_3 | 1 | -1 H_2O | 3 | 3 I_2 | 2 | 2 NaCl | 6 | 6 Te | 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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) NaI | 4 | -4 | -1/4 (Δ[NaI])/(Δt) Na_2TeO_3 | 1 | -1 | -(Δ[Na2TeO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) I_2 | 2 | 2 | 1/2 (Δ[I2])/(Δt) NaCl | 6 | 6 | 1/6 (Δ[NaCl])/(Δt) Te | 1 | 1 | (Δ[Te])/(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 = -1/6 (Δ[HCl])/(Δt) = -1/4 (Δ[NaI])/(Δt) = -(Δ[Na2TeO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/2 (Δ[I2])/(Δt) = 1/6 (Δ[NaCl])/(Δt) = (Δ[Te])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/25e2038221dd9aaeb2b60372db168914.png)
Construct the rate of reaction expression for: HCl + NaI + Na_2TeO_3 ⟶ H_2O + I_2 + NaCl + Te 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: 6 HCl + 4 NaI + Na_2TeO_3 ⟶ 3 H_2O + 2 I_2 + 6 NaCl + Te 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 HCl | 6 | -6 NaI | 4 | -4 Na_2TeO_3 | 1 | -1 H_2O | 3 | 3 I_2 | 2 | 2 NaCl | 6 | 6 Te | 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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) NaI | 4 | -4 | -1/4 (Δ[NaI])/(Δt) Na_2TeO_3 | 1 | -1 | -(Δ[Na2TeO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) I_2 | 2 | 2 | 1/2 (Δ[I2])/(Δt) NaCl | 6 | 6 | 1/6 (Δ[NaCl])/(Δt) Te | 1 | 1 | (Δ[Te])/(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 = -1/6 (Δ[HCl])/(Δt) = -1/4 (Δ[NaI])/(Δt) = -(Δ[Na2TeO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/2 (Δ[I2])/(Δt) = 1/6 (Δ[NaCl])/(Δt) = (Δ[Te])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| hydrogen chloride | sodium iodide | sodium tellurite | water | iodine | sodium chloride | tellurium formula | HCl | NaI | Na_2TeO_3 | H_2O | I_2 | NaCl | Te Hill formula | ClH | INa | Na_2O_3Te_1 | H_2O | I_2 | ClNa | Te name | hydrogen chloride | sodium iodide | sodium tellurite | water | iodine | sodium chloride | tellurium IUPAC name | hydrogen chloride | sodium iodide | | water | molecular iodine | sodium chloride | tellurium