Input interpretation
![H_2O water + SO_2 sulfur dioxide + NaIO_3 sodium iodate ⟶ H_2SO_4 sulfuric acid + I_2 iodine + Na_2SO_4 sodium sulfate](../image_source/91055929ab26f7eac596d7f9c70b9ac6.png)
H_2O water + SO_2 sulfur dioxide + NaIO_3 sodium iodate ⟶ H_2SO_4 sulfuric acid + I_2 iodine + Na_2SO_4 sodium sulfate
Balanced equation
![Balance the chemical equation algebraically: H_2O + SO_2 + NaIO_3 ⟶ H_2SO_4 + I_2 + Na_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 NaIO_3 ⟶ c_4 H_2SO_4 + c_5 I_2 + c_6 Na_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I and Na: H: | 2 c_1 = 2 c_4 O: | c_1 + 2 c_2 + 3 c_3 = 4 c_4 + 4 c_6 S: | c_2 = c_4 + c_6 I: | c_3 = 2 c_5 Na: | c_3 = 2 c_6 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 5 c_3 = 2 c_4 = 4 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 5 SO_2 + 2 NaIO_3 ⟶ 4 H_2SO_4 + I_2 + Na_2SO_4](../image_source/7c4e45e2ff2f91239e8c8bd7bbdd4d1f.png)
Balance the chemical equation algebraically: H_2O + SO_2 + NaIO_3 ⟶ H_2SO_4 + I_2 + Na_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 NaIO_3 ⟶ c_4 H_2SO_4 + c_5 I_2 + c_6 Na_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I and Na: H: | 2 c_1 = 2 c_4 O: | c_1 + 2 c_2 + 3 c_3 = 4 c_4 + 4 c_6 S: | c_2 = c_4 + c_6 I: | c_3 = 2 c_5 Na: | c_3 = 2 c_6 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 5 c_3 = 2 c_4 = 4 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 5 SO_2 + 2 NaIO_3 ⟶ 4 H_2SO_4 + I_2 + Na_2SO_4
Structures
![+ + ⟶ + +](../image_source/0a708cc13ae17b087cb233856baad4c5.png)
+ + ⟶ + +
Names
![water + sulfur dioxide + sodium iodate ⟶ sulfuric acid + iodine + sodium sulfate](../image_source/7ed6cba463cd1146440611a6fa6ae3ca.png)
water + sulfur dioxide + sodium iodate ⟶ sulfuric acid + iodine + sodium sulfate
Reaction thermodynamics
Enthalpy
![| water | sulfur dioxide | sodium iodate | sulfuric acid | iodine | sodium sulfate molecular enthalpy | -285.8 kJ/mol | -296.8 kJ/mol | -481.8 kJ/mol | -814 kJ/mol | 0 kJ/mol | -1387 kJ/mol total enthalpy | -1143 kJ/mol | -1484 kJ/mol | -963.6 kJ/mol | -3256 kJ/mol | 0 kJ/mol | -1387 kJ/mol | H_initial = -3591 kJ/mol | | | H_final = -4643 kJ/mol | | ΔH_rxn^0 | -4643 kJ/mol - -3591 kJ/mol = -1052 kJ/mol (exothermic) | | | | |](../image_source/c39860b6008edd3e711b464645ed5a9d.png)
| water | sulfur dioxide | sodium iodate | sulfuric acid | iodine | sodium sulfate molecular enthalpy | -285.8 kJ/mol | -296.8 kJ/mol | -481.8 kJ/mol | -814 kJ/mol | 0 kJ/mol | -1387 kJ/mol total enthalpy | -1143 kJ/mol | -1484 kJ/mol | -963.6 kJ/mol | -3256 kJ/mol | 0 kJ/mol | -1387 kJ/mol | H_initial = -3591 kJ/mol | | | H_final = -4643 kJ/mol | | ΔH_rxn^0 | -4643 kJ/mol - -3591 kJ/mol = -1052 kJ/mol (exothermic) | | | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2O + SO_2 + NaIO_3 ⟶ H_2SO_4 + I_2 + Na_2SO_4 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: 4 H_2O + 5 SO_2 + 2 NaIO_3 ⟶ 4 H_2SO_4 + I_2 + Na_2SO_4 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 H_2O | 4 | -4 SO_2 | 5 | -5 NaIO_3 | 2 | -2 H_2SO_4 | 4 | 4 I_2 | 1 | 1 Na_2SO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) SO_2 | 5 | -5 | ([SO2])^(-5) NaIO_3 | 2 | -2 | ([NaIO3])^(-2) H_2SO_4 | 4 | 4 | ([H2SO4])^4 I_2 | 1 | 1 | [I2] Na_2SO_4 | 1 | 1 | [Na2SO4] 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 = ([H2O])^(-4) ([SO2])^(-5) ([NaIO3])^(-2) ([H2SO4])^4 [I2] [Na2SO4] = (([H2SO4])^4 [I2] [Na2SO4])/(([H2O])^4 ([SO2])^5 ([NaIO3])^2)](../image_source/534ca32a7dd108270b50297dce1ffba6.png)
Construct the equilibrium constant, K, expression for: H_2O + SO_2 + NaIO_3 ⟶ H_2SO_4 + I_2 + Na_2SO_4 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: 4 H_2O + 5 SO_2 + 2 NaIO_3 ⟶ 4 H_2SO_4 + I_2 + Na_2SO_4 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 H_2O | 4 | -4 SO_2 | 5 | -5 NaIO_3 | 2 | -2 H_2SO_4 | 4 | 4 I_2 | 1 | 1 Na_2SO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) SO_2 | 5 | -5 | ([SO2])^(-5) NaIO_3 | 2 | -2 | ([NaIO3])^(-2) H_2SO_4 | 4 | 4 | ([H2SO4])^4 I_2 | 1 | 1 | [I2] Na_2SO_4 | 1 | 1 | [Na2SO4] 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 = ([H2O])^(-4) ([SO2])^(-5) ([NaIO3])^(-2) ([H2SO4])^4 [I2] [Na2SO4] = (([H2SO4])^4 [I2] [Na2SO4])/(([H2O])^4 ([SO2])^5 ([NaIO3])^2)
Rate of reaction
![Construct the rate of reaction expression for: H_2O + SO_2 + NaIO_3 ⟶ H_2SO_4 + I_2 + Na_2SO_4 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: 4 H_2O + 5 SO_2 + 2 NaIO_3 ⟶ 4 H_2SO_4 + I_2 + Na_2SO_4 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 H_2O | 4 | -4 SO_2 | 5 | -5 NaIO_3 | 2 | -2 H_2SO_4 | 4 | 4 I_2 | 1 | 1 Na_2SO_4 | 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 H_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) SO_2 | 5 | -5 | -1/5 (Δ[SO2])/(Δt) NaIO_3 | 2 | -2 | -1/2 (Δ[NaIO3])/(Δt) H_2SO_4 | 4 | 4 | 1/4 (Δ[H2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/5 (Δ[SO2])/(Δt) = -1/2 (Δ[NaIO3])/(Δt) = 1/4 (Δ[H2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[Na2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/6e1258c6e0af9808a5b357bdcca19ab3.png)
Construct the rate of reaction expression for: H_2O + SO_2 + NaIO_3 ⟶ H_2SO_4 + I_2 + Na_2SO_4 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: 4 H_2O + 5 SO_2 + 2 NaIO_3 ⟶ 4 H_2SO_4 + I_2 + Na_2SO_4 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 H_2O | 4 | -4 SO_2 | 5 | -5 NaIO_3 | 2 | -2 H_2SO_4 | 4 | 4 I_2 | 1 | 1 Na_2SO_4 | 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 H_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) SO_2 | 5 | -5 | -1/5 (Δ[SO2])/(Δt) NaIO_3 | 2 | -2 | -1/2 (Δ[NaIO3])/(Δt) H_2SO_4 | 4 | 4 | 1/4 (Δ[H2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/5 (Δ[SO2])/(Δt) = -1/2 (Δ[NaIO3])/(Δt) = 1/4 (Δ[H2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[Na2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| water | sulfur dioxide | sodium iodate | sulfuric acid | iodine | sodium sulfate formula | H_2O | SO_2 | NaIO_3 | H_2SO_4 | I_2 | Na_2SO_4 Hill formula | H_2O | O_2S | INaO_3 | H_2O_4S | I_2 | Na_2O_4S name | water | sulfur dioxide | sodium iodate | sulfuric acid | iodine | sodium sulfate IUPAC name | water | sulfur dioxide | sodium iodate | sulfuric acid | molecular iodine | disodium sulfate](../image_source/9fdf7f018ee34c85d0c9b24dc2a4dfa1.png)
| water | sulfur dioxide | sodium iodate | sulfuric acid | iodine | sodium sulfate formula | H_2O | SO_2 | NaIO_3 | H_2SO_4 | I_2 | Na_2SO_4 Hill formula | H_2O | O_2S | INaO_3 | H_2O_4S | I_2 | Na_2O_4S name | water | sulfur dioxide | sodium iodate | sulfuric acid | iodine | sodium sulfate IUPAC name | water | sulfur dioxide | sodium iodate | sulfuric acid | molecular iodine | disodium sulfate