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H2O + Cl2 + Ag5IO6 = O2 + AgCl + H5IO6

Input interpretation

H_2O water + Cl_2 chlorine + Ag5IO6 ⟶ O_2 oxygen + AgCl silver chloride + H_5IO_6 periodic acid
H_2O water + Cl_2 chlorine + Ag5IO6 ⟶ O_2 oxygen + AgCl silver chloride + H_5IO_6 periodic acid

Balanced equation

Balance the chemical equation algebraically: H_2O + Cl_2 + Ag5IO6 ⟶ O_2 + AgCl + H_5IO_6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Ag5IO6 ⟶ c_4 O_2 + c_5 AgCl + c_6 H_5IO_6 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Ag and I: H: | 2 c_1 = 5 c_6 O: | c_1 + 6 c_3 = 2 c_4 + 6 c_6 Cl: | 2 c_2 = c_5 Ag: | 5 c_3 = c_5 I: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5/2 c_2 = 5/2 c_3 = 1 c_4 = 5/4 c_5 = 5 c_6 = 1 Multiply by the least common denominator, 4, to eliminate fractional coefficients: c_1 = 10 c_2 = 10 c_3 = 4 c_4 = 5 c_5 = 20 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 H_2O + 10 Cl_2 + 4 Ag5IO6 ⟶ 5 O_2 + 20 AgCl + 4 H_5IO_6
Balance the chemical equation algebraically: H_2O + Cl_2 + Ag5IO6 ⟶ O_2 + AgCl + H_5IO_6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Ag5IO6 ⟶ c_4 O_2 + c_5 AgCl + c_6 H_5IO_6 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Ag and I: H: | 2 c_1 = 5 c_6 O: | c_1 + 6 c_3 = 2 c_4 + 6 c_6 Cl: | 2 c_2 = c_5 Ag: | 5 c_3 = c_5 I: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5/2 c_2 = 5/2 c_3 = 1 c_4 = 5/4 c_5 = 5 c_6 = 1 Multiply by the least common denominator, 4, to eliminate fractional coefficients: c_1 = 10 c_2 = 10 c_3 = 4 c_4 = 5 c_5 = 20 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 H_2O + 10 Cl_2 + 4 Ag5IO6 ⟶ 5 O_2 + 20 AgCl + 4 H_5IO_6

Structures

+ + Ag5IO6 ⟶ + +
+ + Ag5IO6 ⟶ + +

Names

water + chlorine + Ag5IO6 ⟶ oxygen + silver chloride + periodic acid
water + chlorine + Ag5IO6 ⟶ oxygen + silver chloride + periodic acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Ag5IO6 ⟶ O_2 + AgCl + H_5IO_6 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: 10 H_2O + 10 Cl_2 + 4 Ag5IO6 ⟶ 5 O_2 + 20 AgCl + 4 H_5IO_6 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 | 10 | -10 Cl_2 | 10 | -10 Ag5IO6 | 4 | -4 O_2 | 5 | 5 AgCl | 20 | 20 H_5IO_6 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 10 | -10 | ([H2O])^(-10) Cl_2 | 10 | -10 | ([Cl2])^(-10) Ag5IO6 | 4 | -4 | ([Ag5IO6])^(-4) O_2 | 5 | 5 | ([O2])^5 AgCl | 20 | 20 | ([AgCl])^20 H_5IO_6 | 4 | 4 | ([H5IO6])^4 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])^(-10) ([Cl2])^(-10) ([Ag5IO6])^(-4) ([O2])^5 ([AgCl])^20 ([H5IO6])^4 = (([O2])^5 ([AgCl])^20 ([H5IO6])^4)/(([H2O])^10 ([Cl2])^10 ([Ag5IO6])^4)
Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Ag5IO6 ⟶ O_2 + AgCl + H_5IO_6 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: 10 H_2O + 10 Cl_2 + 4 Ag5IO6 ⟶ 5 O_2 + 20 AgCl + 4 H_5IO_6 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 | 10 | -10 Cl_2 | 10 | -10 Ag5IO6 | 4 | -4 O_2 | 5 | 5 AgCl | 20 | 20 H_5IO_6 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 10 | -10 | ([H2O])^(-10) Cl_2 | 10 | -10 | ([Cl2])^(-10) Ag5IO6 | 4 | -4 | ([Ag5IO6])^(-4) O_2 | 5 | 5 | ([O2])^5 AgCl | 20 | 20 | ([AgCl])^20 H_5IO_6 | 4 | 4 | ([H5IO6])^4 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])^(-10) ([Cl2])^(-10) ([Ag5IO6])^(-4) ([O2])^5 ([AgCl])^20 ([H5IO6])^4 = (([O2])^5 ([AgCl])^20 ([H5IO6])^4)/(([H2O])^10 ([Cl2])^10 ([Ag5IO6])^4)

Rate of reaction

Construct the rate of reaction expression for: H_2O + Cl_2 + Ag5IO6 ⟶ O_2 + AgCl + H_5IO_6 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: 10 H_2O + 10 Cl_2 + 4 Ag5IO6 ⟶ 5 O_2 + 20 AgCl + 4 H_5IO_6 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 | 10 | -10 Cl_2 | 10 | -10 Ag5IO6 | 4 | -4 O_2 | 5 | 5 AgCl | 20 | 20 H_5IO_6 | 4 | 4 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 | 10 | -10 | -1/10 (Δ[H2O])/(Δt) Cl_2 | 10 | -10 | -1/10 (Δ[Cl2])/(Δt) Ag5IO6 | 4 | -4 | -1/4 (Δ[Ag5IO6])/(Δt) O_2 | 5 | 5 | 1/5 (Δ[O2])/(Δt) AgCl | 20 | 20 | 1/20 (Δ[AgCl])/(Δt) H_5IO_6 | 4 | 4 | 1/4 (Δ[H5IO6])/(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 = -1/10 (Δ[H2O])/(Δt) = -1/10 (Δ[Cl2])/(Δt) = -1/4 (Δ[Ag5IO6])/(Δt) = 1/5 (Δ[O2])/(Δt) = 1/20 (Δ[AgCl])/(Δt) = 1/4 (Δ[H5IO6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Cl_2 + Ag5IO6 ⟶ O_2 + AgCl + H_5IO_6 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: 10 H_2O + 10 Cl_2 + 4 Ag5IO6 ⟶ 5 O_2 + 20 AgCl + 4 H_5IO_6 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 | 10 | -10 Cl_2 | 10 | -10 Ag5IO6 | 4 | -4 O_2 | 5 | 5 AgCl | 20 | 20 H_5IO_6 | 4 | 4 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 | 10 | -10 | -1/10 (Δ[H2O])/(Δt) Cl_2 | 10 | -10 | -1/10 (Δ[Cl2])/(Δt) Ag5IO6 | 4 | -4 | -1/4 (Δ[Ag5IO6])/(Δt) O_2 | 5 | 5 | 1/5 (Δ[O2])/(Δt) AgCl | 20 | 20 | 1/20 (Δ[AgCl])/(Δt) H_5IO_6 | 4 | 4 | 1/4 (Δ[H5IO6])/(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 = -1/10 (Δ[H2O])/(Δt) = -1/10 (Δ[Cl2])/(Δt) = -1/4 (Δ[Ag5IO6])/(Δt) = 1/5 (Δ[O2])/(Δt) = 1/20 (Δ[AgCl])/(Δt) = 1/4 (Δ[H5IO6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | chlorine | Ag5IO6 | oxygen | silver chloride | periodic acid formula | H_2O | Cl_2 | Ag5IO6 | O_2 | AgCl | H_5IO_6 name | water | chlorine | | oxygen | silver chloride | periodic acid IUPAC name | water | molecular chlorine | | molecular oxygen | chlorosilver |
| water | chlorine | Ag5IO6 | oxygen | silver chloride | periodic acid formula | H_2O | Cl_2 | Ag5IO6 | O_2 | AgCl | H_5IO_6 name | water | chlorine | | oxygen | silver chloride | periodic acid IUPAC name | water | molecular chlorine | | molecular oxygen | chlorosilver |

Substance properties

| water | chlorine | Ag5IO6 | oxygen | silver chloride | periodic acid molar mass | 18.015 g/mol | 70.9 g/mol | 762.24 g/mol | 31.998 g/mol | 143.32 g/mol | 227.94 g/mol phase | liquid (at STP) | gas (at STP) | | gas (at STP) | solid (at STP) | solid (at STP) melting point | 0 °C | -101 °C | | -218 °C | 455 °C | 122 °C boiling point | 99.9839 °C | -34 °C | | -183 °C | 1554 °C | density | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | | 0.001429 g/cm^3 (at 0 °C) | 5.56 g/cm^3 | 1.3875 g/cm^3 solubility in water | | | | | | soluble surface tension | 0.0728 N/m | | | 0.01347 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | | | odorless | | odorless
| water | chlorine | Ag5IO6 | oxygen | silver chloride | periodic acid molar mass | 18.015 g/mol | 70.9 g/mol | 762.24 g/mol | 31.998 g/mol | 143.32 g/mol | 227.94 g/mol phase | liquid (at STP) | gas (at STP) | | gas (at STP) | solid (at STP) | solid (at STP) melting point | 0 °C | -101 °C | | -218 °C | 455 °C | 122 °C boiling point | 99.9839 °C | -34 °C | | -183 °C | 1554 °C | density | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | | 0.001429 g/cm^3 (at 0 °C) | 5.56 g/cm^3 | 1.3875 g/cm^3 solubility in water | | | | | | soluble surface tension | 0.0728 N/m | | | 0.01347 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | | | odorless | | odorless

Units

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