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KI + Y2SO4 = K2SO4 + I2 + Y2O + Y2S

Input interpretation

KI potassium iodide + Y2SO4 ⟶ K_2SO_4 potassium sulfate + I_2 iodine + Y2O + Y2S
KI potassium iodide + Y2SO4 ⟶ K_2SO_4 potassium sulfate + I_2 iodine + Y2O + Y2S

Balanced equation

Balance the chemical equation algebraically: KI + Y2SO4 ⟶ K_2SO_4 + I_2 + Y2O + Y2S Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 Y2SO4 ⟶ c_3 K_2SO_4 + c_4 I_2 + c_5 Y2O + c_6 Y2S Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Y, S and O: I: | c_1 = 2 c_4 K: | c_1 = 2 c_3 Y: | 2 c_2 = 2 c_5 + 2 c_6 S: | c_2 = c_3 + c_6 O: | 4 c_2 = 4 c_3 + c_5 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 5 c_3 = 4 c_4 = 4 c_5 = 4 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 KI + 5 Y2SO4 ⟶ 4 K_2SO_4 + 4 I_2 + 4 Y2O + Y2S
Balance the chemical equation algebraically: KI + Y2SO4 ⟶ K_2SO_4 + I_2 + Y2O + Y2S Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 Y2SO4 ⟶ c_3 K_2SO_4 + c_4 I_2 + c_5 Y2O + c_6 Y2S Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Y, S and O: I: | c_1 = 2 c_4 K: | c_1 = 2 c_3 Y: | 2 c_2 = 2 c_5 + 2 c_6 S: | c_2 = c_3 + c_6 O: | 4 c_2 = 4 c_3 + c_5 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 5 c_3 = 4 c_4 = 4 c_5 = 4 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 KI + 5 Y2SO4 ⟶ 4 K_2SO_4 + 4 I_2 + 4 Y2O + Y2S

Structures

+ Y2SO4 ⟶ + + Y2O + Y2S
+ Y2SO4 ⟶ + + Y2O + Y2S

Names

potassium iodide + Y2SO4 ⟶ potassium sulfate + iodine + Y2O + Y2S
potassium iodide + Y2SO4 ⟶ potassium sulfate + iodine + Y2O + Y2S

Equilibrium constant

Construct the equilibrium constant, K, expression for: KI + Y2SO4 ⟶ K_2SO_4 + I_2 + Y2O + Y2S 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: 8 KI + 5 Y2SO4 ⟶ 4 K_2SO_4 + 4 I_2 + 4 Y2O + Y2S 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 KI | 8 | -8 Y2SO4 | 5 | -5 K_2SO_4 | 4 | 4 I_2 | 4 | 4 Y2O | 4 | 4 Y2S | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KI | 8 | -8 | ([KI])^(-8) Y2SO4 | 5 | -5 | ([Y2SO4])^(-5) K_2SO_4 | 4 | 4 | ([K2SO4])^4 I_2 | 4 | 4 | ([I2])^4 Y2O | 4 | 4 | ([Y2O])^4 Y2S | 1 | 1 | [Y2S] 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 = ([KI])^(-8) ([Y2SO4])^(-5) ([K2SO4])^4 ([I2])^4 ([Y2O])^4 [Y2S] = (([K2SO4])^4 ([I2])^4 ([Y2O])^4 [Y2S])/(([KI])^8 ([Y2SO4])^5)
Construct the equilibrium constant, K, expression for: KI + Y2SO4 ⟶ K_2SO_4 + I_2 + Y2O + Y2S 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: 8 KI + 5 Y2SO4 ⟶ 4 K_2SO_4 + 4 I_2 + 4 Y2O + Y2S 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 KI | 8 | -8 Y2SO4 | 5 | -5 K_2SO_4 | 4 | 4 I_2 | 4 | 4 Y2O | 4 | 4 Y2S | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KI | 8 | -8 | ([KI])^(-8) Y2SO4 | 5 | -5 | ([Y2SO4])^(-5) K_2SO_4 | 4 | 4 | ([K2SO4])^4 I_2 | 4 | 4 | ([I2])^4 Y2O | 4 | 4 | ([Y2O])^4 Y2S | 1 | 1 | [Y2S] 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 = ([KI])^(-8) ([Y2SO4])^(-5) ([K2SO4])^4 ([I2])^4 ([Y2O])^4 [Y2S] = (([K2SO4])^4 ([I2])^4 ([Y2O])^4 [Y2S])/(([KI])^8 ([Y2SO4])^5)

Rate of reaction

Construct the rate of reaction expression for: KI + Y2SO4 ⟶ K_2SO_4 + I_2 + Y2O + Y2S 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: 8 KI + 5 Y2SO4 ⟶ 4 K_2SO_4 + 4 I_2 + 4 Y2O + Y2S 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 KI | 8 | -8 Y2SO4 | 5 | -5 K_2SO_4 | 4 | 4 I_2 | 4 | 4 Y2O | 4 | 4 Y2S | 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 KI | 8 | -8 | -1/8 (Δ[KI])/(Δt) Y2SO4 | 5 | -5 | -1/5 (Δ[Y2SO4])/(Δt) K_2SO_4 | 4 | 4 | 1/4 (Δ[K2SO4])/(Δt) I_2 | 4 | 4 | 1/4 (Δ[I2])/(Δt) Y2O | 4 | 4 | 1/4 (Δ[Y2O])/(Δt) Y2S | 1 | 1 | (Δ[Y2S])/(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 = -1/8 (Δ[KI])/(Δt) = -1/5 (Δ[Y2SO4])/(Δt) = 1/4 (Δ[K2SO4])/(Δt) = 1/4 (Δ[I2])/(Δt) = 1/4 (Δ[Y2O])/(Δt) = (Δ[Y2S])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KI + Y2SO4 ⟶ K_2SO_4 + I_2 + Y2O + Y2S 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: 8 KI + 5 Y2SO4 ⟶ 4 K_2SO_4 + 4 I_2 + 4 Y2O + Y2S 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 KI | 8 | -8 Y2SO4 | 5 | -5 K_2SO_4 | 4 | 4 I_2 | 4 | 4 Y2O | 4 | 4 Y2S | 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 KI | 8 | -8 | -1/8 (Δ[KI])/(Δt) Y2SO4 | 5 | -5 | -1/5 (Δ[Y2SO4])/(Δt) K_2SO_4 | 4 | 4 | 1/4 (Δ[K2SO4])/(Δt) I_2 | 4 | 4 | 1/4 (Δ[I2])/(Δt) Y2O | 4 | 4 | 1/4 (Δ[Y2O])/(Δt) Y2S | 1 | 1 | (Δ[Y2S])/(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 = -1/8 (Δ[KI])/(Δt) = -1/5 (Δ[Y2SO4])/(Δt) = 1/4 (Δ[K2SO4])/(Δt) = 1/4 (Δ[I2])/(Δt) = 1/4 (Δ[Y2O])/(Δt) = (Δ[Y2S])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium iodide | Y2SO4 | potassium sulfate | iodine | Y2O | Y2S formula | KI | Y2SO4 | K_2SO_4 | I_2 | Y2O | Y2S Hill formula | IK | O4SY2 | K_2O_4S | I_2 | OY2 | SY2 name | potassium iodide | | potassium sulfate | iodine | | IUPAC name | potassium iodide | | dipotassium sulfate | molecular iodine | |
| potassium iodide | Y2SO4 | potassium sulfate | iodine | Y2O | Y2S formula | KI | Y2SO4 | K_2SO_4 | I_2 | Y2O | Y2S Hill formula | IK | O4SY2 | K_2O_4S | I_2 | OY2 | SY2 name | potassium iodide | | potassium sulfate | iodine | | IUPAC name | potassium iodide | | dipotassium sulfate | molecular iodine | |

Substance properties

| potassium iodide | Y2SO4 | potassium sulfate | iodine | Y2O | Y2S molar mass | 166.0028 g/mol | 273.87 g/mol | 174.25 g/mol | 253.80894 g/mol | 193.811 g/mol | 209.87 g/mol phase | solid (at STP) | | | solid (at STP) | | melting point | 681 °C | | | 113 °C | | boiling point | 1330 °C | | | 184 °C | | density | 3.123 g/cm^3 | | | 4.94 g/cm^3 | | solubility in water | | | soluble | | | dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | | 0.00227 Pa s (at 116 °C) | |
| potassium iodide | Y2SO4 | potassium sulfate | iodine | Y2O | Y2S molar mass | 166.0028 g/mol | 273.87 g/mol | 174.25 g/mol | 253.80894 g/mol | 193.811 g/mol | 209.87 g/mol phase | solid (at STP) | | | solid (at STP) | | melting point | 681 °C | | | 113 °C | | boiling point | 1330 °C | | | 184 °C | | density | 3.123 g/cm^3 | | | 4.94 g/cm^3 | | solubility in water | | | soluble | | | dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | | 0.00227 Pa s (at 116 °C) | |

Units

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