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KI + Hg2(NO3)2 = I2 + KNO3 + Hg

Input interpretation

KI potassium iodide + Hg_2(NO_3)_2 mercury(I) nitrate ⟶ I_2 iodine + KNO_3 potassium nitrate + Hg mercury
KI potassium iodide + Hg_2(NO_3)_2 mercury(I) nitrate ⟶ I_2 iodine + KNO_3 potassium nitrate + Hg mercury

Balanced equation

Balance the chemical equation algebraically: KI + Hg_2(NO_3)_2 ⟶ I_2 + KNO_3 + Hg Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 Hg_2(NO_3)_2 ⟶ c_3 I_2 + c_4 KNO_3 + c_5 Hg Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Hg, N and O: I: | c_1 = 2 c_3 K: | c_1 = c_4 Hg: | c_2 = c_5 N: | c_2 = c_4 O: | 3 c_2 = 3 c_4 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 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KI + 2 Hg_2(NO_3)_2 ⟶ I_2 + 2 KNO_3 + 2 Hg
Balance the chemical equation algebraically: KI + Hg_2(NO_3)_2 ⟶ I_2 + KNO_3 + Hg Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 Hg_2(NO_3)_2 ⟶ c_3 I_2 + c_4 KNO_3 + c_5 Hg Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Hg, N and O: I: | c_1 = 2 c_3 K: | c_1 = c_4 Hg: | c_2 = c_5 N: | c_2 = c_4 O: | 3 c_2 = 3 c_4 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 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KI + 2 Hg_2(NO_3)_2 ⟶ I_2 + 2 KNO_3 + 2 Hg

Structures

+ ⟶ + +
+ ⟶ + +

Names

potassium iodide + mercury(I) nitrate ⟶ iodine + potassium nitrate + mercury
potassium iodide + mercury(I) nitrate ⟶ iodine + potassium nitrate + mercury

Equilibrium constant

Construct the equilibrium constant, K, expression for: KI + Hg_2(NO_3)_2 ⟶ I_2 + KNO_3 + Hg 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: 2 KI + 2 Hg_2(NO_3)_2 ⟶ I_2 + 2 KNO_3 + 2 Hg 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 | 2 | -2 Hg_2(NO_3)_2 | 2 | -2 I_2 | 1 | 1 KNO_3 | 2 | 2 Hg | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KI | 2 | -2 | ([KI])^(-2) Hg_2(NO_3)_2 | 2 | -2 | ([Hg2(NO3)2])^(-2) I_2 | 1 | 1 | [I2] KNO_3 | 2 | 2 | ([KNO3])^2 Hg | 2 | 2 | ([Hg])^2 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])^(-2) ([Hg2(NO3)2])^(-2) [I2] ([KNO3])^2 ([Hg])^2 = ([I2] ([KNO3])^2 ([Hg])^2)/(([KI])^2 ([Hg2(NO3)2])^2)
Construct the equilibrium constant, K, expression for: KI + Hg_2(NO_3)_2 ⟶ I_2 + KNO_3 + Hg 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: 2 KI + 2 Hg_2(NO_3)_2 ⟶ I_2 + 2 KNO_3 + 2 Hg 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 | 2 | -2 Hg_2(NO_3)_2 | 2 | -2 I_2 | 1 | 1 KNO_3 | 2 | 2 Hg | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KI | 2 | -2 | ([KI])^(-2) Hg_2(NO_3)_2 | 2 | -2 | ([Hg2(NO3)2])^(-2) I_2 | 1 | 1 | [I2] KNO_3 | 2 | 2 | ([KNO3])^2 Hg | 2 | 2 | ([Hg])^2 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])^(-2) ([Hg2(NO3)2])^(-2) [I2] ([KNO3])^2 ([Hg])^2 = ([I2] ([KNO3])^2 ([Hg])^2)/(([KI])^2 ([Hg2(NO3)2])^2)

Rate of reaction

Construct the rate of reaction expression for: KI + Hg_2(NO_3)_2 ⟶ I_2 + KNO_3 + Hg 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: 2 KI + 2 Hg_2(NO_3)_2 ⟶ I_2 + 2 KNO_3 + 2 Hg 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 | 2 | -2 Hg_2(NO_3)_2 | 2 | -2 I_2 | 1 | 1 KNO_3 | 2 | 2 Hg | 2 | 2 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 | 2 | -2 | -1/2 (Δ[KI])/(Δt) Hg_2(NO_3)_2 | 2 | -2 | -1/2 (Δ[Hg2(NO3)2])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) Hg | 2 | 2 | 1/2 (Δ[Hg])/(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 = -1/2 (Δ[KI])/(Δt) = -1/2 (Δ[Hg2(NO3)2])/(Δt) = (Δ[I2])/(Δt) = 1/2 (Δ[KNO3])/(Δt) = 1/2 (Δ[Hg])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KI + Hg_2(NO_3)_2 ⟶ I_2 + KNO_3 + Hg 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: 2 KI + 2 Hg_2(NO_3)_2 ⟶ I_2 + 2 KNO_3 + 2 Hg 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 | 2 | -2 Hg_2(NO_3)_2 | 2 | -2 I_2 | 1 | 1 KNO_3 | 2 | 2 Hg | 2 | 2 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 | 2 | -2 | -1/2 (Δ[KI])/(Δt) Hg_2(NO_3)_2 | 2 | -2 | -1/2 (Δ[Hg2(NO3)2])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) Hg | 2 | 2 | 1/2 (Δ[Hg])/(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 = -1/2 (Δ[KI])/(Δt) = -1/2 (Δ[Hg2(NO3)2])/(Δt) = (Δ[I2])/(Δt) = 1/2 (Δ[KNO3])/(Δt) = 1/2 (Δ[Hg])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium iodide | mercury(I) nitrate | iodine | potassium nitrate | mercury formula | KI | Hg_2(NO_3)_2 | I_2 | KNO_3 | Hg Hill formula | IK | Hg_2N_2O_6 | I_2 | KNO_3 | Hg name | potassium iodide | mercury(I) nitrate | iodine | potassium nitrate | mercury IUPAC name | potassium iodide | | molecular iodine | potassium nitrate | mercury
| potassium iodide | mercury(I) nitrate | iodine | potassium nitrate | mercury formula | KI | Hg_2(NO_3)_2 | I_2 | KNO_3 | Hg Hill formula | IK | Hg_2N_2O_6 | I_2 | KNO_3 | Hg name | potassium iodide | mercury(I) nitrate | iodine | potassium nitrate | mercury IUPAC name | potassium iodide | | molecular iodine | potassium nitrate | mercury

Substance properties

| potassium iodide | mercury(I) nitrate | iodine | potassium nitrate | mercury molar mass | 166.0028 g/mol | 262.596 g/mol | 253.80894 g/mol | 101.1 g/mol | 200.592 g/mol phase | solid (at STP) | | solid (at STP) | solid (at STP) | liquid (at STP) melting point | 681 °C | | 113 °C | 334 °C | -38.87 °C boiling point | 1330 °C | | 184 °C | | 356.6 °C density | 3.123 g/cm^3 | | 4.94 g/cm^3 | | 13.534 g/cm^3 solubility in water | | slightly soluble | | soluble | slightly soluble surface tension | | | | | 0.47 N/m dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | 0.00227 Pa s (at 116 °C) | | 0.001526 Pa s (at 25 °C) odor | | | | odorless | odorless
| potassium iodide | mercury(I) nitrate | iodine | potassium nitrate | mercury molar mass | 166.0028 g/mol | 262.596 g/mol | 253.80894 g/mol | 101.1 g/mol | 200.592 g/mol phase | solid (at STP) | | solid (at STP) | solid (at STP) | liquid (at STP) melting point | 681 °C | | 113 °C | 334 °C | -38.87 °C boiling point | 1330 °C | | 184 °C | | 356.6 °C density | 3.123 g/cm^3 | | 4.94 g/cm^3 | | 13.534 g/cm^3 solubility in water | | slightly soluble | | soluble | slightly soluble surface tension | | | | | 0.47 N/m dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | 0.00227 Pa s (at 116 °C) | | 0.001526 Pa s (at 25 °C) odor | | | | odorless | odorless

Units

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