Search

KI + Mg(NO3)2 = KNO3 + MgI2

Input interpretation

KI potassium iodide + Mg(NO_3)_2 magnesium nitrate ⟶ KNO_3 potassium nitrate + MgI_2 magnesium iodide
KI potassium iodide + Mg(NO_3)_2 magnesium nitrate ⟶ KNO_3 potassium nitrate + MgI_2 magnesium iodide

Balanced equation

Balance the chemical equation algebraically: KI + Mg(NO_3)_2 ⟶ KNO_3 + MgI_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 Mg(NO_3)_2 ⟶ c_3 KNO_3 + c_4 MgI_2 Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Mg, N and O: I: | c_1 = 2 c_4 K: | c_1 = c_3 Mg: | c_2 = c_4 N: | 2 c_2 = c_3 O: | 6 c_2 = 3 c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KI + Mg(NO_3)_2 ⟶ 2 KNO_3 + MgI_2
Balance the chemical equation algebraically: KI + Mg(NO_3)_2 ⟶ KNO_3 + MgI_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KI + c_2 Mg(NO_3)_2 ⟶ c_3 KNO_3 + c_4 MgI_2 Set the number of atoms in the reactants equal to the number of atoms in the products for I, K, Mg, N and O: I: | c_1 = 2 c_4 K: | c_1 = c_3 Mg: | c_2 = c_4 N: | 2 c_2 = c_3 O: | 6 c_2 = 3 c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KI + Mg(NO_3)_2 ⟶ 2 KNO_3 + MgI_2

Structures

+ ⟶ +
+ ⟶ +

Names

potassium iodide + magnesium nitrate ⟶ potassium nitrate + magnesium iodide
potassium iodide + magnesium nitrate ⟶ potassium nitrate + magnesium iodide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KI + Mg(NO_3)_2 ⟶ KNO_3 + MgI_2 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 + Mg(NO_3)_2 ⟶ 2 KNO_3 + MgI_2 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 Mg(NO_3)_2 | 1 | -1 KNO_3 | 2 | 2 MgI_2 | 1 | 1 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) Mg(NO_3)_2 | 1 | -1 | ([Mg(NO3)2])^(-1) KNO_3 | 2 | 2 | ([KNO3])^2 MgI_2 | 1 | 1 | [MgI2] 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) ([Mg(NO3)2])^(-1) ([KNO3])^2 [MgI2] = (([KNO3])^2 [MgI2])/(([KI])^2 [Mg(NO3)2])
Construct the equilibrium constant, K, expression for: KI + Mg(NO_3)_2 ⟶ KNO_3 + MgI_2 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 + Mg(NO_3)_2 ⟶ 2 KNO_3 + MgI_2 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 Mg(NO_3)_2 | 1 | -1 KNO_3 | 2 | 2 MgI_2 | 1 | 1 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) Mg(NO_3)_2 | 1 | -1 | ([Mg(NO3)2])^(-1) KNO_3 | 2 | 2 | ([KNO3])^2 MgI_2 | 1 | 1 | [MgI2] 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) ([Mg(NO3)2])^(-1) ([KNO3])^2 [MgI2] = (([KNO3])^2 [MgI2])/(([KI])^2 [Mg(NO3)2])

Rate of reaction

Construct the rate of reaction expression for: KI + Mg(NO_3)_2 ⟶ KNO_3 + MgI_2 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 + Mg(NO_3)_2 ⟶ 2 KNO_3 + MgI_2 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 Mg(NO_3)_2 | 1 | -1 KNO_3 | 2 | 2 MgI_2 | 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 | 2 | -2 | -1/2 (Δ[KI])/(Δt) Mg(NO_3)_2 | 1 | -1 | -(Δ[Mg(NO3)2])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) MgI_2 | 1 | 1 | (Δ[MgI2])/(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) = -(Δ[Mg(NO3)2])/(Δt) = 1/2 (Δ[KNO3])/(Δt) = (Δ[MgI2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KI + Mg(NO_3)_2 ⟶ KNO_3 + MgI_2 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 + Mg(NO_3)_2 ⟶ 2 KNO_3 + MgI_2 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 Mg(NO_3)_2 | 1 | -1 KNO_3 | 2 | 2 MgI_2 | 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 | 2 | -2 | -1/2 (Δ[KI])/(Δt) Mg(NO_3)_2 | 1 | -1 | -(Δ[Mg(NO3)2])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) MgI_2 | 1 | 1 | (Δ[MgI2])/(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) = -(Δ[Mg(NO3)2])/(Δt) = 1/2 (Δ[KNO3])/(Δt) = (Δ[MgI2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium iodide | magnesium nitrate | potassium nitrate | magnesium iodide formula | KI | Mg(NO_3)_2 | KNO_3 | MgI_2 Hill formula | IK | MgN_2O_6 | KNO_3 | I_2Mg name | potassium iodide | magnesium nitrate | potassium nitrate | magnesium iodide IUPAC name | potassium iodide | magnesium dinitrate | potassium nitrate | magnesium diiodide
| potassium iodide | magnesium nitrate | potassium nitrate | magnesium iodide formula | KI | Mg(NO_3)_2 | KNO_3 | MgI_2 Hill formula | IK | MgN_2O_6 | KNO_3 | I_2Mg name | potassium iodide | magnesium nitrate | potassium nitrate | magnesium iodide IUPAC name | potassium iodide | magnesium dinitrate | potassium nitrate | magnesium diiodide

Substance properties

| potassium iodide | magnesium nitrate | potassium nitrate | magnesium iodide molar mass | 166.0028 g/mol | 148.31 g/mol | 101.1 g/mol | 278.114 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 681 °C | 88.9 °C | 334 °C | 637 °C boiling point | 1330 °C | 330 °C | | density | 3.123 g/cm^3 | 1.2051 g/cm^3 | | 4.43 g/cm^3 solubility in water | | | soluble | dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | | odor | | | odorless | odorless
| potassium iodide | magnesium nitrate | potassium nitrate | magnesium iodide molar mass | 166.0028 g/mol | 148.31 g/mol | 101.1 g/mol | 278.114 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 681 °C | 88.9 °C | 334 °C | 637 °C boiling point | 1330 °C | 330 °C | | density | 3.123 g/cm^3 | 1.2051 g/cm^3 | | 4.43 g/cm^3 solubility in water | | | soluble | dynamic viscosity | 0.0010227 Pa s (at 732.9 °C) | | | odor | | | odorless | odorless

Units

Random Queries

block of carbon
chemical uses of sulfurous acid
name of ammonium-d 4bromide vs acetyl fluoride
H2O + KBrO3 + Na2C2O4 = NaOH + CO2 + KBr
CAS number of cyclohexanebutyric acid vs 1,8-dibromooctane
net ionic charge of antimonate anion vs phosphate anion
atomic mass of sodium
atomic radius of arsenic
element types of tin(II) cation
CAS number of potassium periodate vs sodium fluoride