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K2SO4 + NaNO3 = Na2SO4 + KNO3

Input interpretation

K_2SO_4 potassium sulfate + NaNO_3 sodium nitrate ⟶ Na_2SO_4 sodium sulfate + KNO_3 potassium nitrate
K_2SO_4 potassium sulfate + NaNO_3 sodium nitrate ⟶ Na_2SO_4 sodium sulfate + KNO_3 potassium nitrate

Balanced equation

Balance the chemical equation algebraically: K_2SO_4 + NaNO_3 ⟶ Na_2SO_4 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2SO_4 + c_2 NaNO_3 ⟶ c_3 Na_2SO_4 + c_4 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for K, O, S, N and Na: K: | 2 c_1 = c_4 O: | 4 c_1 + 3 c_2 = 4 c_3 + 3 c_4 S: | c_1 = c_3 N: | c_2 = c_4 Na: | c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K_2SO_4 + 2 NaNO_3 ⟶ Na_2SO_4 + 2 KNO_3
Balance the chemical equation algebraically: K_2SO_4 + NaNO_3 ⟶ Na_2SO_4 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2SO_4 + c_2 NaNO_3 ⟶ c_3 Na_2SO_4 + c_4 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for K, O, S, N and Na: K: | 2 c_1 = c_4 O: | 4 c_1 + 3 c_2 = 4 c_3 + 3 c_4 S: | c_1 = c_3 N: | c_2 = c_4 Na: | c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K_2SO_4 + 2 NaNO_3 ⟶ Na_2SO_4 + 2 KNO_3

Structures

+ ⟶ +
+ ⟶ +

Names

potassium sulfate + sodium nitrate ⟶ sodium sulfate + potassium nitrate
potassium sulfate + sodium nitrate ⟶ sodium sulfate + potassium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: K_2SO_4 + NaNO_3 ⟶ Na_2SO_4 + KNO_3 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: K_2SO_4 + 2 NaNO_3 ⟶ Na_2SO_4 + 2 KNO_3 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 K_2SO_4 | 1 | -1 NaNO_3 | 2 | -2 Na_2SO_4 | 1 | 1 KNO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2SO_4 | 1 | -1 | ([K2SO4])^(-1) NaNO_3 | 2 | -2 | ([NaNO3])^(-2) Na_2SO_4 | 1 | 1 | [Na2SO4] KNO_3 | 2 | 2 | ([KNO3])^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 = ([K2SO4])^(-1) ([NaNO3])^(-2) [Na2SO4] ([KNO3])^2 = ([Na2SO4] ([KNO3])^2)/([K2SO4] ([NaNO3])^2)
Construct the equilibrium constant, K, expression for: K_2SO_4 + NaNO_3 ⟶ Na_2SO_4 + KNO_3 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: K_2SO_4 + 2 NaNO_3 ⟶ Na_2SO_4 + 2 KNO_3 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 K_2SO_4 | 1 | -1 NaNO_3 | 2 | -2 Na_2SO_4 | 1 | 1 KNO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2SO_4 | 1 | -1 | ([K2SO4])^(-1) NaNO_3 | 2 | -2 | ([NaNO3])^(-2) Na_2SO_4 | 1 | 1 | [Na2SO4] KNO_3 | 2 | 2 | ([KNO3])^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 = ([K2SO4])^(-1) ([NaNO3])^(-2) [Na2SO4] ([KNO3])^2 = ([Na2SO4] ([KNO3])^2)/([K2SO4] ([NaNO3])^2)

Rate of reaction

Construct the rate of reaction expression for: K_2SO_4 + NaNO_3 ⟶ Na_2SO_4 + KNO_3 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: K_2SO_4 + 2 NaNO_3 ⟶ Na_2SO_4 + 2 KNO_3 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 K_2SO_4 | 1 | -1 NaNO_3 | 2 | -2 Na_2SO_4 | 1 | 1 KNO_3 | 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 K_2SO_4 | 1 | -1 | -(Δ[K2SO4])/(Δt) NaNO_3 | 2 | -2 | -1/2 (Δ[NaNO3])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(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 = -(Δ[K2SO4])/(Δt) = -1/2 (Δ[NaNO3])/(Δt) = (Δ[Na2SO4])/(Δt) = 1/2 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: K_2SO_4 + NaNO_3 ⟶ Na_2SO_4 + KNO_3 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: K_2SO_4 + 2 NaNO_3 ⟶ Na_2SO_4 + 2 KNO_3 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 K_2SO_4 | 1 | -1 NaNO_3 | 2 | -2 Na_2SO_4 | 1 | 1 KNO_3 | 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 K_2SO_4 | 1 | -1 | -(Δ[K2SO4])/(Δt) NaNO_3 | 2 | -2 | -1/2 (Δ[NaNO3])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(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 = -(Δ[K2SO4])/(Δt) = -1/2 (Δ[NaNO3])/(Δt) = (Δ[Na2SO4])/(Δt) = 1/2 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium sulfate | sodium nitrate | sodium sulfate | potassium nitrate formula | K_2SO_4 | NaNO_3 | Na_2SO_4 | KNO_3 Hill formula | K_2O_4S | NNaO_3 | Na_2O_4S | KNO_3 name | potassium sulfate | sodium nitrate | sodium sulfate | potassium nitrate IUPAC name | dipotassium sulfate | sodium nitrate | disodium sulfate | potassium nitrate
| potassium sulfate | sodium nitrate | sodium sulfate | potassium nitrate formula | K_2SO_4 | NaNO_3 | Na_2SO_4 | KNO_3 Hill formula | K_2O_4S | NNaO_3 | Na_2O_4S | KNO_3 name | potassium sulfate | sodium nitrate | sodium sulfate | potassium nitrate IUPAC name | dipotassium sulfate | sodium nitrate | disodium sulfate | potassium nitrate

Substance properties

| potassium sulfate | sodium nitrate | sodium sulfate | potassium nitrate molar mass | 174.25 g/mol | 84.994 g/mol | 142.04 g/mol | 101.1 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 306 °C | 884 °C | 334 °C boiling point | | | 1429 °C | density | | 2.26 g/cm^3 | 2.68 g/cm^3 | solubility in water | soluble | soluble | soluble | soluble dynamic viscosity | | 0.003 Pa s (at 250 °C) | | odor | | | | odorless
| potassium sulfate | sodium nitrate | sodium sulfate | potassium nitrate molar mass | 174.25 g/mol | 84.994 g/mol | 142.04 g/mol | 101.1 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 306 °C | 884 °C | 334 °C boiling point | | | 1429 °C | density | | 2.26 g/cm^3 | 2.68 g/cm^3 | solubility in water | soluble | soluble | soluble | soluble dynamic viscosity | | 0.003 Pa s (at 250 °C) | | odor | | | | odorless

Units

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