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Na2O + BaSO4 = Na2SO4 + BaO

Input interpretation

Na_2O sodium oxide + BaSO_4 barium sulfate ⟶ Na_2SO_4 sodium sulfate + BaO barium oxide
Na_2O sodium oxide + BaSO_4 barium sulfate ⟶ Na_2SO_4 sodium sulfate + BaO barium oxide

Balanced equation

Balance the chemical equation algebraically: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Na_2O + c_2 BaSO_4 ⟶ c_3 Na_2SO_4 + c_4 BaO Set the number of atoms in the reactants equal to the number of atoms in the products for Na, O, Ba and S: Na: | 2 c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + c_4 Ba: | c_2 = c_4 S: | c_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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: |   | Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO
Balance the chemical equation algebraically: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Na_2O + c_2 BaSO_4 ⟶ c_3 Na_2SO_4 + c_4 BaO Set the number of atoms in the reactants equal to the number of atoms in the products for Na, O, Ba and S: Na: | 2 c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + c_4 Ba: | c_2 = c_4 S: | c_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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO

Structures

 + ⟶ +
+ ⟶ +

Names

sodium oxide + barium sulfate ⟶ sodium sulfate + barium oxide
sodium oxide + barium sulfate ⟶ sodium sulfate + barium oxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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 Na_2O | 1 | -1 BaSO_4 | 1 | -1 Na_2SO_4 | 1 | 1 BaO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Na_2O | 1 | -1 | ([Na2O])^(-1) BaSO_4 | 1 | -1 | ([BaSO4])^(-1) Na_2SO_4 | 1 | 1 | [Na2SO4] BaO | 1 | 1 | [BaO] 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 = ([Na2O])^(-1) ([BaSO4])^(-1) [Na2SO4] [BaO] = ([Na2SO4] [BaO])/([Na2O] [BaSO4])
Construct the equilibrium constant, K, expression for: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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 Na_2O | 1 | -1 BaSO_4 | 1 | -1 Na_2SO_4 | 1 | 1 BaO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Na_2O | 1 | -1 | ([Na2O])^(-1) BaSO_4 | 1 | -1 | ([BaSO4])^(-1) Na_2SO_4 | 1 | 1 | [Na2SO4] BaO | 1 | 1 | [BaO] 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 = ([Na2O])^(-1) ([BaSO4])^(-1) [Na2SO4] [BaO] = ([Na2SO4] [BaO])/([Na2O] [BaSO4])

Rate of reaction

Construct the rate of reaction expression for: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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 Na_2O | 1 | -1 BaSO_4 | 1 | -1 Na_2SO_4 | 1 | 1 BaO | 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 Na_2O | 1 | -1 | -(Δ[Na2O])/(Δt) BaSO_4 | 1 | -1 | -(Δ[BaSO4])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) BaO | 1 | 1 | (Δ[BaO])/(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[Na2O])/(Δt) = -(Δ[BaSO4])/(Δt) = (Δ[Na2SO4])/(Δt) = (Δ[BaO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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: Na_2O + BaSO_4 ⟶ Na_2SO_4 + BaO 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 Na_2O | 1 | -1 BaSO_4 | 1 | -1 Na_2SO_4 | 1 | 1 BaO | 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 Na_2O | 1 | -1 | -(Δ[Na2O])/(Δt) BaSO_4 | 1 | -1 | -(Δ[BaSO4])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) BaO | 1 | 1 | (Δ[BaO])/(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[Na2O])/(Δt) = -(Δ[BaSO4])/(Δt) = (Δ[Na2SO4])/(Δt) = (Δ[BaO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | sodium oxide | barium sulfate | sodium sulfate | barium oxide formula | Na_2O | BaSO_4 | Na_2SO_4 | BaO Hill formula | Na_2O | BaO_4S | Na_2O_4S | BaO name | sodium oxide | barium sulfate | sodium sulfate | barium oxide IUPAC name | disodium oxygen(-2) anion | barium(+2) cation sulfate | disodium sulfate | oxobarium
| sodium oxide | barium sulfate | sodium sulfate | barium oxide formula | Na_2O | BaSO_4 | Na_2SO_4 | BaO Hill formula | Na_2O | BaO_4S | Na_2O_4S | BaO name | sodium oxide | barium sulfate | sodium sulfate | barium oxide IUPAC name | disodium oxygen(-2) anion | barium(+2) cation sulfate | disodium sulfate | oxobarium

Substance properties

 | sodium oxide | barium sulfate | sodium sulfate | barium oxide molar mass | 61.979 g/mol | 233.38 g/mol | 142.04 g/mol | 153.326 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 1345 °C | 884 °C | 1920 °C boiling point | | | 1429 °C |  density | 2.27 g/cm^3 | 4.5 g/cm^3 | 2.68 g/cm^3 | 5.72 g/cm^3 solubility in water | | insoluble | soluble |
| sodium oxide | barium sulfate | sodium sulfate | barium oxide molar mass | 61.979 g/mol | 233.38 g/mol | 142.04 g/mol | 153.326 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 1345 °C | 884 °C | 1920 °C boiling point | | | 1429 °C | density | 2.27 g/cm^3 | 4.5 g/cm^3 | 2.68 g/cm^3 | 5.72 g/cm^3 solubility in water | | insoluble | soluble |

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