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H2SO4 + NaAlO2 = H2O + Na2SO4 + Al2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + AlNaO_2 sodium aluminate ⟶ H_2O water + Na_2SO_4 sodium sulfate + Al_2(SO_4)_3 aluminum sulfate
H_2SO_4 sulfuric acid + AlNaO_2 sodium aluminate ⟶ H_2O water + Na_2SO_4 sodium sulfate + Al_2(SO_4)_3 aluminum sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + AlNaO_2 ⟶ H_2O + Na_2SO_4 + Al_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 AlNaO_2 ⟶ c_3 H_2O + c_4 Na_2SO_4 + c_5 Al_2(SO_4)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Al and Na: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 + 12 c_5 S: | c_1 = c_4 + 3 c_5 Al: | c_2 = 2 c_5 Na: | c_2 = 2 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 2 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 2 AlNaO_2 ⟶ 4 H_2O + Na_2SO_4 + Al_2(SO_4)_3
Balance the chemical equation algebraically: H_2SO_4 + AlNaO_2 ⟶ H_2O + Na_2SO_4 + Al_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 AlNaO_2 ⟶ c_3 H_2O + c_4 Na_2SO_4 + c_5 Al_2(SO_4)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Al and Na: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 + 12 c_5 S: | c_1 = c_4 + 3 c_5 Al: | c_2 = 2 c_5 Na: | c_2 = 2 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 2 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 2 AlNaO_2 ⟶ 4 H_2O + Na_2SO_4 + Al_2(SO_4)_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

sulfuric acid + sodium aluminate ⟶ water + sodium sulfate + aluminum sulfate
sulfuric acid + sodium aluminate ⟶ water + sodium sulfate + aluminum sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + AlNaO_2 ⟶ H_2O + Na_2SO_4 + Al_2(SO_4)_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: 4 H_2SO_4 + 2 AlNaO_2 ⟶ 4 H_2O + Na_2SO_4 + Al_2(SO_4)_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 H_2SO_4 | 4 | -4 AlNaO_2 | 2 | -2 H_2O | 4 | 4 Na_2SO_4 | 1 | 1 Al_2(SO_4)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 4 | -4 | ([H2SO4])^(-4) AlNaO_2 | 2 | -2 | ([AlNaO2])^(-2) H_2O | 4 | 4 | ([H2O])^4 Na_2SO_4 | 1 | 1 | [Na2SO4] Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] 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 = ([H2SO4])^(-4) ([AlNaO2])^(-2) ([H2O])^4 [Na2SO4] [Al2(SO4)3] = (([H2O])^4 [Na2SO4] [Al2(SO4)3])/(([H2SO4])^4 ([AlNaO2])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + AlNaO_2 ⟶ H_2O + Na_2SO_4 + Al_2(SO_4)_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: 4 H_2SO_4 + 2 AlNaO_2 ⟶ 4 H_2O + Na_2SO_4 + Al_2(SO_4)_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 H_2SO_4 | 4 | -4 AlNaO_2 | 2 | -2 H_2O | 4 | 4 Na_2SO_4 | 1 | 1 Al_2(SO_4)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 4 | -4 | ([H2SO4])^(-4) AlNaO_2 | 2 | -2 | ([AlNaO2])^(-2) H_2O | 4 | 4 | ([H2O])^4 Na_2SO_4 | 1 | 1 | [Na2SO4] Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] 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 = ([H2SO4])^(-4) ([AlNaO2])^(-2) ([H2O])^4 [Na2SO4] [Al2(SO4)3] = (([H2O])^4 [Na2SO4] [Al2(SO4)3])/(([H2SO4])^4 ([AlNaO2])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + AlNaO_2 ⟶ H_2O + Na_2SO_4 + Al_2(SO_4)_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: 4 H_2SO_4 + 2 AlNaO_2 ⟶ 4 H_2O + Na_2SO_4 + Al_2(SO_4)_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 H_2SO_4 | 4 | -4 AlNaO_2 | 2 | -2 H_2O | 4 | 4 Na_2SO_4 | 1 | 1 Al_2(SO_4)_3 | 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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) AlNaO_2 | 2 | -2 | -1/2 (Δ[AlNaO2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(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 = -1/4 (Δ[H2SO4])/(Δt) = -1/2 (Δ[AlNaO2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[Na2SO4])/(Δt) = (Δ[Al2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + AlNaO_2 ⟶ H_2O + Na_2SO_4 + Al_2(SO_4)_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: 4 H_2SO_4 + 2 AlNaO_2 ⟶ 4 H_2O + Na_2SO_4 + Al_2(SO_4)_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 H_2SO_4 | 4 | -4 AlNaO_2 | 2 | -2 H_2O | 4 | 4 Na_2SO_4 | 1 | 1 Al_2(SO_4)_3 | 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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) AlNaO_2 | 2 | -2 | -1/2 (Δ[AlNaO2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(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 = -1/4 (Δ[H2SO4])/(Δt) = -1/2 (Δ[AlNaO2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[Na2SO4])/(Δt) = (Δ[Al2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | sodium aluminate | water | sodium sulfate | aluminum sulfate formula | H_2SO_4 | AlNaO_2 | H_2O | Na_2SO_4 | Al_2(SO_4)_3 Hill formula | H_2O_4S | AlNaO_2 | H_2O | Na_2O_4S | Al_2O_12S_3 name | sulfuric acid | sodium aluminate | water | sodium sulfate | aluminum sulfate IUPAC name | sulfuric acid | sodium oxido-oxo-alumane | water | disodium sulfate | dialuminum trisulfate
| sulfuric acid | sodium aluminate | water | sodium sulfate | aluminum sulfate formula | H_2SO_4 | AlNaO_2 | H_2O | Na_2SO_4 | Al_2(SO_4)_3 Hill formula | H_2O_4S | AlNaO_2 | H_2O | Na_2O_4S | Al_2O_12S_3 name | sulfuric acid | sodium aluminate | water | sodium sulfate | aluminum sulfate IUPAC name | sulfuric acid | sodium oxido-oxo-alumane | water | disodium sulfate | dialuminum trisulfate

Substance properties

| sulfuric acid | sodium aluminate | water | sodium sulfate | aluminum sulfate molar mass | 98.07 g/mol | 81.969 g/mol | 18.015 g/mol | 142.04 g/mol | 342.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 10.371 °C | 1800 °C | 0 °C | 884 °C | 770 °C boiling point | 279.6 °C | | 99.9839 °C | 1429 °C | density | 1.8305 g/cm^3 | 1.5 g/cm^3 | 1 g/cm^3 | 2.68 g/cm^3 | 2.71 g/cm^3 solubility in water | very soluble | soluble | | soluble | soluble surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |
| sulfuric acid | sodium aluminate | water | sodium sulfate | aluminum sulfate molar mass | 98.07 g/mol | 81.969 g/mol | 18.015 g/mol | 142.04 g/mol | 342.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 10.371 °C | 1800 °C | 0 °C | 884 °C | 770 °C boiling point | 279.6 °C | | 99.9839 °C | 1429 °C | density | 1.8305 g/cm^3 | 1.5 g/cm^3 | 1 g/cm^3 | 2.68 g/cm^3 | 2.71 g/cm^3 solubility in water | very soluble | soluble | | soluble | soluble surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |

Units

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