Input interpretation
![H_2SO_4 sulfuric acid + NaNO_3 sodium nitrate ⟶ HNO_3 nitric acid + NaHSO_4 sodium bisulfate](../image_source/c0d1d903db30861542fff028ce488fb4.png)
H_2SO_4 sulfuric acid + NaNO_3 sodium nitrate ⟶ HNO_3 nitric acid + NaHSO_4 sodium bisulfate
Balanced equation
![Balance the chemical equation algebraically: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 NaNO_3 ⟶ c_3 HNO_3 + c_4 NaHSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, N and Na: H: | 2 c_1 = c_3 + c_4 O: | 4 c_1 + 3 c_2 = 3 c_3 + 4 c_4 S: | c_1 = c_4 N: | c_2 = c_3 Na: | c_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_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: | | H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4](../image_source/5de94b6f25689cb66bd68b291ce847e7.png)
Balance the chemical equation algebraically: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 NaNO_3 ⟶ c_3 HNO_3 + c_4 NaHSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, N and Na: H: | 2 c_1 = c_3 + c_4 O: | 4 c_1 + 3 c_2 = 3 c_3 + 4 c_4 S: | c_1 = c_4 N: | c_2 = c_3 Na: | c_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_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: | | H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4
Structures
![+ ⟶ +](../image_source/7fa34f1a1fbef4e1d0acbd078a13a7bc.png)
+ ⟶ +
Names
![sulfuric acid + sodium nitrate ⟶ nitric acid + sodium bisulfate](../image_source/eef8bc35d56dce88d46ad0876efab7b8.png)
sulfuric acid + sodium nitrate ⟶ nitric acid + sodium bisulfate
Reaction thermodynamics
Gibbs free energy
![| sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate molecular free energy | -690 kJ/mol | -366 kJ/mol | -80.7 kJ/mol | -992.8 kJ/mol total free energy | -690 kJ/mol | -366 kJ/mol | -80.7 kJ/mol | -992.8 kJ/mol | G_initial = -1056 kJ/mol | | G_final = -1074 kJ/mol | ΔG_rxn^0 | -1074 kJ/mol - -1056 kJ/mol = -17.5 kJ/mol (exergonic) | | |](../image_source/e2f16a3a55683b96dd4a2b8860b5b3e3.png)
| sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate molecular free energy | -690 kJ/mol | -366 kJ/mol | -80.7 kJ/mol | -992.8 kJ/mol total free energy | -690 kJ/mol | -366 kJ/mol | -80.7 kJ/mol | -992.8 kJ/mol | G_initial = -1056 kJ/mol | | G_final = -1074 kJ/mol | ΔG_rxn^0 | -1074 kJ/mol - -1056 kJ/mol = -17.5 kJ/mol (exergonic) | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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 | 1 | -1 NaNO_3 | 1 | -1 HNO_3 | 1 | 1 NaHSO_4 | 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 | 1 | -1 | ([H2SO4])^(-1) NaNO_3 | 1 | -1 | ([NaNO3])^(-1) HNO_3 | 1 | 1 | [HNO3] NaHSO_4 | 1 | 1 | [NaHSO4] 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])^(-1) ([NaNO3])^(-1) [HNO3] [NaHSO4] = ([HNO3] [NaHSO4])/([H2SO4] [NaNO3])](../image_source/9980a22d3dd4d9a2724a7d051cf99a5e.png)
Construct the equilibrium constant, K, expression for: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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 | 1 | -1 NaNO_3 | 1 | -1 HNO_3 | 1 | 1 NaHSO_4 | 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 | 1 | -1 | ([H2SO4])^(-1) NaNO_3 | 1 | -1 | ([NaNO3])^(-1) HNO_3 | 1 | 1 | [HNO3] NaHSO_4 | 1 | 1 | [NaHSO4] 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])^(-1) ([NaNO3])^(-1) [HNO3] [NaHSO4] = ([HNO3] [NaHSO4])/([H2SO4] [NaNO3])
Rate of reaction
![Construct the rate of reaction expression for: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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 | 1 | -1 NaNO_3 | 1 | -1 HNO_3 | 1 | 1 NaHSO_4 | 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) NaNO_3 | 1 | -1 | -(Δ[NaNO3])/(Δt) HNO_3 | 1 | 1 | (Δ[HNO3])/(Δt) NaHSO_4 | 1 | 1 | (Δ[NaHSO4])/(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[H2SO4])/(Δt) = -(Δ[NaNO3])/(Δt) = (Δ[HNO3])/(Δt) = (Δ[NaHSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/4fd678ec8fc4c38b77e7b9db2b6ef116.png)
Construct the rate of reaction expression for: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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: H_2SO_4 + NaNO_3 ⟶ HNO_3 + NaHSO_4 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 | 1 | -1 NaNO_3 | 1 | -1 HNO_3 | 1 | 1 NaHSO_4 | 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) NaNO_3 | 1 | -1 | -(Δ[NaNO3])/(Δt) HNO_3 | 1 | 1 | (Δ[HNO3])/(Δt) NaHSO_4 | 1 | 1 | (Δ[NaHSO4])/(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[H2SO4])/(Δt) = -(Δ[NaNO3])/(Δt) = (Δ[HNO3])/(Δt) = (Δ[NaHSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate formula | H_2SO_4 | NaNO_3 | HNO_3 | NaHSO_4 Hill formula | H_2O_4S | NNaO_3 | HNO_3 | HNaO_4S name | sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate](../image_source/6b7f2a94117cec2ace5f817dfc90b75d.png)
| sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate formula | H_2SO_4 | NaNO_3 | HNO_3 | NaHSO_4 Hill formula | H_2O_4S | NNaO_3 | HNO_3 | HNaO_4S name | sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate
Substance properties
![| sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate molar mass | 98.07 g/mol | 84.994 g/mol | 63.012 g/mol | 120.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | 306 °C | -41.6 °C | 181.85 °C boiling point | 279.6 °C | | 83 °C | density | 1.8305 g/cm^3 | 2.26 g/cm^3 | 1.5129 g/cm^3 | 1.8 g/cm^3 solubility in water | very soluble | soluble | miscible | surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.003 Pa s (at 250 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | |](../image_source/db416a2247845b0660706a9660883cdc.png)
| sulfuric acid | sodium nitrate | nitric acid | sodium bisulfate molar mass | 98.07 g/mol | 84.994 g/mol | 63.012 g/mol | 120.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | 306 °C | -41.6 °C | 181.85 °C boiling point | 279.6 °C | | 83 °C | density | 1.8305 g/cm^3 | 2.26 g/cm^3 | 1.5129 g/cm^3 | 1.8 g/cm^3 solubility in water | very soluble | soluble | miscible | surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.003 Pa s (at 250 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | |
Units