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H2SO4 + CuNO3 = H2 + HNO3 + CuSO4

Input interpretation

H_2SO_4 sulfuric acid + CuNO3 ⟶ H_2 hydrogen + HNO_3 nitric acid + CuSO_4 copper(II) sulfate
H_2SO_4 sulfuric acid + CuNO3 ⟶ H_2 hydrogen + HNO_3 nitric acid + CuSO_4 copper(II) sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + CuNO3 ⟶ H_2 + HNO_3 + CuSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CuNO3 ⟶ c_3 H_2 + c_4 HNO_3 + c_5 CuSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cu and N: H: | 2 c_1 = 2 c_3 + c_4 O: | 4 c_1 + 3 c_2 = 3 c_4 + 4 c_5 S: | c_1 = c_5 Cu: | c_2 = c_5 N: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 CuNO3 ⟶ H_2 + 2 HNO_3 + 2 CuSO_4
Balance the chemical equation algebraically: H_2SO_4 + CuNO3 ⟶ H_2 + HNO_3 + CuSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CuNO3 ⟶ c_3 H_2 + c_4 HNO_3 + c_5 CuSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cu and N: H: | 2 c_1 = 2 c_3 + c_4 O: | 4 c_1 + 3 c_2 = 3 c_4 + 4 c_5 S: | c_1 = c_5 Cu: | c_2 = c_5 N: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 CuNO3 ⟶ H_2 + 2 HNO_3 + 2 CuSO_4

Structures

+ CuNO3 ⟶ + +
+ CuNO3 ⟶ + +

Names

sulfuric acid + CuNO3 ⟶ hydrogen + nitric acid + copper(II) sulfate
sulfuric acid + CuNO3 ⟶ hydrogen + nitric acid + copper(II) sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + CuNO3 ⟶ H_2 + HNO_3 + CuSO_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: 2 H_2SO_4 + 2 CuNO3 ⟶ H_2 + 2 HNO_3 + 2 CuSO_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 | 2 | -2 CuNO3 | 2 | -2 H_2 | 1 | 1 HNO_3 | 2 | 2 CuSO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) CuNO3 | 2 | -2 | ([CuNO3])^(-2) H_2 | 1 | 1 | [H2] HNO_3 | 2 | 2 | ([HNO3])^2 CuSO_4 | 2 | 2 | ([CuSO4])^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 = ([H2SO4])^(-2) ([CuNO3])^(-2) [H2] ([HNO3])^2 ([CuSO4])^2 = ([H2] ([HNO3])^2 ([CuSO4])^2)/(([H2SO4])^2 ([CuNO3])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + CuNO3 ⟶ H_2 + HNO_3 + CuSO_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: 2 H_2SO_4 + 2 CuNO3 ⟶ H_2 + 2 HNO_3 + 2 CuSO_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 | 2 | -2 CuNO3 | 2 | -2 H_2 | 1 | 1 HNO_3 | 2 | 2 CuSO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) CuNO3 | 2 | -2 | ([CuNO3])^(-2) H_2 | 1 | 1 | [H2] HNO_3 | 2 | 2 | ([HNO3])^2 CuSO_4 | 2 | 2 | ([CuSO4])^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 = ([H2SO4])^(-2) ([CuNO3])^(-2) [H2] ([HNO3])^2 ([CuSO4])^2 = ([H2] ([HNO3])^2 ([CuSO4])^2)/(([H2SO4])^2 ([CuNO3])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + CuNO3 ⟶ H_2 + HNO_3 + CuSO_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: 2 H_2SO_4 + 2 CuNO3 ⟶ H_2 + 2 HNO_3 + 2 CuSO_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 | 2 | -2 CuNO3 | 2 | -2 H_2 | 1 | 1 HNO_3 | 2 | 2 CuSO_4 | 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 H_2SO_4 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) CuNO3 | 2 | -2 | -1/2 (Δ[CuNO3])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) CuSO_4 | 2 | 2 | 1/2 (Δ[CuSO4])/(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[H2SO4])/(Δt) = -1/2 (Δ[CuNO3])/(Δt) = (Δ[H2])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = 1/2 (Δ[CuSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + CuNO3 ⟶ H_2 + HNO_3 + CuSO_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: 2 H_2SO_4 + 2 CuNO3 ⟶ H_2 + 2 HNO_3 + 2 CuSO_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 | 2 | -2 CuNO3 | 2 | -2 H_2 | 1 | 1 HNO_3 | 2 | 2 CuSO_4 | 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 H_2SO_4 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) CuNO3 | 2 | -2 | -1/2 (Δ[CuNO3])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) CuSO_4 | 2 | 2 | 1/2 (Δ[CuSO4])/(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[H2SO4])/(Δt) = -1/2 (Δ[CuNO3])/(Δt) = (Δ[H2])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = 1/2 (Δ[CuSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | CuNO3 | hydrogen | nitric acid | copper(II) sulfate formula | H_2SO_4 | CuNO3 | H_2 | HNO_3 | CuSO_4 Hill formula | H_2O_4S | CuNO3 | H_2 | HNO_3 | CuO_4S name | sulfuric acid | | hydrogen | nitric acid | copper(II) sulfate IUPAC name | sulfuric acid | | molecular hydrogen | nitric acid | copper sulfate
| sulfuric acid | CuNO3 | hydrogen | nitric acid | copper(II) sulfate formula | H_2SO_4 | CuNO3 | H_2 | HNO_3 | CuSO_4 Hill formula | H_2O_4S | CuNO3 | H_2 | HNO_3 | CuO_4S name | sulfuric acid | | hydrogen | nitric acid | copper(II) sulfate IUPAC name | sulfuric acid | | molecular hydrogen | nitric acid | copper sulfate

Substance properties

| sulfuric acid | CuNO3 | hydrogen | nitric acid | copper(II) sulfate molar mass | 98.07 g/mol | 125.55 g/mol | 2.016 g/mol | 63.012 g/mol | 159.6 g/mol phase | liquid (at STP) | | gas (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | | -259.2 °C | -41.6 °C | 200 °C boiling point | 279.6 °C | | -252.8 °C | 83 °C | density | 1.8305 g/cm^3 | | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 3.603 g/cm^3 solubility in water | very soluble | | | miscible | surface tension | 0.0735 N/m | | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless | |
| sulfuric acid | CuNO3 | hydrogen | nitric acid | copper(II) sulfate molar mass | 98.07 g/mol | 125.55 g/mol | 2.016 g/mol | 63.012 g/mol | 159.6 g/mol phase | liquid (at STP) | | gas (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | | -259.2 °C | -41.6 °C | 200 °C boiling point | 279.6 °C | | -252.8 °C | 83 °C | density | 1.8305 g/cm^3 | | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 3.603 g/cm^3 solubility in water | very soluble | | | miscible | surface tension | 0.0735 N/m | | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless | |

Units

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