Search

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

Random Queries

ions of hydrogen bromide vs perchloric acid
atomic diameter of bismuth vs aluminum
common compound names of berkelium
density of diphosphoryl chloride
formula of silver(I) picrate monohydrate
Fe + KNO3 = N2 + Fe2O3 + K2O
molar mass of dioxygenyl cation vs titanyl cation
melting point of potassium hydroxide vs copper(II) sulfate
HCl + NaNO3 + Ag = H2 + NaCl + AgNO3
DrugBank number of aspirin