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H2SO4 + HNO3 + NiSO4 = H2O + NO2 + Ni2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + HNO_3 nitric acid + NiSO_4 nickel(II) sulfate ⟶ H_2O water + NO_2 nitrogen dioxide + Ni2(SO4)3
H_2SO_4 sulfuric acid + HNO_3 nitric acid + NiSO_4 nickel(II) sulfate ⟶ H_2O water + NO_2 nitrogen dioxide + Ni2(SO4)3

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + HNO_3 + NiSO_4 ⟶ H_2O + NO_2 + Ni2(SO4)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HNO_3 + c_3 NiSO_4 ⟶ c_4 H_2O + c_5 NO_2 + c_6 Ni2(SO4)3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, N and Ni: H: | 2 c_1 + c_2 = 2 c_4 O: | 4 c_1 + 3 c_2 + 4 c_3 = c_4 + 2 c_5 + 12 c_6 S: | c_1 + c_3 = 3 c_6 N: | c_2 = c_5 Ni: | c_3 = 2 c_6 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 = 2 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: |   | H_2SO_4 + 2 HNO_3 + 2 NiSO_4 ⟶ 2 H_2O + 2 NO_2 + Ni2(SO4)3
Balance the chemical equation algebraically: H_2SO_4 + HNO_3 + NiSO_4 ⟶ H_2O + NO_2 + Ni2(SO4)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HNO_3 + c_3 NiSO_4 ⟶ c_4 H_2O + c_5 NO_2 + c_6 Ni2(SO4)3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, N and Ni: H: | 2 c_1 + c_2 = 2 c_4 O: | 4 c_1 + 3 c_2 + 4 c_3 = c_4 + 2 c_5 + 12 c_6 S: | c_1 + c_3 = 3 c_6 N: | c_2 = c_5 Ni: | c_3 = 2 c_6 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 = 2 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 HNO_3 + 2 NiSO_4 ⟶ 2 H_2O + 2 NO_2 + Ni2(SO4)3

Structures

 + + ⟶ + + Ni2(SO4)3
+ + ⟶ + + Ni2(SO4)3

Names

sulfuric acid + nitric acid + nickel(II) sulfate ⟶ water + nitrogen dioxide + Ni2(SO4)3
sulfuric acid + nitric acid + nickel(II) sulfate ⟶ water + nitrogen dioxide + Ni2(SO4)3

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + HNO_3 + NiSO_4 ⟶ H_2O + NO_2 + Ni2(SO4)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: H_2SO_4 + 2 HNO_3 + 2 NiSO_4 ⟶ 2 H_2O + 2 NO_2 + Ni2(SO4)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 | 1 | -1 HNO_3 | 2 | -2 NiSO_4 | 2 | -2 H_2O | 2 | 2 NO_2 | 2 | 2 Ni2(SO4)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 | 1 | -1 | ([H2SO4])^(-1) HNO_3 | 2 | -2 | ([HNO3])^(-2) NiSO_4 | 2 | -2 | ([NiSO4])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO_2 | 2 | 2 | ([NO2])^2 Ni2(SO4)3 | 1 | 1 | [Ni2(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])^(-1) ([HNO3])^(-2) ([NiSO4])^(-2) ([H2O])^2 ([NO2])^2 [Ni2(SO4)3] = (([H2O])^2 ([NO2])^2 [Ni2(SO4)3])/([H2SO4] ([HNO3])^2 ([NiSO4])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + HNO_3 + NiSO_4 ⟶ H_2O + NO_2 + Ni2(SO4)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: H_2SO_4 + 2 HNO_3 + 2 NiSO_4 ⟶ 2 H_2O + 2 NO_2 + Ni2(SO4)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 | 1 | -1 HNO_3 | 2 | -2 NiSO_4 | 2 | -2 H_2O | 2 | 2 NO_2 | 2 | 2 Ni2(SO4)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 | 1 | -1 | ([H2SO4])^(-1) HNO_3 | 2 | -2 | ([HNO3])^(-2) NiSO_4 | 2 | -2 | ([NiSO4])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO_2 | 2 | 2 | ([NO2])^2 Ni2(SO4)3 | 1 | 1 | [Ni2(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])^(-1) ([HNO3])^(-2) ([NiSO4])^(-2) ([H2O])^2 ([NO2])^2 [Ni2(SO4)3] = (([H2O])^2 ([NO2])^2 [Ni2(SO4)3])/([H2SO4] ([HNO3])^2 ([NiSO4])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + HNO_3 + NiSO_4 ⟶ H_2O + NO_2 + Ni2(SO4)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: H_2SO_4 + 2 HNO_3 + 2 NiSO_4 ⟶ 2 H_2O + 2 NO_2 + Ni2(SO4)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 | 1 | -1 HNO_3 | 2 | -2 NiSO_4 | 2 | -2 H_2O | 2 | 2 NO_2 | 2 | 2 Ni2(SO4)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 | 1 | -1 | -(Δ[H2SO4])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) NiSO_4 | 2 | -2 | -1/2 (Δ[NiSO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO_2 | 2 | 2 | 1/2 (Δ[NO2])/(Δt) Ni2(SO4)3 | 1 | 1 | (Δ[Ni2(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 = -(Δ[H2SO4])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/2 (Δ[NiSO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO2])/(Δt) = (Δ[Ni2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + HNO_3 + NiSO_4 ⟶ H_2O + NO_2 + Ni2(SO4)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: H_2SO_4 + 2 HNO_3 + 2 NiSO_4 ⟶ 2 H_2O + 2 NO_2 + Ni2(SO4)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 | 1 | -1 HNO_3 | 2 | -2 NiSO_4 | 2 | -2 H_2O | 2 | 2 NO_2 | 2 | 2 Ni2(SO4)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 | 1 | -1 | -(Δ[H2SO4])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) NiSO_4 | 2 | -2 | -1/2 (Δ[NiSO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO_2 | 2 | 2 | 1/2 (Δ[NO2])/(Δt) Ni2(SO4)3 | 1 | 1 | (Δ[Ni2(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 = -(Δ[H2SO4])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/2 (Δ[NiSO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO2])/(Δt) = (Δ[Ni2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | sulfuric acid | nitric acid | nickel(II) sulfate | water | nitrogen dioxide | Ni2(SO4)3 formula | H_2SO_4 | HNO_3 | NiSO_4 | H_2O | NO_2 | Ni2(SO4)3 Hill formula | H_2O_4S | HNO_3 | NiO_4S | H_2O | NO_2 | Ni2O12S3 name | sulfuric acid | nitric acid | nickel(II) sulfate | water | nitrogen dioxide |  IUPAC name | sulfuric acid | nitric acid | nickelous sulfate | water | Nitrogen dioxide |
| sulfuric acid | nitric acid | nickel(II) sulfate | water | nitrogen dioxide | Ni2(SO4)3 formula | H_2SO_4 | HNO_3 | NiSO_4 | H_2O | NO_2 | Ni2(SO4)3 Hill formula | H_2O_4S | HNO_3 | NiO_4S | H_2O | NO_2 | Ni2O12S3 name | sulfuric acid | nitric acid | nickel(II) sulfate | water | nitrogen dioxide | IUPAC name | sulfuric acid | nitric acid | nickelous sulfate | water | Nitrogen dioxide |

Substance properties

 | sulfuric acid | nitric acid | nickel(II) sulfate | water | nitrogen dioxide | Ni2(SO4)3 molar mass | 98.07 g/mol | 63.012 g/mol | 154.75 g/mol | 18.015 g/mol | 46.005 g/mol | 405.6 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) |  melting point | 10.371 °C | -41.6 °C | | 0 °C | -11 °C |  boiling point | 279.6 °C | 83 °C | | 99.9839 °C | 21 °C |  density | 1.8305 g/cm^3 | 1.5129 g/cm^3 | 4.01 g/cm^3 | 1 g/cm^3 | 0.00188 g/cm^3 (at 25 °C) |  solubility in water | very soluble | miscible | | | reacts |  surface tension | 0.0735 N/m | | | 0.0728 N/m | |  dynamic viscosity | 0.021 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) |  odor | odorless | | | odorless | |
| sulfuric acid | nitric acid | nickel(II) sulfate | water | nitrogen dioxide | Ni2(SO4)3 molar mass | 98.07 g/mol | 63.012 g/mol | 154.75 g/mol | 18.015 g/mol | 46.005 g/mol | 405.6 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | 10.371 °C | -41.6 °C | | 0 °C | -11 °C | boiling point | 279.6 °C | 83 °C | | 99.9839 °C | 21 °C | density | 1.8305 g/cm^3 | 1.5129 g/cm^3 | 4.01 g/cm^3 | 1 g/cm^3 | 0.00188 g/cm^3 (at 25 °C) | solubility in water | very soluble | miscible | | | reacts | surface tension | 0.0735 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) | odor | odorless | | | odorless | |

Units