Input interpretation
![HNO_3 nitric acid + NiOOH ⟶ H_2O water + O_2 oxygen + Ni(NO_3)_2 nickel(II) nitrate](../image_source/151b48ed59b0c619d1e58ac0e5d9dea5.png)
HNO_3 nitric acid + NiOOH ⟶ H_2O water + O_2 oxygen + Ni(NO_3)_2 nickel(II) nitrate
Balanced equation
![Balance the chemical equation algebraically: HNO_3 + NiOOH ⟶ H_2O + O_2 + Ni(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 NiOOH ⟶ c_3 H_2O + c_4 O_2 + c_5 Ni(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Ni: H: | c_1 + c_2 = 2 c_3 N: | c_1 = 2 c_5 O: | 3 c_1 + 2 c_2 = c_3 + 2 c_4 + 6 c_5 Ni: | c_2 = c_5 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 = 8 c_2 = 4 c_3 = 6 c_4 = 1 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + 4 NiOOH ⟶ 6 H_2O + O_2 + 4 Ni(NO_3)_2](../image_source/b73a0b59e6ae35eedfad21933a245fe8.png)
Balance the chemical equation algebraically: HNO_3 + NiOOH ⟶ H_2O + O_2 + Ni(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 NiOOH ⟶ c_3 H_2O + c_4 O_2 + c_5 Ni(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Ni: H: | c_1 + c_2 = 2 c_3 N: | c_1 = 2 c_5 O: | 3 c_1 + 2 c_2 = c_3 + 2 c_4 + 6 c_5 Ni: | c_2 = c_5 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 = 8 c_2 = 4 c_3 = 6 c_4 = 1 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + 4 NiOOH ⟶ 6 H_2O + O_2 + 4 Ni(NO_3)_2
Structures
![+ NiOOH ⟶ + +](../image_source/caf8c8c974e7deea47e1b712a7a85d2c.png)
+ NiOOH ⟶ + +
Names
![nitric acid + NiOOH ⟶ water + oxygen + nickel(II) nitrate](../image_source/e02b128d3b88107d63ba7a9a5c44957d.png)
nitric acid + NiOOH ⟶ water + oxygen + nickel(II) nitrate
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HNO_3 + NiOOH ⟶ H_2O + O_2 + Ni(NO_3)_2 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: 8 HNO_3 + 4 NiOOH ⟶ 6 H_2O + O_2 + 4 Ni(NO_3)_2 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 HNO_3 | 8 | -8 NiOOH | 4 | -4 H_2O | 6 | 6 O_2 | 1 | 1 Ni(NO_3)_2 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 8 | -8 | ([HNO3])^(-8) NiOOH | 4 | -4 | ([NiOOH])^(-4) H_2O | 6 | 6 | ([H2O])^6 O_2 | 1 | 1 | [O2] Ni(NO_3)_2 | 4 | 4 | ([Ni(NO3)2])^4 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 = ([HNO3])^(-8) ([NiOOH])^(-4) ([H2O])^6 [O2] ([Ni(NO3)2])^4 = (([H2O])^6 [O2] ([Ni(NO3)2])^4)/(([HNO3])^8 ([NiOOH])^4)](../image_source/79001c1229f9f95d483a735d520e8fdb.png)
Construct the equilibrium constant, K, expression for: HNO_3 + NiOOH ⟶ H_2O + O_2 + Ni(NO_3)_2 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: 8 HNO_3 + 4 NiOOH ⟶ 6 H_2O + O_2 + 4 Ni(NO_3)_2 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 HNO_3 | 8 | -8 NiOOH | 4 | -4 H_2O | 6 | 6 O_2 | 1 | 1 Ni(NO_3)_2 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 8 | -8 | ([HNO3])^(-8) NiOOH | 4 | -4 | ([NiOOH])^(-4) H_2O | 6 | 6 | ([H2O])^6 O_2 | 1 | 1 | [O2] Ni(NO_3)_2 | 4 | 4 | ([Ni(NO3)2])^4 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 = ([HNO3])^(-8) ([NiOOH])^(-4) ([H2O])^6 [O2] ([Ni(NO3)2])^4 = (([H2O])^6 [O2] ([Ni(NO3)2])^4)/(([HNO3])^8 ([NiOOH])^4)
Rate of reaction
![Construct the rate of reaction expression for: HNO_3 + NiOOH ⟶ H_2O + O_2 + Ni(NO_3)_2 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: 8 HNO_3 + 4 NiOOH ⟶ 6 H_2O + O_2 + 4 Ni(NO_3)_2 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 HNO_3 | 8 | -8 NiOOH | 4 | -4 H_2O | 6 | 6 O_2 | 1 | 1 Ni(NO_3)_2 | 4 | 4 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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) NiOOH | 4 | -4 | -1/4 (Δ[NiOOH])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) Ni(NO_3)_2 | 4 | 4 | 1/4 (Δ[Ni(NO3)2])/(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 = -1/8 (Δ[HNO3])/(Δt) = -1/4 (Δ[NiOOH])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = 1/4 (Δ[Ni(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/45a733048066a731598c10274abfb96c.png)
Construct the rate of reaction expression for: HNO_3 + NiOOH ⟶ H_2O + O_2 + Ni(NO_3)_2 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: 8 HNO_3 + 4 NiOOH ⟶ 6 H_2O + O_2 + 4 Ni(NO_3)_2 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 HNO_3 | 8 | -8 NiOOH | 4 | -4 H_2O | 6 | 6 O_2 | 1 | 1 Ni(NO_3)_2 | 4 | 4 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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) NiOOH | 4 | -4 | -1/4 (Δ[NiOOH])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) Ni(NO_3)_2 | 4 | 4 | 1/4 (Δ[Ni(NO3)2])/(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 = -1/8 (Δ[HNO3])/(Δt) = -1/4 (Δ[NiOOH])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = 1/4 (Δ[Ni(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| nitric acid | NiOOH | water | oxygen | nickel(II) nitrate formula | HNO_3 | NiOOH | H_2O | O_2 | Ni(NO_3)_2 Hill formula | HNO_3 | HNiO2 | H_2O | O_2 | N_2NiO_6 name | nitric acid | | water | oxygen | nickel(II) nitrate IUPAC name | nitric acid | | water | molecular oxygen | nickel(+2) dinitrate](../image_source/57713ddfa2585dd0ab019baf33cc5f0e.png)
| nitric acid | NiOOH | water | oxygen | nickel(II) nitrate formula | HNO_3 | NiOOH | H_2O | O_2 | Ni(NO_3)_2 Hill formula | HNO_3 | HNiO2 | H_2O | O_2 | N_2NiO_6 name | nitric acid | | water | oxygen | nickel(II) nitrate IUPAC name | nitric acid | | water | molecular oxygen | nickel(+2) dinitrate
Substance properties
![| nitric acid | NiOOH | water | oxygen | nickel(II) nitrate molar mass | 63.012 g/mol | 91.699 g/mol | 18.015 g/mol | 31.998 g/mol | 182.7 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | | 0 °C | -218 °C | 57 °C boiling point | 83 °C | | 99.9839 °C | -183 °C | 137 °C density | 1.5129 g/cm^3 | | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 1.77 g/cm^3 solubility in water | miscible | | | | surface tension | | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |](../image_source/323e5070406b95664b55ffc4af383127.png)
| nitric acid | NiOOH | water | oxygen | nickel(II) nitrate molar mass | 63.012 g/mol | 91.699 g/mol | 18.015 g/mol | 31.998 g/mol | 182.7 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | | 0 °C | -218 °C | 57 °C boiling point | 83 °C | | 99.9839 °C | -183 °C | 137 °C density | 1.5129 g/cm^3 | | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 1.77 g/cm^3 solubility in water | miscible | | | | surface tension | | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |
Units