NiO + 2HNO3 → Ni(NO3)2 + H2O
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- Reaction of nickel(II) oxide and nitric acid
The reaction of nickel(II) oxide and nitric acid yields nickel(II) nitrate and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of nickel(II) oxide and nitric acid
General equation
- Reaction of basic oxide and acid
- Basic oxideBrønsted base + AcidBrønsted acid ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of weakly basic oxide and strong acid
- Weakly basic oxideBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acid and weak baseConjugate base + H2OConjugate acid
Oxidation state of each atom
- Reaction of nickel(II) oxide and nitric acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NiO | Nickel(II) oxide | 1 | Brønsted base | Basic oxide Weakly basic oxide |
HNO3 | Nitric acid | 2 | Brønsted acid | Acid Strong acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Ni(NO3)2 | Nickel(II) nitrate | 1 | Conjugate base | Salt Salt of strong acid and weak base |
H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of nickel(II) oxide and nitric acid
Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
---|---|---|---|---|
per 1 mol of Equation | −113.0 | – | – | – |
per 1 mol of | −113.0 | – | – | – |
per 1 mol of | −56.50 | – | – | – |
per 1 mol of | −113.0 | – | – | – |
per 1 mol of | −113.0 | – | – | – |
Changes in aqueous solution
- Reaction of nickel(II) oxide and nitric acid◆
ΔrG −71.4 kJ/mol K 3.23 × 1012 pK −12.51
Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
---|---|---|---|---|
per 1 mol of Equation | −100.0 | −71.4 | −96.9 | – |
per 1 mol of | −100.0 | −71.4 | −96.9 | – |
per 1 mol of | −50.00 | −35.7 | −48.5 | – |
per 1 mol of | −100.0 | −71.4 | −96.9 | – |
per 1 mol of | −100.0 | −71.4 | −96.9 | – |
Thermodynamic data of reactants
Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
---|---|---|---|---|
NiO (cr) | -239.7[1] | -211.7[1] | 37.99[1] | 44.31[1] |
NiO (g) | 314[1] | – | – | – |
HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ai):Ionized aqueous solution
Thermodynamic data of products
Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
---|---|---|---|---|
Ni(NO3)2 (cr) | -415.1[1] | – | – | – |
Ni(NO3)2 (ai) | -468.6[1] | -268.5[1] | 164.0[1] | – |
Ni(NO3)2 (cr) 3 hydrate | -1326.3[1] | – | – | – |
Ni(NO3)2 (cr) 6 hydrate | -2211.7[1] | – | – | 464[1] |
H2O (cr) | – | – | – | – |
H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -239.7 kJ · mol−1
- ^ ΔfG°, -211.7 kJ · mol−1
- ^ S°, 37.99 J · K−1 · mol−1
- ^ Cp°, 44.31 J · K−1 · mol−1
- ^ ΔfH°, 314. kJ · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -415.1 kJ · mol−1
- ^ ΔfH°, -468.6 kJ · mol−1
- ^ ΔfG°, -268.5 kJ · mol−1
- ^ S°, 164.0 J · K−1 · mol−1
- ^ ΔfH°, -1326.3 kJ · mol−1
- ^ ΔfH°, -2211.7 kJ · mol−1
- ^ Cp°, 464. J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1