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2HSCN + 6H2O 💧⚡→ 2SO2↑ + NH4NO2 + 2CH4↑ + H2↑

2HSCN + 6H₂O 💧⚡→ 2SO₂↑ + NH₄NO₂ + 2CH₄↑ + H₂↑

Last updated: June 13, 2022

Electrolysis of aqueous thiocyanic acid with water as non-redox agent: 2HSCNThiocyanic acid + 6H₂OWater
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2SO₂↑Sulfur dioxide + NH₄NO₂Ammonium nitrite + 2CH₄↑Methane + H₂↑Hydrogen

Electrolysis of aqueous thiocyanic acid yields sulfur dioxide, ammonium nitrite, methane, and hydrogen (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Electrolysis of aqueous solution with water as non redox agent

Table of contents

Reaction data

Chemical equation

Electrolysis of aqueous thiocyanic acid with water as non-redox agent: 2HSCNThiocyanic acid + 6H₂OWater
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2SO₂↑Sulfur dioxide + NH₄NO₂Ammonium nitrite + 2CH₄↑Methane + H₂↑Hydrogen

General equation

Electrolysis of aqueous solution with water as non redox agent: Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H₂ONon-redox agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous thiocyanic acid with water as non-redox agent

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
HSCN	Thiocyanic acid	2	Self redox agent	Miscible with water
H₂O	Water	6	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
SO₂	Sulfur dioxide	2	Oxidized	–
NH₄NO₂	Ammonium nitrite	1	Oxidized	–
CH₄	Methane	2	Reduced	–
H₂	Hydrogen	1	–	–

Thermodynamic changes

Changes in aqueous solution (1)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 423.9 kJ/mol K 0.54 × 10⁻⁷⁴ pK 74.26: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	581.6	423.9	528.0	−209.8
per 1 mol of Thiocyanic acid	290.8	211.9	264.0	−104.9
per 1 mol of Water	96.93	70.65	88.00	−34.97
per 1 mol of Sulfur dioxide	290.8	211.9	264.0	−104.9
per 1 mol of Ammonium nitrite	581.6	423.9	528.0	−209.8
per 1 mol of Methane	290.8	211.9	264.0	−104.9
per 1 mol of Hydrogen	581.6	423.9	528.0	−209.8

Changes in aqueous solution (2)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 441.5 kJ/mol K 0.45 × 10⁻⁷⁷ pK 77.35: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	577.4	441.5	974	–
per 1 mol of Thiocyanic acid	288.7	220.8	487	–
per 1 mol of Water	96.23	73.58	162	–
per 1 mol of Sulfur dioxide	288.7	220.8	487	–
per 1 mol of Ammonium nitrite	577.4	441.5	974	–
per 1 mol of Methane	288.7	220.8	487	–
per 1 mol of Hydrogen	577.4	441.5	974	–

Changes in aqueous solution (3)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 456.7 kJ/mol K 0.98 × 10⁻⁸⁰ pK 80.01: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	553.2	456.7	322.9	–
per 1 mol of Thiocyanic acid	276.6	228.3	161.4	–
per 1 mol of Water	92.20	76.12	53.82	–
per 1 mol of Sulfur dioxide	276.6	228.3	161.4	–
per 1 mol of Ammonium nitrite	553.2	456.7	322.9	–
per 1 mol of Methane	276.6	228.3	161.4	–
per 1 mol of Hydrogen	553.2	456.7	322.9	–

Changes in aqueous solution (4)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 474.3 kJ/mol K 0.81 × 10⁻⁸³ pK 83.09: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	549.0	474.3	769	–
per 1 mol of Thiocyanic acid	274.5	237.2	385	–
per 1 mol of Water	91.50	79.05	128	–
per 1 mol of Sulfur dioxide	274.5	237.2	385	–
per 1 mol of Ammonium nitrite	549.0	474.3	769	–
per 1 mol of Methane	274.5	237.2	385	–
per 1 mol of Hydrogen	549.0	474.3	769	–

Changes in aqueous solution (5)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 423.0 kJ/mol K 0.78 × 10⁻⁷⁴ pK 74.11: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	529.3	423.0	355.4	–
per 1 mol of Thiocyanic acid	264.6	211.5	177.7	–
per 1 mol of Water	88.22	70.50	59.23	–
per 1 mol of Sulfur dioxide	264.6	211.5	177.7	–
per 1 mol of Ammonium nitrite	529.3	423.0	355.4	–
per 1 mol of Methane	264.6	211.5	177.7	–
per 1 mol of Hydrogen	529.3	423.0	355.4	–

Changes in aqueous solution (6)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 440.6 kJ/mol K 0.65 × 10⁻⁷⁷ pK 77.19: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	525.1	440.6	802	–
per 1 mol of Thiocyanic acid	262.6	220.3	401	–
per 1 mol of Water	87.52	73.43	134	–
per 1 mol of Sulfur dioxide	262.6	220.3	401	–
per 1 mol of Ammonium nitrite	525.1	440.6	802	–
per 1 mol of Methane	262.6	220.3	401	–
per 1 mol of Hydrogen	525.1	440.6	802	–

Changes in aqueous solution (7)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 455.7 kJ/mol K 0.15 × 10⁻⁷⁹ pK 79.84: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	500.9	455.7	150.2	–
per 1 mol of Thiocyanic acid	250.4	227.8	75.10	–
per 1 mol of Water	83.48	75.95	25.03	–
per 1 mol of Sulfur dioxide	250.4	227.8	75.10	–
per 1 mol of Ammonium nitrite	500.9	455.7	150.2	–
per 1 mol of Methane	250.4	227.8	75.10	–
per 1 mol of Hydrogen	500.9	455.7	150.2	–

Changes in aqueous solution (8)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 473.3 kJ/mol K 0.12 × 10⁻⁸² pK 82.92: 2HSCNIonized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	496.7	473.3	597	–
per 1 mol of Thiocyanic acid	248.3	236.7	299	–
per 1 mol of Water	82.78	78.88	99.5	–
per 1 mol of Sulfur dioxide	248.3	236.7	299	–
per 1 mol of Ammonium nitrite	496.7	473.3	597	–
per 1 mol of Methane	248.3	236.7	299	–
per 1 mol of Hydrogen	496.7	473.3	597	–

Changes in aqueous solution (9)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 414.2 kJ/mol K 0.27 × 10⁻⁷² pK 72.56: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	414.2	–	–
per 1 mol of Thiocyanic acid	–	207.1	–	–
per 1 mol of Water	–	69.03	–	–
per 1 mol of Sulfur dioxide	–	207.1	–	–
per 1 mol of Ammonium nitrite	–	414.2	–	–
per 1 mol of Methane	–	207.1	–	–
per 1 mol of Hydrogen	–	414.2	–	–

Changes in aqueous solution (10)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 431.8 kJ/mol K 0.22 × 10⁻⁷⁵ pK 75.65: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	431.8	–	–
per 1 mol of Thiocyanic acid	–	215.9	–	–
per 1 mol of Water	–	71.97	–	–
per 1 mol of Sulfur dioxide	–	215.9	–	–
per 1 mol of Ammonium nitrite	–	431.8	–	–
per 1 mol of Methane	–	215.9	–	–
per 1 mol of Hydrogen	–	431.8	–	–

Changes in aqueous solution (11)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 447.0 kJ/mol K 0.49 × 10⁻⁷⁸ pK 78.31: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	447.0	–	–
per 1 mol of Thiocyanic acid	–	223.5	–	–
per 1 mol of Water	–	74.50	–	–
per 1 mol of Sulfur dioxide	–	223.5	–	–
per 1 mol of Ammonium nitrite	–	447.0	–	–
per 1 mol of Methane	–	223.5	–	–
per 1 mol of Hydrogen	–	447.0	–	–

Changes in aqueous solution (12)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 464.6 kJ/mol K 0.40 × 10⁻⁸¹ pK 81.39: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Gas + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	464.6	–	–
per 1 mol of Thiocyanic acid	–	232.3	–	–
per 1 mol of Water	–	77.43	–	–
per 1 mol of Sulfur dioxide	–	232.3	–	–
per 1 mol of Ammonium nitrite	–	464.6	–	–
per 1 mol of Methane	–	232.3	–	–
per 1 mol of Hydrogen	–	464.6	–	–

Changes in aqueous solution (13)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 413.3 kJ/mol K 0.39 × 10⁻⁷² pK 72.41: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	413.3	–	–
per 1 mol of Thiocyanic acid	–	206.7	–	–
per 1 mol of Water	–	68.88	–	–
per 1 mol of Sulfur dioxide	–	206.7	–	–
per 1 mol of Ammonium nitrite	–	413.3	–	–
per 1 mol of Methane	–	206.7	–	–
per 1 mol of Hydrogen	–	413.3	–	–

Changes in aqueous solution (14)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 430.9 kJ/mol K 0.32 × 10⁻⁷⁵ pK 75.49: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Gas + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	430.9	–	–
per 1 mol of Thiocyanic acid	–	215.4	–	–
per 1 mol of Water	–	71.82	–	–
per 1 mol of Sulfur dioxide	–	215.4	–	–
per 1 mol of Ammonium nitrite	–	430.9	–	–
per 1 mol of Methane	–	215.4	–	–
per 1 mol of Hydrogen	–	430.9	–	–

Changes in aqueous solution (15)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 446.0 kJ/mol K 0.73 × 10⁻⁷⁸ pK 78.14: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	446.0	–	–
per 1 mol of Thiocyanic acid	–	223.0	–	–
per 1 mol of Water	–	74.33	–	–
per 1 mol of Sulfur dioxide	–	223.0	–	–
per 1 mol of Ammonium nitrite	–	446.0	–	–
per 1 mol of Methane	–	223.0	–	–
per 1 mol of Hydrogen	–	446.0	–	–

Changes in aqueous solution (16)

Electrolysis of aqueous thiocyanic acid with water as non-redox agent ◆ Δ_rG 463.6 kJ/mol K 0.60 × 10⁻⁸¹ pK 81.22: 2HSCNUn-ionized aqueous solution + 6H₂OLiquid
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2SO₂↑Un-ionized aqueous solution + NH₄NO₂Ionized aqueous solution + 2CH₄↑Un-ionized aqueous solution + H₂↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	463.6	–	–
per 1 mol of Thiocyanic acid	–	231.8	–	–
per 1 mol of Water	–	77.27	–	–
per 1 mol of Sulfur dioxide	–	231.8	–	–
per 1 mol of Ammonium nitrite	–	463.6	–	–
per 1 mol of Methane	–	231.8	–	–
per 1 mol of Hydrogen	–	463.6	–	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
HSCN (ai)	76.44^[1]	92.71^[1]	144.3^[1]	-40.2^[1]
HSCN (ao)	–	97.56^[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]

* (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid, (g):Gas

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
SO₂ (l)	-320.5^[1]	–	–	–
SO₂ (g)	-296.830^[1]	-300.194^[1]	248.22^[1]	39.87^[1]
SO₂ (ao)	-322.980^[1]	-300.676^[1]	161.9^[1]	–
NH₄NO₂ (cr)	-256.5^[1]	–	–	–
NH₄NO₂ (ai)	-237.2^[1]	-111.6^[1]	236.4^[1]	-17.6^[1]
CH₄ (g)	-74.81^[1]	-50.72^[1]	186.264^[1]	35.309^[1]
CH₄ (ao)	-89.04^[1]	-34.33^[1]	83.7^[1]	–
H₂ (g)	0^[1]	0^[1]	130.684^[1]	28.824^[1]
H₂ (ao)	-4.2^[1]	17.6^[1]	577^[1]	–

* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution

References

List of references

1
Janiel J. Reed (1989)
The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list

Δ_rG	423.9 kJ/mol
K	0.54 × 10⁻⁷⁴
pK	74.26

Δ_rG	441.5 kJ/mol
K	0.45 × 10⁻⁷⁷
pK	77.35

Δ_rG	456.7 kJ/mol
K	0.98 × 10⁻⁸⁰
pK	80.01

Δ_rG	474.3 kJ/mol
K	0.81 × 10⁻⁸³
pK	83.09

2HSCN + 6H2O 💧⚡→ 2SO2↑ + NH4NO2 + 2CH4↑ + H2↑

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in aqueous solution (1)

Changes in aqueous solution (2)

Changes in aqueous solution (3)

Changes in aqueous solution (4)

Changes in aqueous solution (5)

Changes in aqueous solution (6)

Changes in aqueous solution (7)

Changes in aqueous solution (8)

Changes in aqueous solution (9)

Changes in aqueous solution (10)

Changes in aqueous solution (11)

Changes in aqueous solution (12)

Changes in aqueous solution (13)

Changes in aqueous solution (14)

Changes in aqueous solution (15)

Changes in aqueous solution (16)

Thermodynamic data of reactants

Thermodynamic data of products

References

List of references

Related reactions

Reactions with same reactants

Related categories

Type of reaction

General equation

Reactant

Product

2HSCN + 6H₂O 💧⚡→ 2SO₂↑ + NH₄NO₂ + 2CH₄↑ + H₂↑