5. Use standard heats of formation and the following equation to determine the enthalpy of formation of C₂H()ΔΗ, = -3127 kJ2C₂H6(g) +70₂(g) ⇒ 4CO2(g) + 6H₂O) Selected Standard Molar Enthalpies of FormationAH₁AH;AH₁Substance (kJ/mol) Substance (kJ/mol) Substance (kJ/mol)Al₂O3(s)-1675.7 HBr(g)CaCO3(s)-1207,6 HCl(g)CaCl₂(s)Ca(OH)₂(s)CCL₂(E)CCL4(8)CHCI ()CH₂(g)C₂H₂(g)C₂H₁(g)C₂H₂(g)CzHs(g)CH()CH₂OH(E)C₂H₂OH()CO(g)CO₂(g)COCI₂(g)+49.1 Fe₂O₂(8)-239.2 Fe,O4(s)-277.6 FeCl₂(s)CH3COOH(E) –484.3 FeCls(s)-110.5 FeS (8)CS₂(e)CS₂(g)CrCla(g)Cu(NO₂)₂ (8)-795.4 HF(g)-985.2 HCN(g).-128.2 H₂O(E)-95.7 H₂O(g)CuO(s)CuCl(s)CuCl₂(s)-134.1 H₂O₂(e)-74.6 HNO (0)+227.4 H₂PO4(s)+52.4 H₂S(g)-84.0 H₂SO4(e)-103.8 FeO(s)–36.3|NH(8)-92.3 N₂H4(e)-273.3 NH Cl(s)+135.1 NH₂NO(s)-285.8 NO(g)-393.5 PbCl₂(s)-219.1 MgCl₂(s)+89.0 MgO(s)+116.7 Mg(OH)2(s)-556.5 HgS(s)-241.8 NO₂(g)-187.8 N₂O(g)-174.1 N₂O(g)1284.4 PH,(g)-20.6 PCl₂(g)814.0 P,O,(s)-272.0 P4O₁0(s)-824.2 KBr(s)-1118.4 KCl(s)-341.8 KCIO,(s)-399.5 KOH(s)-178.2 AgaCO₂ (s)-359.4 AgCl(s)-641.3 AgNO,(s)-601.6 Ag S(s)-924.5 SFB(g)-58.2 SO₂(g)-302.9 NaCl(s)-411.2 SO₂(g)-157.3 NaOH(s)-425.6 SnCl₂(s)-137.2 Na₂CO3(s)-1130.7 SnCl4(e)-220.1-45.9+50.6-314.4-365.6+91.3+33.2+81.6+11.1+5.4-287.0-2144.3-2984.0-393.8-436.5-397.7-424.6-505.8-127.0-124.4-32.6-1220.5-296.8-395.7-325.1-511.3Note: The enthalpy of formation of an element in its standard state isdefined as zero.

Answered: Image /qna-images/answer/f00fcc02-b260-4fa9-9bba-aec1c2a31cd6.jpg

Answered: 5. Use standard heats of formation and…

5. Use standard heats of formation and the following equation to determine the enthalpy of formation of C₂H() ΔΗ, = -3127 kJ 2C₂H6(g) +70₂(g) ⇒ 4CO2(g) + 6H₂O)

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

5. Use standard heats of formation and the following equation to determine the enthalpy of formation of C₂H()
ΔΗ, = -3127 kJ
2C₂H6(g) +70₂(g) ⇒ 4CO2(g) + 6H₂O)

Selected Standard Molar Enthalpies of Formation
AH₁
AH;
AH₁
Substance (kJ/mol) Substance (kJ/mol) Substance (kJ/mol)
Al₂O3(s)
-1675.7 HBr(g)
CaCO3(s)
-1207,6 HCl(g)
CaCl₂(s)
Ca(OH)₂(s)
CCL₂(E)
CCL4(8)
CHCI ()
CH₂(g)
C₂H₂(g)
C₂H₁(g)
C₂H₂(g)
CzHs(g)
CH()
CH₂OH(E)
C₂H₂OH()
CO(g)
CO₂(g)
COCI₂(g)
+49.1 Fe₂O₂(8)
-239.2 Fe,O4(s)
-277.6 FeCl₂(s)
CH3COOH(E) –484.3 FeCls(s)
-110.5 FeS (8)
CS₂(e)
CS₂(g)
CrCla(g)
Cu(NO₂)₂ (8)
-795.4 HF(g)
-985.2 HCN(g).
-128.2 H₂O(E)
-95.7 H₂O(g)
CuO(s)
CuCl(s)
CuCl₂(s)
-134.1 H₂O₂(e)
-74.6 HNO (0)
+227.4 H₂PO4(s)
+52.4 H₂S(g)
-84.0 H₂SO4(e)
-103.8 FeO(s)
–36.3|NH(8)
-92.3 N₂H4(e)
-273.3 NH Cl(s)
+135.1 NH₂NO(s)
-285.8 NO(g)
-393.5 PbCl₂(s)
-219.1 MgCl₂(s)
+89.0 MgO(s)
+116.7 Mg(OH)2(s)
-556.5 HgS(s)
-241.8 NO₂(g)
-187.8 N₂O(g)
-174.1 N₂O(g)
1284.4 PH,(g)
-20.6 PCl₂(g)
814.0 P,O,(s)
-272.0 P4O₁0(s)
-824.2 KBr(s)
-1118.4 KCl(s)
-341.8 KCIO,(s)
-399.5 KOH(s)
-178.2 AgaCO₂ (s)
-359.4 AgCl(s)
-641.3 AgNO,(s)
-601.6 Ag S(s)
-924.5 SFB(g)
-58.2 SO₂(g)
-302.9 NaCl(s)
-411.2 SO₂(g)
-157.3 NaOH(s)
-425.6 SnCl₂(s)
-137.2 Na₂CO3(s)-1130.7 SnCl4(e)
-220.1
-45.9
+50.6
-314.4
-365.6
+91.3
+33.2
+81.6
+11.1
+5.4
-287.0
-2144.3
-2984.0
-393.8
-436.5
-397.7
-424.6
-505.8
-127.0
-124.4
-32.6
-1220.5
-296.8
-395.7
-325.1
-511.3
Note: The enthalpy of formation of an element in its standard state is
defined as zero.

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