2. Calculate the enthalpy change for the reaction : C4H4 (9) + H2 (9) - C2H6 (g) Given the following data: i) C2H4 (9) + 3 O2 (g) → 2 CO2 (9) + 2 H20 (1) AH° = - 1410.9 kJ AH° = - 3119.4 kJ ii) 2 C2H6 (9) + 7 02 (9) - 4 CO2 (9) + 6 H20 (1) iii) 2 H2 (9) + O2 (9) 2 H20 (1) AH° = - 571.6 kJ 3. Calculate the standard enthalpy change for the reaction, C2H2 + 2 H2 (9) C2H6 (9) (9) Given that: i) 2 C2H2 (9) + 5 O2 (9)4 CO2 (9) + 2 H2O (1) ii) 2 C2H6 (9) + 7 02 (9)4 CO2 (9) + 6 H20 (1) iii) 2 H2 (g) + O2 (g) → AH° = - 2599 kJ AH° = - 3119 kJ AH° = - 572 kJ 2 H20 (1) The enthalpy of combustion of methane is -891 kJmol-1. Calculate the enthalpy of formation of methane if the enthalpy of formation of carbon dioxide and water are - 394 kJmol1 and -286 kJmol respectively. Chemical equation for formation of 4. methane: C(s) + 2H2(9) → CH4(9) Given: CH4(9) + 202(9) C(s) + O2(9) → CO2(9) H2(9) + 2 O2 H20 AH = -891 kJmol1 AH = -394 kJmol1 AH = -286 kJmol1 2H201) + CO2(9)
2. Calculate the enthalpy change for the reaction : C4H4 (9) + H2 (9) - C2H6 (g) Given the following data: i) C2H4 (9) + 3 O2 (g) → 2 CO2 (9) + 2 H20 (1) AH° = - 1410.9 kJ AH° = - 3119.4 kJ ii) 2 C2H6 (9) + 7 02 (9) - 4 CO2 (9) + 6 H20 (1) iii) 2 H2 (9) + O2 (9) 2 H20 (1) AH° = - 571.6 kJ 3. Calculate the standard enthalpy change for the reaction, C2H2 + 2 H2 (9) C2H6 (9) (9) Given that: i) 2 C2H2 (9) + 5 O2 (9)4 CO2 (9) + 2 H2O (1) ii) 2 C2H6 (9) + 7 02 (9)4 CO2 (9) + 6 H20 (1) iii) 2 H2 (g) + O2 (g) → AH° = - 2599 kJ AH° = - 3119 kJ AH° = - 572 kJ 2 H20 (1) The enthalpy of combustion of methane is -891 kJmol-1. Calculate the enthalpy of formation of methane if the enthalpy of formation of carbon dioxide and water are - 394 kJmol1 and -286 kJmol respectively. Chemical equation for formation of 4. methane: C(s) + 2H2(9) → CH4(9) Given: CH4(9) + 202(9) C(s) + O2(9) → CO2(9) H2(9) + 2 O2 H20 AH = -891 kJmol1 AH = -394 kJmol1 AH = -286 kJmol1 2H201) + CO2(9)
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Chapter1: Chemical Foundations
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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
Transcribed Image Text:2.
Calculate the enthalpy change for the reaction :
C4H4 (9) + H2 (9)
C2H6 (g)
Given the following data:
i)
C2H4 (9) + 3 O2 (9) → 2 CO2 (9) + 2 H2O (1)
AH° = - 1410.9 kJ
2 C2H6 (9) + 7 02 (9) →4 CO2 (9) + 6 H20 (1)
ii)
iii) 2 H2 (9) + O2 (g) 2 H2O (1)
AH° = - 3119.4 kJ
AH° = - 571.6 kJ
3.
Calculate the standard enthalpy change for the reaction,
C2H2 (g) + 2 H2 (9g) -
C2H6 (9)
Given that:
i)
2 C2H2 (9) + 5 02 (g) 4 CO2 (9) + 2 H2O (1)
AH° = - 2599 kJ
3119 kJ
ii)
2 C2H6 (9) + 7 02 (9) - 4 CO2 (9) + 6 H20 (1)
AH° =
iii) 2 H2 (9) + O2 (9) → 2 H2O ()
AH° = - 572 kJ
The enthalpy of combustion of methane is -891 kJmol-1. Calculate the enthalpy of
formation of methane if the enthalpy of formation of carbon dioxide and water are -
394 kJmol-1 and -286 kJmol respectively. Chemical equation for formation of
4.
methane:
C(s) + 2H2(9)
CH4(9)
Given:
AH = -891 kJmol-1
CH4(9) + 202(9) 2H2O() + CO2(g)
C(s) + Oz(g) → CO2(9)
H2(g) + 2 O2 - H20
AH = -394 kJmol-1
AH = -286 kJmol-1
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