Answer: The order from the Most energy released to most Energy Absorbed Is given as 2---> 4--->,3-->---> 1
B)-61.9 kJ
Explanation:
The change in the internal energy of a system is positive if the reaction absorbs energy and negative if the reaction releases energy. For a system to cause an increase in volume, it must have very high energy built up to be released.
1. Surroundings get colder and the system decreases in volume. Here, the surrounding absorbs energy resulting in positive ΔE
2. Surroundings get hotter and the system expands in volume. Here energy is released causing the system to be negative
3. Surroundings get hotter and the system decreases in volume. Although there is a decreased volume, the system is negative because it releases energy
4. Surroundings get hotter and the system does not change in volume. System is negative because it releases energy even thgoygh there is no change in volume
Therefore the order from the Most energy released to most Energy Absorbed Is given as 2---> 4--->,3-->---> 1
b) Using
ΔE = q+ w from 1st law of thermodynamics
ΔE= ΔH - P ΔV
gIven
ΔH = -75.0KJ
volume= A change from 5.0L TO 2.0L = Final volume - initial volume = 2-5= -3.00L
P= 43.0atm
ΔE= ΔH - P ΔV
P ΔV = 43 atm x -3 = -129L.atm
We first convert L-atm to Joules.
1 L-atm = 101.325 Joules.
129L.atm = 129 x 101.325 = - 13071 J
to KJ becomes
13071/1000 = - 13.071KJ
Recall ΔE= ΔH - P ΔV and putting values
ΔE = -75.0 - (-13.071 KJ)= -75.0 kJ + 13.071 kJ = -61.9 kJ
- Ideal gas constant, in kilopascal-cubic meters per kilomole-Kelvin.
- Temperature, in Kelvin
- Pressure, in kilopascals