Q = ΔU + W
Q is the exchanged heat.
ΔU is the total change in the internal energy of a system.
W is the work done by or on the system.
The statement of the First Law is Thermodynamics is: “energy can be converted
from one form to another with the interaction of heat, work and internal
energy, but it cannot be created nor destroyed, under any circumstances”.
Answer: The formula used to solve the problems related to first law of thermodynamics is [tex]\Delta U=Q+W[/tex]
Explanation:
First law of thermodynamics states that the total energy of the system remains conserved. Energy can neither be destroyed, nor be created but it can only be transformed into one form to another.
Its implication is any change in the internal energy will be either due to heat energy or work energy.
Mathematically,
[tex]\Delta U=Q+W[/tex]
where, Q = heat energy
W = work energy
[tex]\Delta U[/tex] = Change in internal energy
Sign convention for these energies:
For Q: Heat absorbed will be positive and heat released will be negative.
For W: Work done by the system is negative and work done on the system is positive.
For [tex]\Delta U[/tex]: When negative, internal energy is decreasing and when positive, internal energy is increasing.
Hence, the formula used to solve the problems related to first law of thermodynamics is [tex]\Delta U=Q+W[/tex]
