Answer :
Answer:
Q = - 730 KJ
730 KJ is transferred out of the system
Explanation:
According to the first law of thermodynamics, energy can neither be created nor destroyed, but can be transformed from one form to another.
For a particular process/system, the first law is interpreted as
ΔU = Q + W (depending on convention, some textbooks give this relation as ΔU = Q - W)
ΔU is the change in internal energy of the system, in my convention, it is positive if the internal energy increases and negative otherwise.
Q = Heat transferred into or out of the system. Q is positive for heat transferred into the system and negative for heat transferred out of the system.
W = workdone by the system or work done on the system. W is positive for workdone on the system and W is negative for when work is done by the system.
ΔU decreases by 250 KJ, that is, ΔU = - 250 KJ
Q = ?
W = 480 KJ (Work is done on the system)
- 250 = Q + 480
Q = - 250 - 480 = - 730 KJ
The heat is transferred out of the system.
The amount of heat Q is transferred in this process is -730 kJ, which means the heat is transferred into the surroundings.
Given to us,
Decrement in the energy of the system, ΔU = 250 kJ,
work done on the system, W = 480 kJ,
As we know according to the first law of thermodynamics,
energy can neither be created nor be destroyed but can be transformed from one form to another. Further, the first law is given as,
ΔU = Q - W,
where,
ΔU = change in internal energy of the system,
{Positive if the internal energy increases and negative if the internal energy decreases}
Q = Heat transferred,
{Positive for heat transferred into the system and negative for heat transferred out of the system}
W = work done by the system or work done on the system,
{Negative for work done on the system and Positive when work is done by the system}
Now,
the energy of the system decreases by 250 kJ, so
ΔU = -250 kJ,
And, work is done on the system, so
W = - 480 KJ.
Substituting the value,
[tex]\Delta U = Q-W\\-250 = Q -(-480)\\-250 = Q+480\\-250-480 = Q\\Q = - 730\ \rm kJ[/tex]
Hence, the amount of heat Q is transferred in this process is -730 kJ, which means the heat is transferred into the surroundings.
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