Assume the work done compressing the He gas is -63 kJ and the internal energy change of the gas is 79 kJ. What is the heat loss
1 answer:
Answer:
Heat gain of 142 kJ
Explanation:
We can see that job done by compressing the He gas is negative, it means that the sign convention we are going to use is negative for all the work done by the gas and positive for all the job done to the gas. With that being said, the first law of thermodynamics equation will help us to solve this problem.
Δ ⇒
Δ
Therefore, the gas gained heat by an amount of 142 kJ.
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Answer:
q=1910.71 W/m²
T=383.07 K
Explanation:
Given that
L₁=0.25 m ,K₁=1.13 W/(m.K)
L₂=0.2 m , K₂=1.45 W/(m.K)
L₃= 0.1 m , K₃=0.66 W/(m.K)
h₁=115 W/(m².K)
h₂=23 W/(m².K)
The total thermal resistance
Now by putting the values
Put A= 1 m² ( To find heat transfer per unit area)
R= 0.56 K/W
We know that
q= ΔT/R
Here ΔT = 1370 - 300 K =1070 K
Now by putting the values
q= 1070/0.56
q=1910.71 W/m²
Lets T is the outside surface temperature
q = h₂ ( T- 300)
Now by putting the values
1910.71 = 23 ( T- 300)
T=383.07 K
Answer:
work will be positive when it is under polytropic expansion process
Explanation:
It states a polytropic process with n equal to 1.67. there is a polytropic expansion that mean work is positive and if it was polytropic compression then it would be negative
Also work during the process of polytropic is given as
the work will be positive when it is under the polytropic expansion process