Answer:
232 J/K
Explanation:
The amount of heat gained by the air = the amount of heat lost by the tea.
q_air = -q_tea
q = -mCΔT
q = -(0.250 kg) (4184 J/kg/ºC) (20.0ºC − 85.0ºC)
q = 68,000 J
The change in entropy is:
dS = dQ/T
Since the room temperature is constant (isothermal):
ΔS = ΔQ/T
Plug in values (remember to use absolute temperature):
ΔS = (68,000 J) / (293 K)
ΔS = 232 J/K
Answer:
Change in specific internal Energy
Explanation:
Given:
- Mass of the gas, m=0.4 lb
- Initial pressure and volume are

- Final pressure and temperature are

- Heat transfer from the gas is 2.1 Btu
Since the process is isotropic we have

So the final volume of the gas is calculated.
Work in any isotropic is given by w

According to the first law of thermodynamics we have

So the Specific Internal Change is given by

So the specific Change in Internal energy is calculated.
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