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Answer:
T=151 K, U=-1.848*10^6J
Explanation:
The given process occurs when the pressure is constant. Given gas follows the Ideal Gas Law:
pV=nRT
For the given scenario, we operate with the amount of the gas- n- calculated in moles. To find n, we use molar mass: M=102 g/mol.
Using the given mass m, molar mass M, we can get the following equation:
pV=mRT/M
To calculate change in the internal energy, we need to know initial and final temperatures. We can calculate both temperatures as:
T=pVM/(Rm); so initial T=302.61K and final T=151.289K
Now we can calculate change of U:
U=3/2 mRT/M using T- difference in temperatures
U=-1.848*10^6 J
Note, that the energy was taken away from the system.
Answer:
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Explanation:
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Answer:
The resistance is 24.9 Ω
Explanation:
The resistivity is equal to:

The area is:
A = 60 * 60 = 3600 um² = 0.36x10⁻⁴cm²

If NA is greater, then, the term 1/NA can be neglected, thus the equation:

Where
V = 0.44 V
E = 11.68*8.85x10¹⁴ f/cm


The length is:
L = 10 - 0.335 = 9.665 um
The resistance is:

The work done during the process is 359 btu
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<u>Explanation:</u>
Given-
P1 = 15psia
P2 = 140 psia
V1 = 7ft³
a = 5 psia/ft³
b = C
P = aV +b
Work done, W = ?
P1 = aV1 + b
15 = 5 (7) + b
b = -20 psia
P2 = aV2 + b
140 = 5 ( V2) - 20
V2 = 32 ft³
The work done by the process is the area under the curve which is trapezoidal.
Therefore,
Work done, W = area of trapezoid
= (P2 + P1 / 2) (V2 - V1)
= ( 140 + 15 / 2 ) ( 32 - 7)
= 1937.5 psia ft³
= 1937.5/ 5.4039 = 359 btu
Therefore, the work done during the process is 359 btu