Which phase change results in an increase in entropy?
2 answers:
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Answer:
The volume in the first tank = 0.32
The volume in the second tank = 2.066
The final pressure of the mixture = 203.64 K pa
Explanation:
<u>First Tank </u>
Mass = 2 kg
Pressure = 550 k pa
Temperature = 25 °c = 298 K
Gas constant for nitrogen = 0.297
From the ideal gas equation
P V = m R T
550 × V = 2 × 0.297 × 298
V = 0.32
This is the volume in the first tank.
<u>Second tank</u>
Mass = 4 kg
Pressure = 150 K pa
Temperature = 25 °c = 298 K
Gas constant for oxygen = 0.26
From the ideal gas equation
P V = m R T
150 × V = 4 × 0.26 × 298
V = 2.066
This is the volume in the second tank.
This is the iso thermal mixing. i.e.
----- (1)
Put this value in equation (1)
× 2.386 = 550 × 0.32 + 150 × 2.066
= 203.64 K pa
Therefore the final pressure of the mixture = 203.64 K pa
Hello!
The pressure of the gas when it's temperature reaches 928 °C is 3823,36 kPa
To solve that we need to apply Gay-Lussac's Law. It states that the pressure of a gas when the volume is left constant (like in the case of a sealed container like an aerosol can) is proportional to temperature. This is the relationship derived from this law that we use to solve this problem:
Have a nice day!
The pressure of the gas when it's temperature reaches 928 °C is 3823,36 kPa
To solve that we need to apply Gay-Lussac's Law. It states that the pressure of a gas when the volume is left constant (like in the case of a sealed container like an aerosol can) is proportional to temperature. This is the relationship derived from this law that we use to solve this problem:
Have a nice day!