Answer:
The second experiment (reversible path) does more work
Explanation:
Step 1:
A piston confines 0.200 mol Ne(g) in 1.20L at 25 degree °C
<em>(a) The gas is allowed to expand through an additional 1.20 L against a constant of 1.00atm</em>
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Irreversible path: w =-Pex*ΔV
⇒ with Pex = 1.00 atm
⇒ with ΔV = 1.20 L
W = -(1.00 atm) * 1.20 L
W = -1.20L*atm *101.325 J /1 L*atm = -121.59 J
<em>(b) The gas is allowed to expand reversibly and isothermally to the same final volume.</em>
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W = -nRTln(Vfinal/Vinitial)
⇒ with n = the number of moles = 0.200
⇒ with R = gas constant = 8.3145 J/K*mol
⇒ with T = 298 Kelvin
⇒ with Vfinal/Vinitial = 2.40/1.20 = 2
W = -(0.200mol) * 8.3145 J/K*mol *298K *ln(2.4/1.2)
W = -343.5 J
The second experiment (reversible path) does more work
The answer is it shifts right. This could be explained by Le
Chatelier's principle. It states that that when a system experiences a commotion
(such as absorption, temperature, or heaviness variations), it will answer to reinstate
a new equilibrium state. This just means that if there is an energy added, the
reaction is trying to remove it again by going to the right.
Answer:
The liquid will boil.
Explanation:
Boiling will occur when the vapor pressure is equal to the atmospheric pressure. This is called the boiling point. Without any external pressure the liquid molecules will be able to spread out and change from a liquid to a gas.
Answer:
Explanation:
We have two pressures, two temperatures, and one volume.
This looks like a question in which we can use the Combined Gas Law to calculate the volume.
Data:
Calculation:
