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ANSWERS: 5
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Assuming the pressure remains the same, the temperature would have to increase to maintain the greater volume. It's Charle's Law. V1/ T1 = V2 / T2 100 mL / 300K = 200 ml / T2 After cross-multiplying to solve for T2, we get 600 K. (source: http://members.aol.com/profchm/charles.html)
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Air expands when the temperature rises, and air is compressed the the temperature drops -
It falls. Compression and expansion of gasses was the basis of the first refrigerators. Still is for the most part...
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Expanded air is more spread out so average kinetic energy of molecules in a given place (temperature) lowers due to less molecules themselves. So, I guess it does drop.
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g'day Impossibility, Thank you for your question. According to PhysLink and a post from Peter Talman at Portsmouth University "The Ideal Gas Law states pV = nRT, where P = The pressure of the gas in Pa, V = Volume of gas in m3, n = Number of moles of gas, R = A constant of about 8.314 and T = Temperature in K. As a gas (like air) expands, the value of V increases and this has the effect of increasing T (The temperature). As the energy needed to increase it's temperature must be supplied from somewhere, the gas takes the energy from the surrounding system giving the effect of cooling. This is a principle used in refrigeration. " I have attached sources for your reference. Regards References Physlink http://www.physlink.com/Education/AskExperts/ae454.cfm
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