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Solnce55 [7]
3 years ago
10

True or false nothing is smaller than atom

Chemistry
1 answer:
Papessa [141]3 years ago
3 0
False. there are quarks, gluons, electrons and nuetrions.
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Which of the following statements explain why the van der Waals equation must be used to describe real gases? X. interactions be
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Answer:

Statements Y and Z.

Explanation:

The Van der Waals equation is the next one:

nRT = (P + \frac{an^{2}}{V^{2}})(V -nb) (1)

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nRT = PV (2)

<em>where n: is the moles of the gas, R: is the gas constant, T: is the temperature, P: is the measured pressure, V: is the volume of the container, and a and b: are measured constants for a specific gas.  </em>

As we can see from equation (1), the Van der Waals equation introduces two terms that correct the P and the V of the ideal gas equation (2),<u> by the incorporation of the intermolecular interaction between the gases and the gases volume</u>. The term an²/V² corrects the P of the ideal gas equation since the measured pressure is decreased by the attraction forces between the gases. The term nb corrects the V of the ideal gas equation, <u>taking into account the volume occuppied by the gas in the total volume, which implies</u> a reduction of the total space available for the gas molecules.          

So, the correct statements are the Y and Z: the non-zero volumes of the gas particles effectively decrease the amount of "empty space" between them and the molecular attractions between gas particles decrease the pressure exerted by the gas.            

Have a nice day!

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