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42) The van der Waals equation has an adjustment for Pressure and one for volume , these adjustments account for real gases having what? A) (I) Real gas molecules e...

Question

42) The van der Waals equation has an adjustment for Pressure and one for volume , these adjustments account for real gases having what? A) (I) Real gas molecules exert ionic forces on each other: (2) Gas molecules have volume. B) (1) Real gas molecules exert ionic forces 0n each other: (2) Gas molecules have energy C) (I) Real g4s_ molecules exert forces cach other. Gas molecules have volume . D) None of the above have BOTH of the two factors accurately stated E) ( 1) Real gas molecules exert f

42) The van der Waals equation has an adjustment for Pressure and one for volume , these adjustments account for real gases having what? A) (I) Real gas molecules exert ionic forces on each other: (2) Gas molecules have volume. B) (1) Real gas molecules exert ionic forces 0n each other: (2) Gas molecules have energy C) (I) Real g4s_ molecules exert forces cach other. Gas molecules have volume . D) None of the above have BOTH of the two factors accurately stated E) ( 1) Real gas molecules exert forces On cach other. (2) Gas molecules have enetgy. 43) Potential energy is energy available by virtue of an object's horizontal position_ B) the energy associated with the motion of atoms and molecules_ solar energy: ie energy that comes from the sun . D) the energy stored within the structural units of chemical substances.



Answers

At high gas densities, the van der Waals equation modifies the ideal-gas law to account for nonzero molecular volume and for the van der Waals force that we discussed in Section 17.1 . The van der Waals equation is $\left(p+\frac{n^{2} a}{v^{2}}\right)(v-n b)=n R T$ where $a$ and $b$ are constants that depend on the particular gas. For nitrogen $\left(\mathrm{N}_{2}\right), a=0.14 \mathrm{~Pa} \cdot \mathrm{m}^{6} / \mathrm{mol}^{2}$ and $b=3.91 \times 10^{-5} \mathrm{~m}^{3} / \mathrm{mol} .$ For $1.000 \mathrm{~mol}$ of $\mathrm{N}_{2}$ at 10.00 atm pressure, confined to a volume of $2.000 \mathrm{~L},$ find the temperatures predicted (a) by the ideal-gas law and (b) by the van der Waals equation.

Yeah, Problem number five. In this problem, we will use to equations I didn't gas equation and abandoned rails Equations which are given as PV equals and are t And the second equation is P plus a and squared over V squared. Multiply the minus and be equal and are see we will plug in the known values to obtain the pressures and compare their material deviation for put your number eight in the audience Gasp! We can simply insert the given values in is equal to one more and T is equal to 27 three husband and three is equal to 4.48 month nine 10 Power Negative fool Meter Cube. After we express the pressure, as P is equal to in you are t over v. So it will equal to one multiplying 8.3145 Yeah. Multiply 273 over 4.48 Multiply 10 car Negative four. So we will get the pressure is equal to 5.7. Multiply it important Port Temple six The scan And for the second question, P in the case off Wonder Wells equation, we need parameters for the c 02 gas, and these are given as a is equal to all points. 364 and P is equal to 4.27 Multiply Temple Negative five. Let's now solve the equation for P so P B T W plus study. It's credit. Rewrite it. We the thank you less Okay, a. And it's good over with. Good multiply B minus and be equal and are t and then get the beaten one side. So VP v d w equal to and all t over the minus and be minus a and it's good over. These could yeah, and then p will equal to after plugged the values 8.3145 Yeah. Multiply 273 over 4.48 Multiply 10 power Negative fool minus 4.27 Multiply temp. Our negative five No, it could minus 4.3 64 over 4.48 Multiply 10 power Negative rate noted. That's the end is equal one. So we will get that the pressure is equal to but three points 79 Might deploy 10 power no top temperature six plus again, which is different from the ideal gas equation. We will get that this difference from this equation 100 minus p from the V. D W equation overpay off the ideal gas. Multiply 100 equal to 100 minus three points. 79 open 5.7 multiply 100 equal to 25.3 100%. Thank you.

Okay, this problem was a little bit interesting for me because I never ever used the Vander wal's stuff. Let me get down here. Lost my problem. So we are given the following information, It turns out that the Vanderbilts constant be Equals four times the total volume actually occupied by the molecules of a mole of gas. Using that number, we're going to calculate the fraction of volume from here. Yeah, actually occupied by argon atoms at And then we've got two conditions are first condition is at STP and then I'll do the second condition we get there. Well, one nice thing when we're figuring this out at sdP one mole of any gas including our gun Occupies a volume of 22.4 L. When we look up B. In the table in our textbook, we found we find that B is equal to where did I write this down? .03- two. And again that's leaders per mall. That's how many leaders remote. And this is also leaders promote. So we're told that this Factor of four times the total volume Is what it's actually going to occupy. So we're going to take 0.03-2 whoops divided by four And that equals 03,- 8.05 times 10 to the -3. And that'll be little is primal. And now to find our fraction we're simply going to take 8.05 Times 10 to the -3 Leaders from all divided by 20 to 4 leaders Permal. And I got for this one 3.59 times 10 to the -4. Now this one did have the answer in the back of the book. And they reported I'm going to right here. Book reported a percentage. So to do percentage we'd have to multiply this number times 100. So we get 359 Times 10 to the -2%. And I'm gonna put like a dotted circle around this because it did very specifically say find the fraction this is the fraction. This is not a fraction, that's 1%. Our second problem asks us to do the same thing but this time we're going to not be at STP we are going to be at 20 0.27 mega pascal's And 0°C. So now we're going to use the ideal gas law to solve for V. And we're gonna have one mall because that's what we're dealing with. Our pressure is Excuse me, are is 831, There's my units and at 0°C. Is that Calvin divided by 20.27 and of course I'll go times 10 to the third killer pascal's Solving for v. On this one. I got 0.1120 and that will be leaders per mole because that was per one mall. We'll do the same thing now 85 times 10 to the minus third. Leaders per mole Divided by 0.1120 leaders Permal. And for this I got 7.19 Times 10 to the -2. And this is the fraction. Again, your book book reported a percent, Which would be simply this number times 100, Was at 7.19 times 10 to the -2. Yeah, it was 7.19 percent. And again, I'll put this around here. That's the answer in the book, but that's not really what they asked you for.

Okay, So if you recall, um, in the kinetic military, Very, we say that our Internet miracle forces are Manjula Legler with people but by our Vander Wal's forces between I think, ah, the forces increases with increasing molecular mass. So the gas with the highest Milica amassed is most likely to depart from the law. So six has the highest Morty Will Matt. It is most likely to depart from the kinetic energy or kinetic theory, huh?

Yeah, yeah. We have born energy e equals three over to Katie. So temperature comes out to be two e over three K. Yeah. Now, two times three cake was 1.38 times 10 to the minus 23 e. For part A using e equals 7.9 times 10 to the minus four. Evie, or times 1.6 times tend to the native 19 jewels. We find the temporary were 6.1 kelvin for part B e equals full part for a TV 4.4 a TV times. This gives us temperature equals 34 600. Catherine? Yeah. Uh huh. Now, in the first case for hydrogen. So this is temperature off hydrogen on This is temperature off his iam. So temperature off hydrogen is much, much less than 300 Calvin. Which means that the hydrogen bond will dissociate at room temperature in Yeah. Shit. Hey, Liam. So this was associate at room temperature at this will not. This is hydrogen, and this is not dissociated. This is not dissociated.


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