Moles YesterDay

Haha, get it? Because mole day was yesterday! Ok, you can shoot me in the head now for making such a lame joke. According to this post (Adventures in Ethic and Science), that was yesterday. To commemorate it… It is the subject of today’s…

Pop Quizz!

This is the 6th edition of *drum rolls* Pop Quizz! A quizz in which the answers are not obvious and if it is obvious, and you get it wrong, you are rebuked at!!!

Occasionally, I will occasionally ask a question, and the reader will answer them! For every wrong answer, I will consider one of your comments a spam. Ha! See how you like that suckers! (I am kidding, of course) Sometimes, a wrong answer won’t invite rage, some really obvious one will, and you will be called an idiot if you can’t answer the obvious one. In fact, I may have to make an extra page on my blog for the lists of idiots. 🙂

So, the question of the day is… How much is a mole? And for extra credit, what is the unit based on?

 

 

 

 

 

 

 

hint: It is kind of like a dozen, but except much larger, and it is used to count how many atoms or molecules there are in certain amounts of mass.

 

 

And the answer is…

 

 

*drum rolls*

 

*dying of anticipation*

 

 

*heart attack*

 

…and the answer is… 6.022×10^23!!! It is also called Avogadro’s number. Now, that is a huge number. It is like this: 602,200,000,000,000,000,000,000, which is 6 followed by 26 digits. Now, they are not all zeroes, but I am not going to bother filling it in, since  6022 is enough. Anyways, it is used in chemistry because there are just way too much atoms, you know, them being so small and all. The numbers are bsed on the number of C12 atoms in 12 grams. With that, you can use the atomic mass of other atoms to find out the amount of moles in certain amount of mass. For example, H1’s atomic mass unit is 1, so 1gram of hydrogen contains 1 mole of atoms. O16’s amu is 16, so 16 grams of oxygen contains 1 mole of atoms. Water is H2O, so if you add the amus of those elements together, you get an amu of 18 grams. You need 18 grams of water to get 1 mole of it. Now, you could have 1 mole of eggs, but that is way to impractical, and that amount of eggs does not exist.

Now, there is a special way you can find the amount of moles in gas. In room temperature and pressure, it will occupy 22.4 liters. Or, you could use the ideal gas law:

PV=nRT

P is pressure, V is volume, n is the amount of moles, R is the gas constant, which is 8.314 when kilopascal is used for pressure, and 0.082 when the atm, or the pressure of one atmosphere of Earth, is used, and finally, T is temperature in kelvin, which starts from 0, and 0 degrees celsius is 273.15 degrees Kelvin. You plug in the numbers, and you can find how much volume there is in certain number of moles at certain pressures. Isn’t that cool! Of course, this equation has its limitations, including the fact that as the temperature of the gas gets closer to condensation temperature, it deviates from the ideal behavior as told by the equation.

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