CHEMISTRY COMMUNITY

Ricky Z1D

X should probably never be zero because X is supposed to represent an unknown concentration that is trying to be solved in the equilibrium formula. Check back on pg 142 of the course reader for explanation written by Dr. Lavelle. What you are thinking of is when Kc is really small, defined by Dr. La...

Ricky Z1D

That is exactly what was covered in pgs 138 and 139 of the course reader. Change in concentration, pressure and temperature will change equilibrium. Something can remain at equilibrium if you do nothing to it, but if you start taking out product, then the reactants will be the only things reacting t...

Ricky Z1D

https://drive.google.com/open?id=0Bwbyg2fLGHJ7U3VDUHlPRF82amc Picture of the answer through google drive link. Notice first to balance the equation. Use the ICE box. Notice that you are basically given the initial and equilibrium of BrCl. You can solve for change of BrCl with those two. Remember th...

Ricky Z1D

As you have written out, the problem gave .1 mmol (millimoles). You want to convert moles to concentration which is moles/Liters. Liters is already in the correct units of .5 liters (rather than milliliter). So you have to convert .1 mmol to mols before calculating. So that is .1 mmol * 10 -3 or 1 *...

Ricky Z1D

Those are the electronegativity numbers for the elements, you can a find a periodic table with that information on page 87 of the course reader or page 92 in the textbook.

Ricky Z1D

You should look on page 84 of the course reader.

The key point is: atoms in period 3 or higher have d-orbitals in valence shell that accommodate additional electrons.

You can also look at pg 87 in the textbook, 3.10 expanded valence shell section.

Ricky Z1D

CH. 3 49 A.pdf: (32.11 KiB) Downloaded 112 times

Ricky Z1D

Pretty sure the recent email should reflect the changes. We did skip molecular orbital theory, so that's probably why we will finish chemical equilibiurm this week and will have the test earlier since test 2 will cover up to chemical equilibrium.

Ricky Z1D

Here is an image of a full credit answer for you to double check your work.

https://drive.google.com/open?id=0Bwbyg2fLGHJ7ZFByeFFHV3lFUjQ

Ricky Z1D

This should be the answer.

Heisenberg's uncertainty principle is meant for small objects like electrons, not 2150 kg cars. This calculation will not help in determining error of the radar.

https://drive.google.com/open?id=0Bwbyg2fLGHJ7UnlQUFgyZkQ2czA

Ricky Z1D

You were given volume of 250ml and Molarity of .20 mol/L. Use the Molarity equation where Moles/Volume= Molarity and solve for Moles. Which is Moles= Molarity X Volume Plug in the numbers: Moles= .20mol/L X .25L (250ml X 10 -3 ) =5 X 10 -2 mol Convert moles to Grams using molar mass of CuSO4 5H20 wh...

Ricky Z1D

Exam 1 actually cover material from fundamentals to ch.2. The page numbers are correct though, pages 18-36 is fundamentals and 37-74 is ch.1-2.

Ricky Z1D

I think the only way to counter messiness is to write small and to keep steps organized in a pattern. I started from the top left of the question and wrote the steps below each other until I ran out of space and then I moved towards the right of the page. I think another way to counter messiness is ...

Ricky Z1D

This was one of the problems done during the Wednesday review session. The answer was 1.66 x 10^-17 J. The numbers you multiplied by were exactly what we used, so may be we just rounded it differently.

Ricky Z1D

Chemical bonds will not be on the exam. Ch. 2 is electron configuration and atomic orbitals.

Ricky Z1D

Will we have to remember the mass of an electron, 9.11 x 10^-31 kg, or will this information be given on the test?

Ricky Z1D

Check out the video on Wave Properties of Electrons and The De Broglie Equation Video Module. At 2 minutes 37 seconds of the video, Dr. Lavelle explains the two interferences with better visual representation than during Friday's class.

Ricky Z1D

According to what Dr. Lavelle said in class on friday, the cut off is anything after 10^-14 or 10^-16.

Ricky Z1D

In an actual lab, we would be able to find out actual yield by measuring the final product and compare it to the theoretical yield. However, since we are not doing a lab for every problem, the book and Dr. Lavelle should be giving out the actual yields.

Ricky Z1D

Source: http://www.chemistryjokes.com/jokes/wha ... -attitude/

CHEMISTRY COMMUNITY

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