This week in science we learned about moles and relative mass. We did many practice problems to understand the concept. Then after about four worksheets, as a class, conducted an experiment to see how mass at the beginning of a lab doesn't effect the outcome.
     
     The one packet that we did in class involved comparing the mass of chicken and quail eggs.  We made a table of the masses for both then created ratios for the masses and the number of eggs for each mass.  We discovered that no matter the difference in mass between the two, the ratio was always the same.  This is because the general mass of one egg is consistent throughout, so as long as you have the same number of eggs, the ratio of the masses will always be the same.  To find the ratio of the eggs, you would take the  (mass of the chicken eggs)/(mass of the quail eggs).  You then reduce your faction and you then have your mass ratio between your two objects.  The ratio of this example turned out to be 16:1.  Later on in the same packet we proceeded to dothe exact same thing with another table, only this one was comparing the mass of oxygen and sulfur and the ratio turned out to be 1:2.

     Also during this week we learned about moles.  A mole is the amount of pure substance containing the same number of chemical units as there are atoms in exactly 12.00 g of 12^C.  We also learned that one entire mole is 6.022 x 10^23.  This number is used in formulas when trying to figure out how much of a mole something is.  While learning about moles we also learned how to create relative size equations.  What you would do is take a whole mole, or 6.022 x 10^23 and divid that by whatever number you have, for example 36 x 10^22.  When you would divid this you would find the answer to be 1.67, which is then your relative size. Some more examples of these problems are on this worksheet shown.  

     We did more examples involving moles on another worksheet.  On this worksheet we used moles and mass to figure out how many atoms are in something.  In our example we looked at a copper pipe in clas, which had a mass of 151.5g total and its weight of copper was 126.4gCu.  You then take the mass of the copper, 126.4gCu and multiply that by 1 MoleCu/63.6gCu then multiply that by 6.022x10^23/1 MoleCu and get 1.120x10^24, which is your answer for how many atoms are in the copper pipe.  We did another problem involving how many moles of something was in a substance. That example is on the worksheet shown here, as well as then one above.

     We also did a lab in class, but I was only there for the first day, which mostly involved taking measurements.