Hi chemistry studs!
Per. 1, we will be re-doing the lab on monday, instructions to follow in class on monday. For now, you should be reviewing and working limiting reagent problems. Please be ready to begin lab ASAP because I am going to try to do something else that day as well.
Per. 2 and 5, if you did not get a positive mass for grams of oxygen, please use the following data to calculate the mole ratio of Mg:O.
Mass of equipment (no Mg) = 29.809
Mass of equipment + Mg = 29.935
Mass of equipment + magnesium oxide = 29.990
These are not necessary correct results, they are simply sample data from another student's lab. The correct empirical formula is MgO (ionic bonding rules: O is -2 and Mg is +2 so they go together in a 1:1 ratio).
Use this data if you didn't get data that makes sense i.e. the magnesium oxide weighed less than the magnesium.
We will have a post lab on monday and start on chapter 7.
Hope your weekend is going well,
Ms. Marostica
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So do you want us to do the whole lab write up this weekend because on the website it says the magnesium oxide lad is due the 30, so i'm a little confused on when you want the lab done.
Do we need to include the set up of the ring stand/burner in our method?
What if we get a ratio that does not have integers? For example 3.5 to 2.
If you get 3.5 : 2, double the ratio to get whole numbers. 7:4
If your word processing program has equation writer, you will find it in "insert"--> object. In the new version, pull up the insert tab and select insert equation. (Its towards the right)
whats the name of the metal net thing that we put the crucible on? does anyone know?
I was wondering if anyone knew how to set up and do Mass percents, and if they know a page in the chemistry book for a sample problem Thank you!
Check the index.
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