HON CHEMISTRY: Good job using chemical formulas as tools today! So it turns out there are tons of ways that you can use them. Like finding molar mass, moles, and molecules! Did it all sound familiar to you – like we were repeating yesterday’s lecture? Here’s the lecture from Tuesday.
Did we have to do percent error for our moles of chalk lab?
Hope – Not this time, you don’t have an accepted value.
Thank you.
For the quiz do we have to know the common name, the scientific name, and the formula on the research we did with #58
Mrs. skinner if carbon has 12amu and carbon’s molar mass is 12g then does that mean that 1amu is equal to 1g? I don’t understand that. Also I don’t understand really what an amu is?
(Yes, I’m not Ms. Skinner)
What you said is pretty much it. If you look at a periodic table and look at oxygen’s molar mass, after rounding it will be 16, so oxygen’s mass is 16u.
It seems to be (even though it isn’t defined that way) that both a proton and neutron have a mass of 1 amu (but not together), seeing that hydrogen’s molar mass (for its most common isotope) is 1 amu when it consists of only one proton and one electron (which is ignored).
Are there any questions that we need to include for the moles of chalk lab?
What all do we need to include in our “Moles of Chalk” lab?
D we box our answers when we do math problems in our lab notebook?
Wouldn’t different flavors of gum have different amounts of sugar in them?