Hon Chemistry 10-18-11 Using Chemical Formulas – Moles & Mass

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.

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10 thoughts on “Hon Chemistry 10-18-11 Using Chemical Formulas – Moles & Mass

  1. For the quiz do we have to know the common name, the scientific name, and the formula on the research we did with #58

  2. 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).

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