Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
7 Cards in this Set
- Front
- Back
- 3rd side (hint)
|
Atomic Mass of an Element + Isotopes |
(%)(mass of Isotope 1) + (%)(mass of Isotope 2)... = Atomic Mass of Element |
(0.9889)(12u) + (0.0111)(13.0034u) = 12.01u |
|
|
Mass of Atoms using Moles |
(# Atoms)(#amu) = (Units of Atoms)(1g/6.022x10^23) = Mass in grams of Atoms |
(6 atoms)(243amu) = (1.46x10^3 u)(1g/6.022x10^23) = 2.42 x 10^-21g |
|
|
Determining Moles of Atoms |
(g of Element)(1 mol Element / # amu g) = (Mol of Element)(6.022x10^23 / 1 mol of Element) = # of Atoms |
(10.0g Al)(1 mol Al/26.98g Al) = (0.317 mol Al)(6.022x10^23/1 mol Al) = 2.23x10^23 atoms |
|
|
Molar Mass of Compound |
(Moles of Element 1)(amu) = Molar Mass 1 (g) (Moles of Element 2)(amu) = Molar Mass 2 (g).... Molar Mass 1(g) + 2(g) = Molar Mass of Compound |
C10H6O3: (10 C)(12.01g) = 120.1g (6 H)(1.008g) = 6.048g (3 O)(16.00g) = 48.00g 120.1+6.048+48.00 = 174.1g (Mass of C10H6O3) |
|
|
Percent Composition of Compound |
(Mass of Element in 1 mol of Compound / Mass of 1 mol of Compound) x 100% = Percent of Element in Compound |
(24.02g C / 46.07g c2h5oh) x 100 = 52.14 % C |
|
|
Determining Formula of a Compound |
(g of Substance in Compound)(Mass of Element / Mass of Substance) = (Mass of Element in Substance / Mass of Compound) x 100 = % Element
(% of Element x 100g of Compound) x (1 mol Element / amu) = (mol of Element ÷ Smallest # mol) = # of mol Element in Compound |
0.1638g CO2 (12.01g C / 44.01g CO2) = (0.04470g C / 0.1156g compound) x 100 = 38.67% C (38.67% C)(100) = (38.67g C)(1 mol C / 12.01g C) = 3.220 mol C... CH5N |
|
|
Determining Empirical and Molecular Formulas |
- |
|
