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17 Cards in this Set
- Front
- Back
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Stoichiometry |
the calculation of relative quantities of reactantsand products inchemical reactions. |
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Mole |
The mole is a unit of measurement used inchemistry to express amounts of a chemical substance |
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6.022×10^23 mol−1 |
Avogadro constant |
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Molar Mass |
One mole of a compound contains Avogadro's number (6.022 x 1023) of molecules (molecular compound) or formula units (ionic compound). The molar mass of a compound tells you the mass of 1 mole of that substance. In other words, it tells you the number of grams per mole of a compound. The units for molar mass are, therefore, grams/mole. |
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12.5 g CaCl2 = _______ mol CaCl2
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0.113 mol CaCl2
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10.0 g Na2SO4 = _______ mol Na2SO4
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0.0704 mol Na2SO4
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16 g NaOH = _______ mol NaOH |
0.40 mol NaOH
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125 mg NaOH = ______ mol NaOH
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3.13 x 10-3 mol NaOH |
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0.125 mol CaCl2 = _____ g CaCl2 |
13.9 g CaCl2 |
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0.25 mol Na2SO4 = ______ g Na2SO4
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36 g Na2SO4
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1.55 mol NaOH = ______ g NaOH
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62.0 g NaOH
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molar mass: Fe2O3 |
159.7 g/mol
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molar mass: AgNO3
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169.9 g/mol
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molar mass: Pb(Cr2O7)2
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639.2 g/mol
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molar mass: Ca(ClO4)2
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239.1 g/mol
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How many atoms can be found in 3.91 moles of xenon? |
3.91 mols Xe * (6.022 x 10^23 atoms / 1 mole Xe) = 2.35 x 10^24 atoms Xe |
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Mass Percent of: KCl
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Cl = 35.45 moles/g = 47.5553%
K = 39.09 moles/g = 52.4447% |
