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Chapter 3 Mass relationship in chemical reaction

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Yau Hsiung Wong

on 7 October 2013

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Transcript of Chapter 3 Mass relationship in chemical reaction

Chapter 3


Atomic mass unit (amu)

1) For atoms ---> Atomic mass (amu)
2) For molecules ---> Molecular mass (amu)
3) For formula units ---> Formula mass (amu)
In general ---> molar mass (g/mol)
Finding Moles
1) Moles (mol) = Mass (g) / molar mass (g/mol)
2) Moles (mol) = # of particles / 6.02x 10^23
Finding % composition
of element in compound
n x molar mass of element/ molar mass of compound x 100 %
Finding Empirical and
Molecular formula
1) Percentage (%)
2) Mass (g)
3) Moles (mol)
4) Smallest whole-number ratios
5) ---> Empirical formula (EF)
6) (Emprical mass) n = Formula mass
7) ---> Molecular formula (MF)
1) Balance the chemical equation.
2) Determine known (reactant) and unknown (product)
3) Convert known (mass) into moles.
4) Use coefficients (
molar ratio
) to relate the known to unknown
5) Solve for unknown (in moles)
6) Convert unknown into mass
7) Identify limiting reactant (LR) and excess reactant (ER)
8) Choose the
amount of product (based on LR) = thereotical yield
9) Calculate percent yield if given actual yield
10) Percent yield (%) = actual yield (g)/ theoretical yield (g)

Average Atomic Mass (AAM)
1) AAM= Sum of (isotopic mass x fractional abundance)
2) AAM= Sum of (isotopic mass x percentage abundance)/ 100
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