Answered: Results table. To clean up, zoom out…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 3ALQ: True or false? The atom with the largest subscript in a formula is die atom with the largest percent...

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Results table. To clean up, zoom out from the balance and drag the sample to the red disposal

container. Repeat with ammonium chloride (NH4Cl), located on the Salts shelf.
C12H22O11 NH4Cl
Mass (g) 1.0481 g 1.0444g
Molar Mass (g/mol)
Moles
Moles of each element
Atoms of each element

Much like the previous calculation, you will use the periodic table to determine the molar mass
of the compound. The example shown is for sodium chloride, NaCl. The molar mass is the mass
of 1 sodium (22.98g/mole) and 1 chlorine (35.45g/mole) added together, 58.43g/mole. If the
formula shows multiple atoms, as in sugar, you must take that into account. For sugar, it will be
12 times the mass of a carbon atom plus 22 time the mass of hydrogen atom, plus 11 times the
mass of oxygen atoms.
The calculation of moles will be similar to that done in the previous calculation as well.
5.924 g NaCl × 1 mole NaCl
58.43 g NaCl =0.1014 mole NaCl
Now to determine the moles of each element, we will use the ratio of atoms in the formula of
the compound.
0.1014 mole NaCl × 1 mole Na

1 mole NaCl =0.1014 mole Na
You would do the same for chlorine.
To determine the atoms of each element, we will use Avogadro’s number.
0.1014 mole Na × 6.02 ×1023 Na atoms
1 mole Na =6.103× 1022 Na atoms
You would do the same for chlorine.

just need steps to see if im doing it correctly

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