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1. A sample of gold (Au) has a mass of 35.12 g.
a. Calculate the number of moles of gold (Au) in the sample and record in
Table 1. Show your work.
b. Calculate the number of atoms of gold (Au) in the sample and record
in Table 1. Show your work.

2. A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.
a. Calculate the number of moles of C12H22O11 contained in the sample
and record in Table 1. Show your work.
b. Calculate the moles of each element in C12H22O11 and record in Table
1. Show your work.
c. Calculate the number of atoms of each type in C12H22O11 and record in
Table 1. Show your work.

Respuesta :

JcAlmighty
Q1. a) The answer is 0.1783 moles.
Atomic mass (Ar) of gold is 196.97 g. A mole (M) is an atomic or molar mass in 1000 ml:
Au: 1M = 196.97g/1000ml                           ⇒ 1000 ml = 196.97g/1M
A sample of gold: xM = 35.12g/1000ml     ⇒ 1000 ml = 35.12g/x

1000 ml = 196.97g/1M = 35.12g/x
⇒ 196.97g/1M = 35.12g/x
     x = 35.12g / 196.97g * 1M = 0.1783M


Q1. b) The answer is 1.073 × 10²³ atoms.

To calculate this, we will use Avogadro's number which is the number of units (atoms, molecules) in 1 mole of substance: 6.02 × 10²³ units per 1 mole

From the previous task, we know that the sample of gold has 0.1783 moles.

Now, let's make a proportion:

6.02 × 10²³atoms : 1M = x : 0.1783 M

After crossing the products:

x = 6.02× 10²³atoms * 0.1783 M / 1M = 1.073 × 10²³ atoms



Q2. a) The answer is 0.0035 moles.

Let's first calculate molar mass (Mr) of sucrose which is a sum of atomic masses (Ar) of elements:

Mr(C₁₂H₂₂O₁₁) = 12Ar(C) + 22Ar(H) + 11Ar(O) = 12*12 + 22*1 + 11*16 = 

                      = 144 + 22 + 176 = 342 g

A mole (M) is an atomic or molar mass in 1000 ml:

Sucrose: 1M = 342g/1000ml                                ⇒ 1000 ml = 342g/1M

A sample of sucrose: xM = 1.202g/1000ml        ⇒ 1000 ml = 1.202g/x

1000 ml = 342g/1M = 1.202g/x

⇒  342g/1M = 1.202g/x

      x = 1.202g / 342g * 1M = 0.0035 M



Q2. b) The answers are:

- carbon: 0.042 moles

- hydrogen: 0.077 moles

- oxygen: 0.0385 moles

In a sample of sucrose of 0.0035 M, there are 12 atoms of carbon:

12 * 0.0035M = 0.042 M

In a sample of sucrose of 0.0035 M, there are 22 atoms of hydrogen:

22 * 0.0035M = 0.077 M

In a sample of sucrose of 0.0035 M, there are 11 atoms of oxygen:

11 * 0.0035M = 0.0385 M



Q2. c) The answers are:

- carbon: 2.5 × 10²⁴ atoms

- hydrogen: 4.6 × 10²⁴ atoms

- oxygen: 2.3 × 10²⁴ atoms

To calculate this, we will use Avogadro's number which is the number of units (atoms, molecules) in 1 mole of substance: 6.02 × 10²³ units per 1 mole

- carbon: 0.042 moles (from the previous task)

Now, let's make a proportion:

6.02 × 10²³atoms : 1M = x : 0.042 M

After crossing the products:

x = 6.02× 10²³atoms * 0.042 M / 1M = 0.25 × 10²³ atoms = 2.5 × 10²⁴ atoms


- hydrogen: 0.077 moles (from the previous task)

Now, let's make a proportion:

6.02 × 10²³atoms : 1M = x : 0.077 M

After crossing the products:

x = 6.02× 10²³atoms * 0.077 M / 1M = 0.46 × 10²³ atoms = 4.6 × 10²⁴ atoms


- oxygen: 0.0385 moles (from the previous task)

Now, let's make a proportion:

6.02 × 10²³atoms : 1M = x : 0.0385 M

After crossing the products:

x = 6.02× 10²³atoms * 0.0385 M / 1M = 0.23 × 10²³ atoms = 2.3 × 10²⁴ atoms

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