Question

How many electrons are in 1.01 oz of a pure gold coin?

Answer 1

There are 6.83.10²⁴ electron particles in 1.01 oz of a pure gold coin

Further explanation

A mole is a unit of many particles (atoms, molecules, ions) where 1 mole is the number of particles contained in a substance that is the same amount as many atoms in 12 gr C-12

1 mole = 6.02.10²³ particles

While the number of moles can also be obtained by dividing the mass (in grams) with$\large{\boxed{\bold{mole\:=\:\frac{grams}{ the\:relative\:mass\:of\:elements\:or\:the relative\:mass\:of\:molecules} }}}$

So that in 1 mole of gold there are 6.02.10²³ gold atoms

In the gold atom itself (Gold atomic number = Au = 79) there are 79 electrons so the number of electron ions is: 79 x 6.02.10²³ particles = 4.75.10²⁵ electron particles

1.01 oz of a pure gold coin = 28,3495 grams

relative atomic mass Gold = 197 grams / mole

So that Gold mole = grams : relative atomic mass Gold

Gold mole = 28,3495 grams: 197 grams / mole

Gold mole = 0.1439

Then in 0.1439 gold mole, there are as many electron particles:

 0.1439 x4.75.10²⁵ = 6.83.10²⁴electron particles

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Keywords: mole, Avogadro’s number, electron, gold

Answer 2

$\boxed{6.9157250\times{{10}^{24}}}$ electrons are present in 1.01 oz of pure gold coin.

Further Explanation:

Mole is a measure of the amount of substance. It is defined as the mass of a substance that has the same number of fundamental units as there are atoms in 12 g of carbon-12. Such fundamental units can be atoms, molecules or formula units.

In step 1, we have to convert the mass of gold from oz to grams. The conversion factor for this is,

${\text{1 oz}}={\text{28}}{\text{.3495g}}$                                 …… (1)

Step 1:

So the mass of gold is calculated as follows:

$\begin{gathered}{\text{Mass of gold}}=\left({{\text{1}}{\text{.01 oz}}}\right)\left({\frac{{{\text{28}}{\text{.3495g}}}}{{{\text{1 oz}}}}}\right)\\=28.632995\;{\text{g}}\\\approx{\mathbf{28}}{\mathbf{.633}}\;{\mathbf{g}}\\\end{gathered}$

In step 2, the number of moles of gold is calculated. The moles of gold is calculated by using equation (2).

Step 2:

The formula to calculate the moles of gold is as follows:

${\text{Moles of gold}}=\frac{{{\text{Given mass of gold}}}}{{{\text{Molar mass of gold}}}}$                             …… (2)

Given mass of gold is 28.633 g.

Molar mass of gold is 196.967 g/mol.

Substitute these values in equation (2).

$\begin{gathered}{\text{Moles of gold}}=\left({28.633{\text{g}}}\right)\left({\frac{{{\text{1 mol}}}}{{{\text{196}}{\text{.967g}}}}}\right)\\={\mathbf{0}}{\mathbf{.145369}}\;{\mathbf{mol}}\\\end{gathered}$

In step 3, the number of moles of electrons is to be calculated. The moles of electrons are calculated using equation (3).  

Step 3:

As we know, the atomic number of the element is equal to the number of protons in it, which in turn is equal to the number of electrons in a neutral atom. According to periodic table, the atomic number of gold is 79 and therefore it has 79 protons and 79 electrons.

The formula to calculate the moles of electrons in gold is as follows:

${\text{Moles of electrons in gold}}{\mathbf{=}}\left({{\text{Number of electrons in gold}}}\right)\left({{\text{Moles of gold}}}\right)$       …… (3)

The number of electrons in gold is 79.

The moles of gold is 0.145369 mol.

Substitute these values in equation (3).

$\begin{gathered}{\text{Moles of electrons in gold}}{\mathbf{=}}\left({{\text{79}}}\right)\left({{\text{0}}{\text{.145369 mol}}}\right)\\={\mathbf{11}}{\mathbf{.4841}}\;{\mathbf{mol}}\\\end{gathered}$

In step 4, the moles of electrons calculated in step 3 are to be multiplied with the Avogadro number in order to calculate the number of electrons in the gold atom. This is done by using equation (4).

Step 4:

The number of electrons in gold is calculated as follows:

${\text{Number of electrons in gold}}{\mathbf{=}}\left({{\text{Moles of electrons}}}\right)\left({{\text{Avogadro's Number}}}\right)$            …… (4)

The moles of electrons are 11.4841 mol.

The value of Avogadro’s number is ${\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{{\text{23}}}}{\text{ electrons/mol}}$.

Substitute these values in equation (4).

$\begin{gathered}{\text{Number of electrons in gold}}{\mathbf{=}}\left({11.4841\;{\text{mol}}}\right)\left({\frac{{{\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{{\text{23}}}}{\text{electrons}}}}{{{\text{1 mol}}}}}\right)\\={\mathbf{6}}{\mathbf{.9157250\times1}}{{\mathbf{0}}^{{\mathbf{24}}}}\\\end{gathered}$

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2. What is the number of moles of ions in HCl solution? https://brainly.com/question/5950133

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Mole concept

Keywords: moles, molar mass, gold, electrons, Avogadro’s number, number of electrons, 11.4841 mol, atomic number, protons.