At Westonci.ca, we make it easy for you to get the answers you need from a community of knowledgeable individuals. Explore thousands of questions and answers from a knowledgeable community of experts ready to help you find solutions. Experience the convenience of finding accurate answers to your questions from knowledgeable experts on our platform.

Select the correct answer from each drop-down menu.

What is the empirical formula?

A compound used to treat iron deficiency contains 36.76% iron and 21.11% sulfur.

Fe [ ] S [ ]


Sagot :

To determine the empirical formula of a compound given the percentages of its elements, follow these steps:

1. Determine the mass percentages of the elements in grams:
Given that the compound contains 36.76% iron (Fe) and 21.11% sulfur (S), we can assume a 100-gram sample for simplicity. This implies we have:
- 36.76 grams of iron (Fe)
- 21.11 grams of sulfur (S)

2. Calculate the moles of each element:
We use the molar masses of iron and sulfur to convert the mass into moles. The molar masses are:
- Iron (Fe): 55.845 g/mol
- Sulfur (S): 32.06 g/mol

Using the formula [tex]\( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \)[/tex]:

For iron (Fe):
[tex]\[ \text{moles of Fe} = \frac{36.76 \text{ g}}{55.845 \text{ g/mol}} = 0.6582 \text{ mol} \][/tex]

For sulfur (S):
[tex]\[ \text{moles of S} = \frac{21.11 \text{ g}}{32.06 \text{ g/mol}} = 0.6585 \text{ mol} \][/tex]

3. Calculate the mole ratio:
To find the mole ratio, divide each element's moles by the smallest number of moles calculated:

- For Fe:
[tex]\[ \text{ratio of Fe} = \frac{0.6582}{0.6582} = 1.0 \][/tex]

- For S:
[tex]\[ \text{ratio of S} = \frac{0.6585}{0.6582} = 1.0 \][/tex]

4. Derive the empirical formula:
The mole ratio for both elements is approximately 1:1. Therefore, the empirical formula of the compound is:

[tex]\[ \text{Fe}_1\text{S}_1 \text{ or simply } \text{FeS} \][/tex]

So, the correct answer is:
- [tex]$Fe$[/tex] [tex]\( \square\)[/tex] = 1
- [tex]$S$[/tex] [tex]\( \square\)[/tex] = 1

The empirical formula is [tex]\( \text{FeS} \)[/tex].

Answer:

FeS

Explanation:

1. Determine the mass percentages of the elements in grams:

Given that the compound contains 36.76% iron (Fe) and 21.11% sulfur (S), we can assume a 100-gram sample for simplicity. This implies we have:

- 36.76 grams of iron (Fe)

- 21.11 grams of sulfur (S)

2. Calculate the moles of each element:

We use the molar masses of iron and sulfur to convert the mass into moles. The molar masses are:

- Iron (Fe): 55.845 g/mol

- Sulfur (S): 32.06 g/mol

Using the formula \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \):

For iron (Fe):

\[

  \text{moles of Fe} = \frac{36.76 \text{ g}}{55.845 \text{ g/mol}} = 0.6582 \text{ mol}

  \]

For sulfur (S):

\[

  \text{moles of S} = \frac{21.11 \text{ g}}{32.06 \text{ g/mol}} = 0.6585 \text{ mol}

  \]

3. Calculate the mole ratio:

To find the mole ratio, divide each element's moles by the smallest number of moles calculated:

- For Fe:

\[

  \text{ratio of Fe} = (0.6582)/(0.6582) = 1.0

  \]

- For S:

\[

  \text{ratio of S} = (0.6585)/(0.6582) = 1.0

  \]

4. Derive the empirical formula:

The mole ratio for both elements is approximately 1:1. Therefore, the empirical formula of the compound is:

\[

  \text{Fe}_1\text{S}_1 \text{ or simply } \text{FeS}

  \]

So, the correct answer is:

- $Fe$ \( \square\) = 1

- $S$ \( \square\) = 1

The empirical formula is \( \text{FeS} \).

We appreciate your time. Please come back anytime for the latest information and answers to your questions. Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. Thank you for trusting Westonci.ca. Don't forget to revisit us for more accurate and insightful answers.