Answered

Discover a wealth of knowledge at Westonci.ca, where experts provide answers to your most pressing questions. Ask your questions and receive precise answers from experienced professionals across different disciplines. Join our Q&A platform to connect with experts dedicated to providing accurate answers to your questions in various fields.

How many grams of [tex]Fe_2O_3[/tex] can form from [tex]26.7 \, \text{g}[/tex] of [tex]O_2[/tex]?

[tex]4 \, Fe(s) + 3 \, O_2(g) \longrightarrow 2 \, Fe_2O_3(s)[/tex]

Sagot :

GinnyAnswer
Certainly! Let's go through the problem step by step.

Step 1: Understand the given data and balanced chemical equation

The balanced chemical equation is:
[tex]\[ 4 \text{Fe (s)} + 3 \text{O}_2 \text{(g)} \rightarrow 2 \text{Fe}_2\text{O}_3 \text{(s)} \][/tex]

Step 2: Determine the molar masses

From the periodic table:
- The molar mass of [tex]\( \text{O}_2 \)[/tex] is approximately [tex]\( 32.00 \, \text{g/mol} \)[/tex].
- The molar mass of [tex]\( \text{Fe}_2\text{O}_3 \)[/tex] is approximately [tex]\( 159.69 \, \text{g/mol} \)[/tex].

Step 3: Calculate the number of moles of [tex]\( \text{O}_2 \)[/tex]

Using the formula to convert grams to moles:
[tex]\[ \text{moles of } \text{O}_2 = \frac{\text{mass of } \text{O}_2}{\text{molar mass of } \text{O}_2} \][/tex]
[tex]\[ \text{moles of } \text{O}_2 = \frac{26.7 \, \text{g}}{32.00 \, \text{g/mol}} = 0.834375 \, \text{moles} \][/tex]

Step 4: Use stoichiometry to find the moles of [tex]\( \text{Fe}_2\text{O}_3 \)[/tex]

From the balanced chemical equation, we know that 3 moles of [tex]\( \text{O}_2 \)[/tex] produce 2 moles of [tex]\( \text{Fe}_2\text{O}_3 \)[/tex]. So, we can set up the following ratio:
[tex]\[ \frac{2 \, \text{moles of } \text{Fe}_2\text{O}_3}{3 \, \text{moles of } \text{O}_2} \][/tex]

Now, we use this ratio to find out how many moles of [tex]\( \text{Fe}_2\text{O}_3 \)[/tex] are formed from the 0.834375 moles of [tex]\( \text{O}_2 \)[/tex]:
[tex]\[ \text{moles of } \text{Fe}_2\text{O}_3 = 0.834375 \, \text{moles of } \text{O}_2 \times \frac{2 \, \text{moles of } \text{Fe}_2\text{O}_3}{3 \, \text{moles of } \text{O}_2} \][/tex]
[tex]\[ \text{moles of } \text{Fe}_2\text{O}_3 = 0.55625 \, \text{moles} \][/tex]

Step 5: Convert moles of [tex]\( \text{Fe}_2\text{O}_3 \)[/tex] to mass

Using the molar mass of [tex]\( \text{Fe}_2\text{O}_3 \)[/tex]:
[tex]\[ \text{mass of } \text{Fe}_2\text{O}_3 = \text{moles of } \text{Fe}_2\text{O}_3 \times \text{molar mass of } \text{Fe}_2\text{O}_3 \][/tex]
[tex]\[ \text{mass of } \text{Fe}_2\text{O}_3 = 0.55625 \, \text{moles} \times 159.69 \, \text{g/mol} \][/tex]
[tex]\[ \text{mass of } \text{Fe}_2\text{O}_3 = 88.8275625 \, \text{g} \][/tex]

Final Answer: The mass of [tex]\( \text{Fe}_2\text{O}_3 \)[/tex] that can form from 26.7 grams of [tex]\( \text{O}_2 \)[/tex] is approximately 88.83 grams.
Thank you for visiting. Our goal is to provide the most accurate answers for all your informational needs. Come back soon. We hope our answers were useful. Return anytime for more information and answers to any other questions you have. Get the answers you need at Westonci.ca. Stay informed by returning for our latest expert advice.