Get the best answers to your questions with the help of IDNLearn.com's experts. Our platform offers reliable and detailed answers, ensuring you have the information you need.
Sagot :
Let's analyze the balanced chemical reaction and answer each part of the question systematically.
The balanced equation is:
[tex]\[ 3 \text{Fe} + 4 \text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + 4 \text{H}_2 \][/tex]
### 2.1 How many moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] will be formed from 12 moles of Fe?
From the balanced equation, the molar ratio of Fe to Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] is 3:1. This means 3 moles of Fe produce 1 mole of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex].
To find the moles of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] formed from 12 moles of Fe, we use the ratio:
[tex]\[ \text{Moles of Fe}_3\text{O}_4 = \frac{12 \text{ moles of Fe}}{3} = 4 \text{ moles} \][/tex]
Thus, 4 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] will be formed from 12 moles of Fe.
### 2.2 How many moles of Fe are needed to produce 16 moles of [tex]\(\text{H}_2\)[/tex]?
From the balanced equation, the molar ratio of Fe to H[tex]\(_2\)[/tex] is 3:4. This means 3 moles of Fe produce 4 moles of H[tex]\(_2\)[/tex].
To find the moles of Fe needed to produce 16 moles of H[tex]\(_2\)[/tex], we use the ratio:
[tex]\[ \text{Moles of Fe} = \frac{3}{4} \times 16 \text{ moles of H}_2 = 12 \text{ moles} \][/tex]
Thus, 12 moles of Fe are needed to produce 16 moles of [tex]\(\text{H}_2\)[/tex].
### 2.3 How many moles of [tex]\(\text{H}_2\)[/tex] will be formed if 40 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] are formed?
From the balanced equation, the molar ratio of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] to H[tex]\(_2\)[/tex] is 1:4. This means 1 mole of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] produces 4 moles of H[tex]\(_2\)[/tex].
To find the moles of H[tex]\(_2\)[/tex] formed from 40 moles of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex], we use the ratio:
[tex]\[ \text{Moles of H}_2 = 4 \times 40 \text{ moles of Fe}_3\text{O}_4 = 160 \text{ moles} \][/tex]
Thus, 160 moles of [tex]\(\text{H}_2\)[/tex] will be formed if 40 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] are formed.
### 2.4 How many moles of [tex]\(\text{H}_2\text{O}\)[/tex] are needed to react with 14.5 moles of Fe?
From the balanced equation, the molar ratio of Fe to H[tex]\(_2\)[/tex]O is 3:4. This means 3 moles of Fe react with 4 moles of H[tex]\(_2\)[/tex]O.
To find the moles of H[tex]\(_2\)[/tex]O needed to react with 14.5 moles of Fe, we use the ratio:
[tex]\[ \text{Moles of H}_2\text{O} = \frac{4}{3} \times 14.5 \text{ moles of Fe} = \frac{4 \times 14.5}{3} = \frac{58}{3} \approx 19.33 \text{ moles} \][/tex]
Thus, approximately 19.33 moles of [tex]\(\text{H}_2\text{O}\)[/tex] are needed to react with 14.5 moles of Fe.
In summary:
2.1. 4 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] will be formed from 12 moles of Fe.
2.2. 12 moles of Fe are needed to produce 16 moles of [tex]\(\text{H}_2\)[/tex].
2.3. 160 moles of [tex]\(\text{H}_2\)[/tex] will be formed if 40 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] are formed.
2.4. Approximately 19.33 moles of [tex]\(\text{H}_2\text{O}\)[/tex] are needed to react with 14.5 moles of Fe.
The balanced equation is:
[tex]\[ 3 \text{Fe} + 4 \text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + 4 \text{H}_2 \][/tex]
### 2.1 How many moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] will be formed from 12 moles of Fe?
From the balanced equation, the molar ratio of Fe to Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] is 3:1. This means 3 moles of Fe produce 1 mole of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex].
To find the moles of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] formed from 12 moles of Fe, we use the ratio:
[tex]\[ \text{Moles of Fe}_3\text{O}_4 = \frac{12 \text{ moles of Fe}}{3} = 4 \text{ moles} \][/tex]
Thus, 4 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] will be formed from 12 moles of Fe.
### 2.2 How many moles of Fe are needed to produce 16 moles of [tex]\(\text{H}_2\)[/tex]?
From the balanced equation, the molar ratio of Fe to H[tex]\(_2\)[/tex] is 3:4. This means 3 moles of Fe produce 4 moles of H[tex]\(_2\)[/tex].
To find the moles of Fe needed to produce 16 moles of H[tex]\(_2\)[/tex], we use the ratio:
[tex]\[ \text{Moles of Fe} = \frac{3}{4} \times 16 \text{ moles of H}_2 = 12 \text{ moles} \][/tex]
Thus, 12 moles of Fe are needed to produce 16 moles of [tex]\(\text{H}_2\)[/tex].
### 2.3 How many moles of [tex]\(\text{H}_2\)[/tex] will be formed if 40 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] are formed?
From the balanced equation, the molar ratio of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] to H[tex]\(_2\)[/tex] is 1:4. This means 1 mole of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex] produces 4 moles of H[tex]\(_2\)[/tex].
To find the moles of H[tex]\(_2\)[/tex] formed from 40 moles of Fe[tex]\(_3\)[/tex]O[tex]\(_4\)[/tex], we use the ratio:
[tex]\[ \text{Moles of H}_2 = 4 \times 40 \text{ moles of Fe}_3\text{O}_4 = 160 \text{ moles} \][/tex]
Thus, 160 moles of [tex]\(\text{H}_2\)[/tex] will be formed if 40 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] are formed.
### 2.4 How many moles of [tex]\(\text{H}_2\text{O}\)[/tex] are needed to react with 14.5 moles of Fe?
From the balanced equation, the molar ratio of Fe to H[tex]\(_2\)[/tex]O is 3:4. This means 3 moles of Fe react with 4 moles of H[tex]\(_2\)[/tex]O.
To find the moles of H[tex]\(_2\)[/tex]O needed to react with 14.5 moles of Fe, we use the ratio:
[tex]\[ \text{Moles of H}_2\text{O} = \frac{4}{3} \times 14.5 \text{ moles of Fe} = \frac{4 \times 14.5}{3} = \frac{58}{3} \approx 19.33 \text{ moles} \][/tex]
Thus, approximately 19.33 moles of [tex]\(\text{H}_2\text{O}\)[/tex] are needed to react with 14.5 moles of Fe.
In summary:
2.1. 4 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] will be formed from 12 moles of Fe.
2.2. 12 moles of Fe are needed to produce 16 moles of [tex]\(\text{H}_2\)[/tex].
2.3. 160 moles of [tex]\(\text{H}_2\)[/tex] will be formed if 40 moles of [tex]\(\text{Fe}_3\text{O}_4\)[/tex] are formed.
2.4. Approximately 19.33 moles of [tex]\(\text{H}_2\text{O}\)[/tex] are needed to react with 14.5 moles of Fe.
Thank you for contributing to our discussion. Don't forget to check back for new answers. Keep asking, answering, and sharing useful information. Thank you for choosing IDNLearn.com. We’re dedicated to providing clear answers, so visit us again for more solutions.
