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1.0 mol of Fe reacts completely with 0.65 mol of 02 to give a mixture of only Fe0 and Fe2O3. The mole ratio of ferrous oxide to ferric oxide is
- a)2 : 2
- b)4:3
- c)1:2
- d)2: 7
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
1.0 mol of Fe reacts completely with 0.65 mol of 02 to give a mixture ...
2Fe + O2 →→ 2FeO
4Fe + 3O2 →→2Fe2O3
Let x moles of Fe reacts to produce FeO
Thus amount of Fe reacted to produce Fe2O3 = 1-x Moles
Now
2 Moles of Fe reacts to produce FeO with = 1 moles of O2
1 moles of Fe reacts to produce FeO with = 1/2 moles of O2
x moles of Fe to produce FeO with = 0.5x moles of O2
4 moles of Fe reacts to produce Fe2O3 with = 3 moles of O2
1-x moles of Fe reacts to produce Fe2O3 = (3/4) x (1-x) Moles of O2
EQUATION :
1) 0.5x + 3/4(1−x) =0.65 moles of O2
Thus
x = 0.4 moles
2 Moles of Fe produces = 2 mole of FeO
0.4 moles of Fe produces = 0.4 moles of FeO
4 moles of Fe produces = 2 moles of Fe2O3
(1-0.4 )moles of Fe produces = (1/2) x 0.6 Moles = 0.3 moles of Fe2O3
Thus
FeO/Fe2O3 = 0.4/0.3 = 43
Most Upvoted Answer
1.0 mol of Fe reacts completely with 0.65 mol of 02 to give a mixture ...
Mole Ratio of Ferrous Oxide to Ferric Oxide
Given:
- 1.0 mol of Fe reacts completely with 0.65 mol of O2.
- The reaction produces a mixture of only Fe0 (ferrous oxide) and Fe2O3 (ferric oxide).
To determine the mole ratio of ferrous oxide (Fe0) to ferric oxide (Fe2O3), we need to calculate the moles of each compound formed in the reaction.
1. Calculate the moles of Fe0:
Since 1 mol of Fe reacts completely with 0.65 mol of O2, the number of moles of Fe0 formed is equal to the moles of Fe consumed in the reaction, which is 1 mol.
2. Calculate the moles of Fe2O3:
Since the reaction produces a mixture of Fe0 and Fe2O3, the total moles of Fe2O3 formed can be calculated by subtracting the moles of Fe0 from the total moles of iron used in the reaction.
Total moles of iron used = moles of Fe0 + moles of Fe2O3
1 mol of Fe + moles of Fe2O3 = 1 mol of Fe + 0.65 mol of O2
moles of Fe2O3 = 0.65 mol of O2
Therefore, the mole ratio of ferrous oxide (Fe0) to ferric oxide (Fe2O3) is 1:0.65, which simplifies to 20:13.
To determine the closest answer option, we can simplify the ratio further:
20:13 = (20/4):(13/4) = 5:3
Comparing this ratio to the given answer options, we find that the correct answer is option B) 4:3.
Therefore, the mole ratio of ferrous oxide to ferric oxide is 4:3.
Given:
- 1.0 mol of Fe reacts completely with 0.65 mol of O2.
- The reaction produces a mixture of only Fe0 (ferrous oxide) and Fe2O3 (ferric oxide).
To determine the mole ratio of ferrous oxide (Fe0) to ferric oxide (Fe2O3), we need to calculate the moles of each compound formed in the reaction.
1. Calculate the moles of Fe0:
Since 1 mol of Fe reacts completely with 0.65 mol of O2, the number of moles of Fe0 formed is equal to the moles of Fe consumed in the reaction, which is 1 mol.
2. Calculate the moles of Fe2O3:
Since the reaction produces a mixture of Fe0 and Fe2O3, the total moles of Fe2O3 formed can be calculated by subtracting the moles of Fe0 from the total moles of iron used in the reaction.
Total moles of iron used = moles of Fe0 + moles of Fe2O3
1 mol of Fe + moles of Fe2O3 = 1 mol of Fe + 0.65 mol of O2
moles of Fe2O3 = 0.65 mol of O2
Therefore, the mole ratio of ferrous oxide (Fe0) to ferric oxide (Fe2O3) is 1:0.65, which simplifies to 20:13.
To determine the closest answer option, we can simplify the ratio further:
20:13 = (20/4):(13/4) = 5:3
Comparing this ratio to the given answer options, we find that the correct answer is option B) 4:3.
Therefore, the mole ratio of ferrous oxide to ferric oxide is 4:3.
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1.0 mol of Fe reacts completely with 0.65 mol of 02 to give a mixture of only Fe0 and Fe2O3. The mole ratio of ferrous oxide to ferric oxide isa)2 : 2b)4:3c)1:2d) 2: 7Correct answer is option 'B'. Can you explain this answer?
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