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To find out how many moles of FeCr2O7 are required to produce 107 moles of Fe2O3, we first need to consider the balanced chemical reaction. The reaction can be represented as:
[ 2 , \text{FeCr}_2\text{O}_7 \rightarrow 2 , \text{Fe}_2\text{O}_3 + 2 , \text{Cr}_2\text{O}_3 ]
From the equation, 2 moles of FeCr2O7 produce 2 moles of Fe2O3, which means 1 mole of FeCr2O7 produces 1 mole of Fe2O3. Therefore, to produce 107 moles of Fe2O3, you would need 107 moles of FeCr2O7.
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How many moles of O2 are required to produce 107.9 moles of FE2O3?
The balanced chemical equation for the formation of iron(III) oxide (Fe2O3) from iron (Fe) and oxygen (O2) is: 4 Fe + 3 O2 → 2 Fe2O3. From the equation, it can be seen that 3 moles of O2 are required to produce 2 moles of Fe2O3. Therefore, to produce 107.9 moles of Fe2O3, you would need (107.9 moles Fe2O3) × (3 moles O2 / 2 moles Fe2O3) = 161.85 moles of O2.
If 309 moles of FeCr2O7 react how many moles of O2 will be consumed?
To determine how many moles of O2 are consumed when 309 moles of FeCr2O7 react, we first need the balanced chemical equation for the reaction. Assuming FeCr2O7 decomposes to yield Fe, Cr, and O2, a typical reaction could produce 3 moles of O2 for every mole of FeCr2O7. If this is the case, 309 moles of FeCr2O7 would consume 3 × 309 = 927 moles of O2.
How many moles of Fe2O3 are necessary to produce 0.824 mol of CO2?
To determine how many moles of Fe2O3 are required to produce 0.824 moles of CO2, we first need to look at the balanced chemical reaction involved in the process. In the reduction of iron(III) oxide (Fe2O3) with carbon (C), the reaction can be represented as: [ \text{Fe}_2\text{O}_3 + 3\text{C} \rightarrow 2\text{Fe} + 3\text{CO} ] In this reaction, 1 mole of Fe2O3 produces 3 moles of CO. Since CO2 is produced from the combustion of CO, we need to convert CO to CO2. However, the stoichiometry from Fe2O3 to CO directly leads us to find that 1 mole of Fe2O3 results in the generation of 3 moles of CO, which can then produce CO2. Thus, to produce 0.824 moles of CO2, we will need to calculate based on the conversion of moles of CO to CO2 (1:1 ratio). Therefore, we need: [ \text{Moles of Fe}_2\text{O}_3 = \frac{0.824 , \text{mol CO2}}{3 , \text{mol CO}} \approx 0.2747 , \text{mol Fe2O3} ] Thus, approximately 0.275 moles of Fe2O3 are needed to produce 0.824 moles of CO2.
How many moles of Fe2O3 are in 231 g of the compound?
231 g of Fe2O3 are equal to 0,69 moles.
How many moles of fe2o3 are made from 6 moles of o2?
Fe ions =,Fe 2+andFe 3+Oxygen ions =,O 2-So, as you should see, Fe3O4, is an invalid species as the charge on the first iron ion would be 3 * 2+ = 6 +, and the charge on the second iron ion would be 3 * 3+ = 9+. This can not equal 4 * 2- = 8 -.
How many moles of O2 are required to produce 107.9 moles of FE2O3?
The balanced chemical equation for the formation of iron(III) oxide (Fe2O3) from iron (Fe) and oxygen (O2) is: 4 Fe + 3 O2 → 2 Fe2O3. From the equation, it can be seen that 3 moles of O2 are required to produce 2 moles of Fe2O3. Therefore, to produce 107.9 moles of Fe2O3, you would need (107.9 moles Fe2O3) × (3 moles O2 / 2 moles Fe2O3) = 161.85 moles of O2.
If 309 moles of FeCr2O7 react how many moles of O2 will be consumed?
To determine how many moles of O2 are consumed when 309 moles of FeCr2O7 react, we first need the balanced chemical equation for the reaction. Assuming FeCr2O7 decomposes to yield Fe, Cr, and O2, a typical reaction could produce 3 moles of O2 for every mole of FeCr2O7. If this is the case, 309 moles of FeCr2O7 would consume 3 × 309 = 927 moles of O2.
How many moles of Fe2O3 are necessary to produce 0.824 mol of CO2?
To determine how many moles of Fe2O3 are required to produce 0.824 moles of CO2, we first need to look at the balanced chemical reaction involved in the process. In the reduction of iron(III) oxide (Fe2O3) with carbon (C), the reaction can be represented as: [ \text{Fe}_2\text{O}_3 + 3\text{C} \rightarrow 2\text{Fe} + 3\text{CO} ] In this reaction, 1 mole of Fe2O3 produces 3 moles of CO. Since CO2 is produced from the combustion of CO, we need to convert CO to CO2. However, the stoichiometry from Fe2O3 to CO directly leads us to find that 1 mole of Fe2O3 results in the generation of 3 moles of CO, which can then produce CO2. Thus, to produce 0.824 moles of CO2, we will need to calculate based on the conversion of moles of CO to CO2 (1:1 ratio). Therefore, we need: [ \text{Moles of Fe}_2\text{O}_3 = \frac{0.824 , \text{mol CO2}}{3 , \text{mol CO}} \approx 0.2747 , \text{mol Fe2O3} ] Thus, approximately 0.275 moles of Fe2O3 are needed to produce 0.824 moles of CO2.
How many moles of iron can be produced from the reaction of 10 mol Fe2O3 and 25 mol of CO?
From the balanced chemical equation 3Fe2O3 + CO → 2Fe3O4 + CO2, it can be seen that 3 moles of Fe2O3 react with 1 mole of CO to produce 2 moles of Fe. Therefore, if 25 moles of CO react, it will produce 25/3 * 2 = 16.67 moles of Fe.
How many moles of Fe2O3 are in 231 g of the compound?
231 g of Fe2O3 are equal to 0,69 moles.
How many Fe atoms are in 0.25 moles of Fe?
To determine the number of moles of Fe that can be made from 25 moles of Fe2O3, you need to write the balanced chemical equation for producing O2 from Fe2O3. 2Fe2O3 = 4Fe + 3O2, which means that 2 moles of Fe2O3 will produce 4 moles of Fe and 3 moles of O2 . Set up a proportion. 3 moles of O2 ÷ 2 moles of Fe2O3 = x moles of O2 ÷ 25 moles of Fe2O3 Cross multiply and divide. 3 moles of O2 * 25 moles of Fe2O3 ÷ 2 moles of Fe2O3 = 37.5 moles of O2 produced.
How many moles of fe2o3 are in 217g of the compound?
To determine the number of moles of Fe2O3 in 217g of the compound, you first need to calculate the molar mass of Fe2O3, which is 159.69 g/mol. Then, divide the given mass (217g) by the molar mass to find the moles. Moles = 217g / 159.69 g/mol = 1.36 moles of Fe2O3.
What mole ratio would you use to determine moles Fe if moles Fe2O3 is known?
If the moles of Fe2O3 are known, you would use the mole ratio from the balanced chemical equation for the reaction involving Fe2O3 and Fe. In the balanced equation, the mole ratio between Fe2O3 and Fe is 2:2, which simplifies to 1:1. This means that for every mole of Fe2O3, there is an equivalent mole of Fe.
The formula for rust can be represented by Fe2O3 How many moles of Fe are present in 14.2 g of the compound?
To find the number of moles of Fe in 14.2 g of Fe2O3, we need to use the molar mass of Fe2O3 (molecular weight = 159.69 g/mol) and the ratio of Fe to Fe2O3. There are 2 moles of Fe in 1 mole of Fe2O3, so we find the moles of Fe in 14.2 g of Fe2O3 by: (14.2 g / 159.69 g/mol) * 2 = 0.249 moles of Fe.
Identify the number of moles of excess reagent left over when 6.258 moles of iron(III) oxide are reacted with 8.359 moles of aluminum in the thermite reaction?
The balanced equation for the thermite reaction involving iron(III) oxide (Fe2O3) and aluminum (Al) is: Fe2O3 + 2Al -> 2Fe + Al2O3 From the equation, it is clear that 1 mole of Fe2O3 reacts with 2 moles of Al. The number of moles of Al needed to react with 6.258 moles of Fe2O3 is 3.129 moles (6.258 moles Fe2O3 * 2 moles Al / 1 mole Fe2O3). Since 8.359 moles of Al are provided, the excess amount of Al is 8.359 moles - 3.129 moles = 5.230 moles.
How many grams of oxygen are needed to react with 350 grams of iron to produce 500 grams of fe203?
The balanced chemical equation for the reaction between iron and oxygen to produce Fe2O3 is 4Fe + 3O2 -> 2Fe2O3. From the equation, we see that 3 moles of oxygen react with 4 moles of iron to produce 2 moles of Fe2O3. Therefore, to find the grams of oxygen needed, we need to calculate the molar mass of Fe2O3 and then determine the number of grams needed using the mole ratio from the balanced equation.
If 1.00 kg of Fe2O3 completely reacts with CO the volume of CO2 released at STP will be?
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
