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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.
When iron reacts with oxygen it forms iron oxide or rust. 4 Fe plus 3 O2 2 Fe2O3 If 112 g of iron (Fe) combines with 24 g of oxygen (O2) how much iron oxide is formed?
To determine the amount of iron oxide (Fe2O3) formed, we first need to identify the limiting reactant. The molar mass of Fe is approximately 56 g/mol and for O2, it is about 32 g/mol. Calculating the moles, 112 g of Fe gives 2 moles (112 g / 56 g/mol), and 24 g of O2 gives 0.75 moles (24 g / 32 g/mol). The balanced reaction shows that 4 moles of Fe react with 3 moles of O2; thus, O2 is the limiting reactant. According to the stoichiometry, 0.75 moles of O2 will produce 1.0 mole of Fe2O3, which corresponds to approximately 160 g (1 mole of Fe2O3 is 160 g). Therefore, 160 g of iron oxide is formed.
How many moles of oxygen gas O2 are in 64 grams of O2?
The answer is 2 moles.
How many moles of CO are produced from 5 moles o2?
The answer is 10 moles of carbon monoxide.2 C + O2 = 2 CO
HOW MANY MOLES OF O2 ARE NEEDED TO MAKE 3 MOLE OF WATER?
3 moles of O, so that must be 6 moles of O2
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.
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.
If 1176 grams of FeS2 is allowed to react with 704 grams of O2 according to the following equation how many grams of Fe2O3 are produced?
First, balance the equation: 4FeS2 + 11O2 → 2Fe2O3 + 8SO2. Calculate the moles of each reactant: moles FeS2 = 1176 g / molar mass of FeS2, moles O2 = 704 g / molar mass of O2. Identify the limiting reactant based on the stoichiometry of the reaction, then use stoichiometry to calculate the grams of Fe2O3 produced.
When iron reacts with oxygen it forms iron oxide or rust. 4 Fe plus 3 O2 2 Fe2O3 If 112 g of iron (Fe) combines with 24 g of oxygen (O2) how much iron oxide is formed?
To determine the amount of iron oxide (Fe2O3) formed, we first need to identify the limiting reactant. The molar mass of Fe is approximately 56 g/mol and for O2, it is about 32 g/mol. Calculating the moles, 112 g of Fe gives 2 moles (112 g / 56 g/mol), and 24 g of O2 gives 0.75 moles (24 g / 32 g/mol). The balanced reaction shows that 4 moles of Fe react with 3 moles of O2; thus, O2 is the limiting reactant. According to the stoichiometry, 0.75 moles of O2 will produce 1.0 mole of Fe2O3, which corresponds to approximately 160 g (1 mole of Fe2O3 is 160 g). Therefore, 160 g of iron oxide is formed.
How many moles of oxygen gas O2 are in 64 grams of O2?
The answer is 2 moles.
How many grams of oxygen needed to get iron3 oxide?
To form iron(III) oxide, the chemical equation is: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) From the equation, it can be seen that 3 moles of oxygen (O2) are needed to react with 4 moles of iron (Fe) to produce 2 moles of iron(III) oxide (Fe2O3). The molar mass of oxygen (O2) is approximately 32 g/mol. Therefore, you would need 96 grams of oxygen to react with the iron needed to form iron(III) oxide.
How many moles of h2o are produced when 2.55 moles of O2 react?
4
How many moles of CO are produced from 5 moles o2?
The answer is 10 moles of carbon monoxide.2 C + O2 = 2 CO
HOW MANY MOLES OF O2 ARE NEEDED TO MAKE 3 MOLE OF WATER?
3 moles of O, so that must be 6 moles of O2
If 2Ag2O and 4Ag o2 then if you started with 3.25 moles of Ag2O how many moles of O2 would be produced?
what is ag2o
How many grams of O2 are in 15 moles of O2. with work shown?
15 moles O2 (32 grams/1 mole O2) = 480 grams
How many moles of O2 are needed to to produce 10.2 moles of H2O?
For the reaction 2 H2 + O2 -> 2 H2O, we see that 1 mole of O2 produces 2 moles of H2O. Therefore, to produce 10.2 moles of H2O, we would need 5.1 moles of O2.
