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How many moles of fe3o4 are needed to prepare 4.05moles of fe2o3?
To find the moles of Fe3O4 needed, we first need to determine the molar ratio between Fe3O4 and Fe2O3. The balanced chemical equation for the conversion will provide this information. If the equation is Fe3O4 -> 2Fe2O3, then the molar ratio is 1:2. Thus, 4.05 moles of Fe2O3 would require 2 * 4.05 = 8.1 moles of Fe3O4.
What is the correct form of the conversion factor needed to convert the number of moles of O2 to the number of moles of Fe2O3?
To convert the number of moles of O2 to the number of moles of Fe2O3, you can use the stoichiometric coefficients from the balanced chemical equation for the reaction. For example, in the formation of Fe2O3 from iron (Fe) and oxygen (O2), the balanced equation is 4 Fe + 3 O2 → 2 Fe2O3. Thus, the conversion factor is based on the ratio of moles of O2 to moles of Fe2O3, which is 3 moles of O2 for every 2 moles of Fe2O3. Therefore, the conversion factor is ( \frac{2 , \text{moles of Fe2O3}}{3 , \text{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.
How many moles of iron oxide are needed to react with 2.5 mol of Al?
The balanced chemical equation for the reaction between iron oxide (Fe2O3) and aluminum (Al) is 2Al + Fe2O3 → Al2O3 + 2Fe. This shows that 2 moles of Al react with 1 mole of Fe2O3. Therefore, 2.5 moles of Al would need 1.25 moles of Fe2O3 to completely react.
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 CO are needed to react with 3.16 g of Fe2O3?
To calculate the grams of CO needed to react with Fe2O3, you need to write a balanced chemical equation for the reaction, determine the moles of Fe2O3 given the mass provided, and use the stoichiometry of the balanced equation to find the moles of CO needed. Finally, convert the moles of CO to grams using the molar mass of CO.
If 4.00 kg of Fe2O3 are available to react how many moles of CO are needed and how many moles of each product are formed?
mass / molar mass molar mass Fe2O3 = 159.69 g/mol mass Fe2)3 = 4.00 kg = 4000 g moles = 4000 g / 159.69 g/mol = 25.05 moles Fe2O3 The balanced equation tells you that 1 mole Fe2O3 requires 3 moles CO to react So 25.05 moles needs (3 x 25.05) moles CO = 75.15 moles Co is needed to react 4.00 kg Fe2O3 = 75.2 mol (3 sig figs) b) The equation tells you that 1 moles Fe2O3 reacts to form 2 moles Fe So 25.05 moles will form (2 x 25.05) mol Fe moles Fe formed = 50.10 moles = 50.1 mol (3 sig figs) The equation tells you 1 mole Fe2O3 reacts to form 3 moles CO2 So 25.05 mol Fe2O3 will form (3 x 25.05) mol CO2 = 75.15 moles CO2 = 75.2 mol (3 sig figs) ==
How many grams of iron oxide will be needed to react in order to form 15.0 grams of iron?
To determine the grams of iron oxide (Fe2O3) needed to produce 15.0 grams of iron (Fe), we can use stoichiometry. The balanced chemical equation for the reduction of iron(III) oxide is: Fe2O3 + 3CO → 2Fe + 3CO2. From the equation, 2 moles of Fe are produced from 1 mole of Fe2O3. The molar mass of iron is approximately 55.85 g/mol, so 15.0 g of iron corresponds to about 0.268 moles of Fe. Thus, to find the moles of Fe2O3 needed, we calculate 0.134 moles (since 0.268 moles of Fe requires half that amount of Fe2O3). The molar mass of Fe2O3 is about 159.69 g/mol, so 0.134 moles of Fe2O3 would be approximately 21.4 grams.
How many grams of Fe3O4 are required to react completey with 300 grams of H2?
The balanced chemical equation for the reaction between Fe3O4 and H2 is: Fe3O4 + 4H2 -> 3Fe + 4H2O From the equation, it can be seen that 1 mole of Fe3O4 reacts with 4 moles of H2. Calculate the moles of H2 in 300g, then use the mole ratio to find the moles of Fe3O4 needed. Finally, convert the moles of Fe3O4 to grams using its molar mass to determine the amount required.
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 -.
What mass of hydrogen chloride is require to react with 100 g of rust?
Taking rust to be Fe2O3, you would have the following reaction:Fe2O3 + 6HCl ==> 2FeCl3 + 3H2O100 g Fe2O3 x 1 mole Fe2O3/159.7 g = 0.626 moles Fe2O3moles HCl needed = 0.626 moles Fe2O3 x 6 moles HCl/mole Fe2O3 = 3.76 moles HCl neededMass HCl needed = 3.76 moles HCl x 36.5 g/mole = 137 g HCl needed
