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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 iron oxide are produced from 8.00 mol of iron?
The balanced chemical equation for the formation of iron oxide is: 4 Fe + 3 O2 -> 2 Fe2O3. From the equation, we see that 4 moles of iron are required to produce 2 moles of iron oxide. Therefore, with 8.00 mol of iron, we can produce 4.00 mol of iron oxide. To find the mass of iron oxide produced, we multiply the moles of Fe2O3 by its molar mass, which is approximately 159.7 g/mol. This gives us 4.00 mol x 159.7 g/mol = 638.8 grams of iron oxide produced.
How many grams of Fe2O3 are formed when 16.7g of Fe reacts completely with oxygen?
The rusting of iron has the reaction 4 Fe + 3 O2 equals 2 Fe2O3. So every 2 moles of iron produces 1 moles of iron oxide. 16.7 grams is .299 moles of iron. This means there are 0.149 moles of iron oxide or 23.88 grams.
What is the chemical equation when iron oxide reacts with hydrogen chloride?
The chemical equation for the reaction between iron oxide (Fe2O3) and hydrogen chloride (HCl) is: Fe2O3 + 6HCl → 2FeCl3 + 3H2O. In this reaction, iron oxide is converted to iron(III) chloride and water is produced as a byproduct.
In the following reaction how grams of iron will be produced from 0.750 moles of aluminum2Al s Fe2O3 s 2Fe l Al2O3 s?
55.8 * 0.750 = 41.85
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.
What is produced when iron reacts with water?
Iron oxide is produced.The chemical reaction is given as 2Fe+3H20=Fe2O3+3H2
How many grams of iron oxide are produced from 8.00 mol of iron?
The balanced chemical equation for the formation of iron oxide is: 4 Fe + 3 O2 -> 2 Fe2O3. From the equation, we see that 4 moles of iron are required to produce 2 moles of iron oxide. Therefore, with 8.00 mol of iron, we can produce 4.00 mol of iron oxide. To find the mass of iron oxide produced, we multiply the moles of Fe2O3 by its molar mass, which is approximately 159.7 g/mol. This gives us 4.00 mol x 159.7 g/mol = 638.8 grams of iron oxide produced.
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 grams of Fe2O3 are formed when 16.7g of Fe reacts completely with oxygen?
The rusting of iron has the reaction 4 Fe + 3 O2 equals 2 Fe2O3. So every 2 moles of iron produces 1 moles of iron oxide. 16.7 grams is .299 moles of iron. This means there are 0.149 moles of iron oxide or 23.88 grams.
What mass of iron can be obtained from 3.80 g iron oxide reacting with excess carbon monoxide?
1,25
What is the chemical equation when iron oxide reacts with hydrogen chloride?
The chemical equation for the reaction between iron oxide (Fe2O3) and hydrogen chloride (HCl) is: Fe2O3 + 6HCl → 2FeCl3 + 3H2O. In this reaction, iron oxide is converted to iron(III) chloride and water is produced as a byproduct.
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.
What chemicals are produced when Iron oxide and sulphuric acid are mixed?
When iron oxide and sulfuric acid are mixed, iron sulfate and water are produced. The chemical reaction can be represented as Fe2O3 + H2SO4 → Fe2(SO4)3 + H2O.
Is Fe2O3 a combination reaction?
No, Fe2O3 is not a combination reaction. It is actually the chemical formula for iron(III) oxide, which is a compound composed of iron and oxygen atoms. In a combination reaction, two or more reactants combine to form a single product.
