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The reaction is:
4 Fe + 3 O2 = 2 Fe2O3
The answer is 319,38 g.
Wiki User
∙ 8y ago
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.
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How many grams of iron will be needed to react completely with an excess of oxygen to form 40 grams of iron3 oxide?
To determine the amount of iron needed to react with 40 grams of iron(III) oxide, you should use the stoichiometry of the reaction. Calculate the molar mass of iron(III) oxide (Fe2O3) and determine the molar ratio between iron and iron(III) oxide in the balanced chemical equation. From there, you can calculate the amount of iron needed to fully react with 40 grams of iron(III) oxide.
A 55 g sample of iron reacts with 24 g of oxygen to form how many grams of iron oxide?
Iron oxide is formed by the reaction of iron and oxygen in a 1:1 ratio by mass. Therefore, the 55 g of iron will react completely with 55 g of oxygen to form iron oxide.
How many elements in iron oxide?
Iron oxide has two main chemical compounds: iron(II) oxide (FeO) and iron(III) oxide (Fe2O3). Both compounds consist of two elements - iron and oxygen.
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.
What type of reaction produces iron?
Iron is typically produced through a chemical reduction reaction of iron ore (Fe2O3) with carbon in a blast furnace, resulting in the production of metallic iron. This reaction is a form of chemical reduction, where iron oxide is reduced to elemental iron by the carbon monoxide produced in the furnace.
How many grams of iron will be needed to react completely with an excess of oxygen to form 40 grams of iron3 oxide?
To determine the amount of iron needed to react with 40 grams of iron(III) oxide, you should use the stoichiometry of the reaction. Calculate the molar mass of iron(III) oxide (Fe2O3) and determine the molar ratio between iron and iron(III) oxide in the balanced chemical equation. From there, you can calculate the amount of iron needed to fully react with 40 grams of iron(III) oxide.
A 55 g sample of iron reacts with 24 g of oxygen to form how many grams of iron oxide?
Iron oxide is formed by the reaction of iron and oxygen in a 1:1 ratio by mass. Therefore, the 55 g of iron will react completely with 55 g of oxygen to form iron oxide.
How many atoms of iron rusted that weight 63.8 grams?
To find the number of atoms in 63.8 grams of rust (iron oxide), you need to first determine the molar mass of iron oxide (Fe2O3), which is 159.7 g/mol. Next, calculate the number of moles in 63.8 grams by dividing the weight by the molar mass. Then use Avogadro's number (6.022 x 10^23) to convert moles to atoms.
Sodium oxide and water react to produce sodium hydroxide. How many grams of sodium hydroxide is produced from 120.0g of sodium oxide?
155.2 g
How many grams of water will be produced if 32.0 g of nitrous oxide are also produced in the reaction?
To find the mass of water produced, we first need to determine the molar ratio of water to nitrous oxide in the reaction. Once we have the mole ratio, we can use it to calculate the moles of water produced from the moles of nitrous oxide. Finally, we can convert the moles of water to grams using the molar mass of water.
How many grams of iron can be obtained from a 268g sample of iron 3 oxide?
To find the amount of iron in iron (III) oxide, we first need to calculate the molar mass of Fe2O3. The molar mass of Fe2O3 is 159.69 g/mol. By looking at the ratio of atoms in Fe2O3, we see that 2 moles of Fe are present in 1 mole of Fe2O3. By applying this ratio, we can find that 2 moles of Fe correspond to 159.69g, so 1 mole will be 79.85g. Next, we can calculate the amount of Fe in 268g of Fe2O3. By using stoichiometry, we determine that 1 mol of Fe is equal to 55.85 g. Multiplying this by the number of moles of Fe (79.85g/55.85g) present in the 268g sample of Fe2O3, we get that approximately 115g of Fe can be obtained from the 268g sample of Fe2O3.
How many grams of ammonia are consumed in the reaction of 75.0g lead (II) oxide?
The complete question: Lead (II) oxide reacts with ammonia forming solid lead nitrogen gas and liquid water. 1.)How many grams of ammonia are consumed in the reaction of 75.0g lead (II) oxide? 2.) If 56.4g of lead are produced how many grams of nitrogen are also formed?
How many elements in iron oxide?
Iron oxide has two main chemical compounds: iron(II) oxide (FeO) and iron(III) oxide (Fe2O3). Both compounds consist of two elements - iron and oxygen.
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 molecules of iron are there in iron oxide?
One molecule of iron oxide (Fe2O3) contains two iron atoms per molecule. So, for every molecule of iron oxide, there are two iron atoms, which means one iron oxide molecule contains two iron atoms.
What type of reaction produces iron?
Iron is typically produced through a chemical reduction reaction of iron ore (Fe2O3) with carbon in a blast furnace, resulting in the production of metallic iron. This reaction is a form of chemical reduction, where iron oxide is reduced to elemental iron by the carbon monoxide produced in the furnace.
How many grams of Aluminium oxide will be produced from the complete reaction of 1.87 L of oxygen gas at 793.0 mm Hg and 28.0 Celsius degree?
To find the grams of aluminum oxide produced, we need to first calculate the moles of oxygen gas using the ideal gas law. Then, we use the balanced chemical equation to determine the moles of aluminum oxide produced. Finally, we convert moles to grams using the molar mass of aluminum oxide. Be sure to adjust the conditions of the gases to standard temperature and pressure for accurate calculations.
