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To calculate the mass of aluminum (Al) needed to completely react with 135 g of iron, you first need to determine the molar ratio between them from the balanced chemical equation. The balanced equation for the reaction between aluminum and iron is 2Al + 3Fe2O3 -> 3Fe + Al2O3. From this ratio, you can calculate that 2 moles of aluminum (Al) react with 3 moles of iron (Fe). Next, calculate the molar mass of aluminum (Al) and use it to convert the given mass of iron to moles. Finally, use the molar ratio to find the mass of aluminum needed.
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What substances in damp air that are needed for the iron to react?
In damp air, the primary substances needed for iron to react are moisture (water vapor) and oxygen. The presence of water facilitates the formation of electrolytic solutions, which can accelerate the oxidation process of iron. This leads to corrosion, commonly seen as rust (iron oxide), when iron reacts with both oxygen and water. Additionally, impurities in the air, such as salt or pollutants, can further enhance this reaction.
Does iron reacts with water?
Pure Iron (Fe) doesn't directly react with water, but it will oxidize (rust), especially if the iron is just wet and is exposed to air a lot. I believe iron will eventually oxidize if kept completely underwater too, but as there is less free Oxygen for it to react with down there, it is a longer process.
What mass of iron must react to produce 3600 kJ of energy?
To determine the mass of iron required to produce 3600 kJ of energy, we need to know the specific reaction and its enthalpy change (ΔH). For example, in the reaction of iron with oxygen to form iron oxide (rust), the ΔH value would be essential. If we assume an example ΔH of -800 kJ/mol for the formation of iron oxide, then we can calculate that approximately 4.5 moles of iron would be needed to produce 3600 kJ of energy, which corresponds to about 252 grams of iron (using iron's molar mass of 55.85 g/mol).
What reacts with iron oxide to get a product of pure iron?
You can react Aluminum to react with Ironoxide to get Iron. Iron(II)oxide + Aluminum --> Aluminumoxide + Iron Fe2O3 + 2Al --> Al2O3 + 2Fe
Does carbon react with steel?
Carbon react with iron forming carbides in steel.
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.
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.
How many atoms of iron are needed to completely react with three molecules of oxygen?
Two atoms of iron are needed to completely react with three molecules of oxygen to form two molecules of iron(III) oxide (Fe2O3). Each iron atom will lose three electrons to form Fe3+ ions, while each oxygen molecule will gain two electrons to form O2- ions.
What mass of iron is needed to react with 16 grams of sulfur?
iron forms iron sulphide when reacts with sulphur, Fe + S = FeS in this reaction 32 g of sulphur require 56 g of iron so 16 g sulphur requires 28 g of iron.
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 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 grams of iron iii hydroxide will react with 85g or sodium chloride?
The iron(III) hydroxide is not soluble in water and doesn't react with sodium chloride.
How many millimeters of a 2 Molar solution of hydrochloric acid are needed to completely react with 75 grams of iron sulfide?
FeS + 2HCl >> FeCl2 + H2S 75 grams FeS (1mole FeS/87.92 grams)(2 mole HCl/1 mole FeS) = 1.71 moles HCl 2 Molar HCl = 1.71 moles HCl/Liters = 0.855 Liters HCl, or as asked for; 855 milliliters of hydrochloric acid needed
How much iron is required to react with 48.0 grams of sulfur in the reaction 2Fe plus 3S yields Fe2S3?
Based on the balanced chemical equation 2Fe + 3S -> Fe2S3, the molar ratio of Fe to S is 2:3. First, convert the 48.0 grams of sulfur to moles, then use the molar ratio to find the moles of iron needed. Finally, convert the moles of iron to grams to determine the required amount of iron.
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.
An iron ore sample is found to be 35.00 percent Fe by mass How many grams of ore is needed to obtain 454.0 grams of Fe?
To calculate this, you first need to determine the mass of pure iron in 454.0 grams. This is done by multiplying 454.0 grams by 0.35 (the decimal equivalent of 35.00%). This gives 158.9 grams of pure iron. To find out how many grams of ore is needed, you need to set up the equation 0.35 * Mass of ore = 158.9 grams, which gives you 454 grams of ore needed.
How many grams of iron II sulfide have to react with hydrochloric acid to generate 12 g of hydrogen sulfide?
To calculate the grams of iron II sulfide needed, we start by finding the moles of hydrogen sulfide produced. This is done by dividing the given mass of hydrogen sulfide by its molar mass. Then, we use the balanced chemical equation to determine that for every 4 moles of hydrogen sulfide, 1 mole of iron II sulfide is needed. From this, we find the grams of iron II sulfide required by multiplying the moles of iron II sulfide by its molar mass.
