If 17.3g of powdered aluminium are allowed to react with axcess Fe2O3 Fe2O3 how much heat is produced by this reaction
2Al(s) + Fe2O3(s) --> 2Fe (s) + Al2O3 (s). First, you need to look up on the web to find delta H for this reaction. If you can't find it, you can calculate it from the following:
dHo formation of reaction = (n*dHo formation of products) - (n*dHo formation of reactants)
You can find dHo formation values in tables from your text or on the web. I will call dHo formation of reaction = B
Then B x (17.3 g/2*atomic mass Al in g) = your answer.
Post your work if you get stuck.
-273kJ/gC°
To determine the amount of heat produced by the reaction between powdered aluminum and excess Fe2O3, we need to calculate the heat of the reaction using the balanced chemical equation and the enthalpy of formation values for the compounds involved. Here are the step-by-step calculations:
Step 1: Write the balanced chemical equation for the reaction between aluminum (Al) and iron(III) oxide (Fe2O3):
2Al + Fe2O3 -> Al2O3 + 2Fe
Step 2: Determine the molar mass of aluminum (Al) and iron(III) oxide (Fe2O3):
Molar mass of Al = 26.98 g/mol
Molar mass of Fe2O3 = (2 * Molar mass of Fe) + (3 * Molar mass of O)
= (2 * 55.85 g/mol) + (3 * 16.00 g/mol)
= 55.85 g/mol + 48.00 g/mol
= 103.85 g/mol
Step 3: Convert the given mass of aluminum (17.3 g) to moles:
Number of moles = Given mass / Molar mass
= 17.3 g / 26.98 g/mol
≈ 0.641 moles
Step 4: Determine the limiting reactant (the reactant that is completely consumed) by comparing the moles of aluminum to the stoichiometric ratio of the balanced equation:
Using the balanced equation, we see that 2 moles of aluminum react with 1 mole of Fe2O3.
Therefore, 0.641 moles of aluminum would react with (0.641 / 2) moles of Fe2O3.
As the Fe2O3 is present in excess, it won't be fully consumed, so aluminum is the limiting reactant.
Step 5: Calculate the heat of the reaction using the enthalpy of formation values for the compounds involved:
Given enthalpy of formation values:
ΔHf[Al2O3] = -1676 kJ/mol
ΔHf[Fe] = 0 kJ/mol
The balanced equation tells us that 2 moles of aluminum react, so we multiply ΔHf[Al2O3] by 2:
ΔHreaction = 2 * ΔHf[Al2O3]
= 2 * -1676 kJ/mol
= -3352 kJ
Step 6: Calculate the heat produced by the reaction using the moles of aluminum:
Heat produced by the reaction = ΔHreaction * moles of aluminum
= -3352 kJ * 0.641
≈ -2148.53 kJ
Therefore, the heat produced by the reaction between 17.3 g of powdered aluminum and excess Fe2O3 is approximately -2148.53 kJ. The negative sign indicates that the reaction is exothermic, meaning it releases heat.
To determine the amount of heat produced by the reaction between powdered aluminum (Al) and excess iron(III) oxide (Fe2O3), we need to first calculate the limiting reactant. The limiting reactant is the one that will be completely consumed during the reaction and determines the maximum amount of product formed.
1. Calculate the number of moles of each reactant:
- Mass of aluminum (Al): 17.3 g
- Molar mass of aluminum (Al): 26.98 g/mol
Number of moles of Al = Mass of Al / Molar mass of Al
Substituting the values: Number of moles of Al = 17.3 g / 26.98 g/mol
2. Determine the stoichiometric ratio of the reactants based on the balanced equation between aluminum and iron(III) oxide:
2Al + Fe2O3 → Al2O3 + 2Fe
From the equation, we can see that 2 moles of aluminum react with 1 mole of iron(III) oxide.
3. Calculate the number of moles of iron(III) oxide:
Number of moles of Fe2O3 = Number of moles of Al / Stoichiometric ratio
Substituting the values: Number of moles of Fe2O3 = (17.3 g / 26.98 g/mol) / (2 mol Al / 1 mol Fe2O3)
4. Determine the mass of iron(III) oxide:
Mass of Fe2O3 = Number of moles of Fe2O3 x Molar mass of Fe2O3
To calculate the molar mass of iron(III) oxide (Fe2O3), you need to look up the atomic masses of iron (Fe) and oxygen (O) from the periodic table.
5. Calculate the amount of heat produced using the molar mass values and the balanced equation:
Based on the balanced equation 2Al + Fe2O3 → Al2O3 + 2Fe, the stoichiometry tells us that 1 mole of aluminum reacts with 2 moles of iron to produce a certain amount of heat (which you can typically find in a reference table). Note that the reaction is exothermic, so it releases heat.
If you have the heat of reaction value, you can multiply it by the number of moles of iron(III) oxide to find the amount of heat produced.
Now you have the step-by-step process to calculate the amount of heat produced by the reaction between aluminum and iron(III) oxide. Remember to gather all the necessary data, such as molar masses and the heat of reaction value, to complete the calculation accurately.