Problem: How much energy is evolved during the reaction of 51.2 g of Al, according to the reaction below?Assume that there is excess Fe2O3.Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)          ΔH°rxn = -852 kJ A) 51.2 kJ B) 448 kJ C) 224 kJ D) 1617 kJ E) 808 kJ

FREE Expert Solution

Use the balanced equation and provided mass of Al to find the energy released 

Recall that the provided Δ°H will account for 2 moles of Al from the balanced equation

Calculating the energy from mass of Al (Al is 26.98 g/mol)

97% (335 ratings)
View Complete Written Solution
Problem Details

How much energy is evolved during the reaction of 51.2 g of Al, according to the reaction below?

Assume that there is excess Fe2O3.

Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)          ΔH°rxn = -852 kJ 

A) 51.2 kJ 

B) 448 kJ 

C) 224 kJ 

D) 1617 kJ 

E) 808 kJ

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equation concept. You can view video lessons to learn Thermochemical Equation. Or if you need more Thermochemical Equation practice, you can also practice Thermochemical Equation practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofHow much energy is evolved during the reaction of 51.2 g of ...as medium difficulty.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Arnett's class at FAMU.