🤓 Based on our data, we think this question is relevant for Professor Capps' class at American Public University System.
Step 1: Balanced equation for the reaction
Iron (Fe) reacts with oxygen (O2) to form the product Fe2O3.
Mn(s) + O2(g) → Mn3O4(s)
We can balance this equation by adding 3 to Mn and 2 to O2.
3 Mn(s) + 3 O2(g) → Mn3O4(s)
Step 2: Heat released by the chemical reaction
We will consider these facts when solving this problem:
1387 kJ of heat is released when 1 mol of Mn3O4 is formed.
The amount of heat is:
How many kilojoules of heat will be released when exactly 1 mole of manganese, Mn, is burned to form Mn3O4(s) at standard state conditions?
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 Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.
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Based on our data, we think this problem is relevant for Professor Capps' class at American Public University System.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.