Problem: Meals-ready-to-eat (MREs) are military meals that can be heated on a flameless heater. The heat is produced by the following reaction: Mg(s) + 2 H2O(l) → Mg(OH)2(s) + H2(g).Calculate the standard enthalpy change for this reaction.

FREE Expert Solution

We’re being asked to determine the standard enthalpy change ΔH˚rxn of the reaction. Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved


H°rxn = H°f, products - H°f, reactants


We’re given the balanced equation for the reaction: 

Mg (s) + 2 H2O (l) → Mg(OH)2 (s) + H(g)


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Problem Details

Meals-ready-to-eat (MREs) are military meals that can be heated on a flameless heater. The heat is produced by the following reaction: Mg(s) + 2 H2O(l) → Mg(OH)2(s) + H2(g).

Calculate the standard enthalpy change for this reaction.

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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 LoBue's class at GS.