The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called "Heater Meals." Just pour water into the heater unit, wait a few minutes, and you have a hot meal. The source of energy in the heater is Mg(s) + 2 H₂O(l) → Mg(OH)2 (s) + H₂(g) Calculate the enthalpy change under standard conditions, in joules, for this reaction. What quantity of magnesium is needed to supply the energy required to warm 45 mL of water (d = 1.00 g/mL) from 20. °C to 95 °C? The specific heat capacity of water is 4.184 J/g °C. A, H* (kJ/mol) Compound Mg(OH)2 (s) H₂O(l) -924.54 -285.83 AFER MEALD The "heater meal" uses the reaction of magnesium with water as a source of energy as heat. Enthalpy change = J/mol-rxn g Mg

The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called "Heater Meals." Just pour water into the heater unit, wait a few minutes, and you have a hot meal. The source of energy in the heater is Mg(s) + 2 H₂O(l) → Mg(OH)2 (s) + H₂(g) Calculate the enthalpy change under standard conditions, in joules, for this reaction. What quantity of magnesium is needed to supply the energy required to warm 45 mL of water (d = 1.00 g/mL) from 20. °C to 95 °C? The specific heat capacity of water is 4.184 J/g °C. A, H* (kJ/mol) Compound Mg(OH)2 (s) H₂O(l) -924.54 -285.83 AFER MEALD The "heater meal" uses the reaction of magnesium with water as a source of energy as heat. Enthalpy change = J/mol-rxn g Mg

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called "Heater Meals." Just pour water into the
heater unit, wait a few minutes, and you have a hot meal. The source of energy in the heater is
Mg(s) + 2 H₂O(l) → Mg(OH)2 (s) + H₂(g)
Calculate the enthalpy change under standard conditions, in joules, for this reaction. What quantity of magnesium is needed to supply the energy required to warm 45
mL of water (d = 1.00 g/mL) from 20. °C to 95 °C? The specific heat capacity of water is 4.184 J/g · °C.
Af HⓇ (kJ/mol)
Compound
Mg(OH)2 (s)
H₂O(l)
-924.54
-285.83
MEATER MEALS
The "heater meal" uses the reaction of magnesium with water as a source of energy as heat.
Enthalpy change =
J/mol-rxn
g Mg

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