Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the following reaction: 4Fe(s) +302(g) →2Fe2O3(s) Standard thermodynamic quantities for selected substances at 25 °C Reactant or product Fe(s) O₂(g) Fe₂O3(s) AH (kJ/mol) 0.0 0.0 -824.2 You may want to reference (Pages 392-398) Section 9.10 while completing this problem. ▼ The product has the only nonzero heat of formation, so it is the only value needed to calculate the enthalpy of this reaction. Normally, you would w to express the enthalpy of a reaction with respect to one mole of a chemical species, whether it is a reactant or product. However, since the balan chemical equation contains only coefficients greater than 1, you should consider how the enthalpy relates to one mole of each substance accordin to the coefficients. In other words, -1648.4 kJ of heat is released when 4 mol of Fe reacts with 3 mol of O₂ to produce 2 mol of Fe₂O3. Part B Calculate how much heat (in kilojoules) a hand warmer containing 10.0 g of iron powder produces Express the energy in kilojoules to three significant figures. 195] ΑΣΦΑΦ q= Submit Request Answer 4 ? kJ
Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the following reaction: 4Fe(s) +302(g) →2Fe2O3(s) Standard thermodynamic quantities for selected substances at 25 °C Reactant or product Fe(s) O₂(g) Fe₂O3(s) AH (kJ/mol) 0.0 0.0 -824.2 You may want to reference (Pages 392-398) Section 9.10 while completing this problem. ▼ The product has the only nonzero heat of formation, so it is the only value needed to calculate the enthalpy of this reaction. Normally, you would w to express the enthalpy of a reaction with respect to one mole of a chemical species, whether it is a reactant or product. However, since the balan chemical equation contains only coefficients greater than 1, you should consider how the enthalpy relates to one mole of each substance accordin to the coefficients. In other words, -1648.4 kJ of heat is released when 4 mol of Fe reacts with 3 mol of O₂ to produce 2 mol of Fe₂O3. Part B Calculate how much heat (in kilojoules) a hand warmer containing 10.0 g of iron powder produces Express the energy in kilojoules to three significant figures. 195] ΑΣΦΑΦ q= Submit Request Answer 4 ? kJ
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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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
Transcribed Image Text:Dry chemical hand warmers utilize the oxidation of iron to form iron
oxide according to the following reaction:
4Fe(s) +302(g) →2Fe2O3(s)
Standard thermodynamic quantities for selected substances
at 25 °C
Reactant or
product
Fe(s)
O₂(g)
Fe₂O3(s)
AH (kJ/mol)
0.0
0.0
-824.2
You may want to reference (Pages 392-398) Section 9.10 while
completing this problem.
▼
The product has the only nonzero heat of formation, so it is the only value needed to calculate the enthalpy of this reaction. Normally, you would w
to express the enthalpy of a reaction with respect to one mole of a chemical species, whether it is a reactant or product. However, since the balanc
chemical equation contains only coefficients greater than 1, you should consider how the enthalpy relates to one mole of each substance accordin
to the coefficients. In other words, -1648.4 kJ of heat is released when 4 mol of Fe reacts with 3 mol of O₂ to produce 2 mol of Fe₂O3.
Part B
Calculate how much heat (in kilojoules) a hand warmer containing 10.0 g of iron powder produces.
Express the energy in kilojoules to three significant figures.
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