1.)The internal energy of a system increases 253 J , while the system loses 93 J of heat. Determine the sign and the magnitude of work involved in this change. Show units! 2.)Consider the following thermochemical equation:Fe2O3 (s) + 2 Al (s) --> 2 Fe (s) + Al2O3 (s) ∆H = –1704 kJDetermine the heat evolved, in kJ, when 23.3 g Al is consumed in this reaction. Show units! 3.)Calculate the heat needed, in joules, to raise the temperature of 32 g iron, Fe, from 25oC to 93oC. (specific heat capacity of iron is 0.450 J/goC). Show units.

Internal energy (∆E) :- It is the energy of a thermodynamic system which is present in that…

Answered: 1.) The internal energy of a system…

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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1.)

The internal energy of a system increases 253 J , while the system loses 93 J of heat. Determine the sign and the magnitude of work involved in this change. Show units!

2.)

Consider the following thermochemical equation:

Fe₂O₃ (s) + 2 Al (s) --> 2 Fe (s) + Al₂O₃ (s) ∆H = –1704 kJ

Determine the heat evolved, in kJ, when 23.3 g Al is consumed in this reaction. Show units!

3.)

Calculate the heat needed, in joules, to raise the temperature of 32 g iron, Fe, from 25^oC to 93^oC. (specific heat capacity of iron is 0.450 J/g^oC). Show units.

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