Given the following reaction:4 Fe(s) + 3 O2 (g) → 2 Fe2O3 (s) ΔH = -1648 kJ52.0 g of Fe (MM = 55.845 g/mol) are reacted as above in 1.000 x 103 g of water (MM = 18.02, ΔHFUSION = 6.01 kJ/mol, ΔHVAP = 40.65 kJ/mol, specific heat = 4.18 J/(g C) that is at 20.0 °C. What will the final temperature of the water be?

The balanced reaction taking place is given as, => 4 Fe(s) + 3 O2 (g) → 2 Fe2O3 (s)…

Answered: Given the following reaction: 4 Fe(s)…

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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Given the following reaction:

4 Fe(s) + 3 O₂ (g) → 2 Fe₂O₃ (s) ΔH = -1648 kJ

52.0 g of Fe (MM = 55.845 g/mol) are reacted as above in 1.000 x 10³ g of water (MM = 18.02, ΔH_FUSION = 6.01 kJ/mol, ΔH_VAP = 40.65 kJ/mol, specific heat = 4.18 J/(g C) that is at 20.0 °C. What will the final temperature of the water be?

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