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

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 66E: Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL...

See similar textbooks

Related questions

Question

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?

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions