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A 1095 g piece of iron initially at 1371 °C is submerged in 1000.0 g of water initially at 20.0 °C. The temperature of the water increases, and some of the water evaporates. At thermal equilibrium, the final temperature of the iron, water, and water vapor (steam) is 100.0 °C. How many moles of water evaporated to reach thermal equilibrium?

A 1095 g piece of iron initially at 1371 °C is submerged in 1000.0 g of water initially at 20.0 °C. The temperature of the water increases, and some of the water evaporates. At thermal equilibrium, the final temperature of the iron, water, and water vapor (steam) is 100.0 °C. How many moles of water evaporated to reach thermal equilibrium?

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter7: Chemical Energy
Section: Chapter Questions
Problem 62E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...
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A 1095 g piece of iron initially at 1371 °C is submerged in 1000.0 g of water initially at 20.0 °C. The temperature of the water increases, and some of the water evaporates. At thermal equilibrium, the final temperature of the iron, water, and water vapor (steam) is 100.0 °C. How many moles of water evaporated to reach thermal equilibrium? The specific heat capacity of iron is Cs, Fe = 0.449 J /g.°C The specific heat capacity of liquid water is Cs, water = 4.18 J/g.°C The enthalpy of vaporization of water is AHvap :40.7 kJ/mol Circle your answer on the written template. Be sure that it is in the correct units (mol) and has the correct number of significant figures.
Transcribed Image Text:A 1095 g piece of iron initially at 1371 °C is submerged in 1000.0 g of water initially at 20.0 °C. The temperature of the water increases, and some of the water evaporates. At thermal equilibrium, the final temperature of the iron, water, and water vapor (steam) is 100.0 °C. How many moles of water evaporated to reach thermal equilibrium? The specific heat capacity of iron is Cs, Fe = 0.449 J /g.°C The specific heat capacity of liquid water is Cs, water = 4.18 J/g.°C The enthalpy of vaporization of water is AHvap :40.7 kJ/mol Circle your answer on the written template. Be sure that it is in the correct units (mol) and has the correct number of significant figures.
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