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At 1 atm, how much energy is required to heat 47.0 g H₂O(s) at -24.0 °C to H₂O(g) at 167.0 °C? Use the heat transfer constants found in this table. q= kJ

At 1 atm, how much energy is required to heat 47.0 g H₂O(s) at -24.0 °C to H₂O(g) at 167.0 °C? Use the heat transfer constants found in this table. q= kJ

World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter10: Energy
Section: Chapter Questions
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At 1 atm, how much energy is required to heat 47.0 g H₂O(s) at -24.0 °C to H₂O(g) at 167.0 °C? Use the heat transfer constants found in this table. q= kJ
Transcribed Image Text:At 1 atm, how much energy is required to heat 47.0 g H₂O(s) at -24.0 °C to H₂O(g) at 167.0 °C? Use the heat transfer constants found in this table. q= kJ
A 0.532 g sample of steam at 103.5 °C is condensed into a container with 5.40 g of water at 16.0 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18, the specific heat of steam is 2.01 C, and AHvap = 40.7 kJ/mol. g. T₁ = °C
Transcribed Image Text:A 0.532 g sample of steam at 103.5 °C is condensed into a container with 5.40 g of water at 16.0 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18, the specific heat of steam is 2.01 C, and AHvap = 40.7 kJ/mol. g. T₁ = °C
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