Two 20.0 g ice cubes at -13.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T₁, of the water after all the ice melts. heat capacity of H,O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol 45.1 Incorrect

Two 20.0 g ice cubes at -13.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T₁, of the water after all the ice melts. heat capacity of H,O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol 45.1 Incorrect

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter3: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 66P: One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of...

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One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of 2.000 atm when it is slowly heated. If the temperature of the gas rises by 10.00 K and 400.0 J of heat are added in the process, what is its final volume?
An ideal gas initially at 300 K undergoes an isobaric expansion at 2.50 kPa. If the volume increases from 1.00 m3 to 3.00 m3 and 12.5 kJ is transferred to the gas by heat, what are (a) the change in its internal energy and (b) its final temperature?
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