A quantity of 505 J of heat are added to 11.3 g of water at 28.3 °C. What is thefinal temperature of water? ( specific heat of water = 4.18 J/g.0C ).Choose...Choose...-37.639.0A balloon of helium gas lost 36.4 k) of heat while it was raising up, simultaneously,the helium gas expanded from 64.0L to 80.0 L against 563 mmHg pressure.Calculate the change in the internal energy (AU) of helium gas ( in kJ). Giventhat ( atm.L = 101.3 J)268-238.7-48.25188.711.8510.7

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A quantity of 505 J of heat are added to 11.3 g of water at 28.3 °C. What is the final temperature of water? ( specific heat of water = 4.18 J/g.ºC ).

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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Question

A quantity of 505 J of heat are added to 11.3 g of water at 28.3 °C. What is the
final temperature of water? ( specific heat of water = 4.18 J/g.0C ).
Choose...
Choose...
-37.6
39.0
A balloon of helium gas lost 36.4 k) of heat while it was raising up, simultaneously,
the helium gas expanded from 64.0L to 80.0 L against 563 mmHg pressure.
Calculate the change in the internal energy (AU) of helium gas ( in kJ). Given
that ( atm.L = 101.3 J)
268
-238.7
-48.25
188.7
11.85
10.7

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