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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:Temperature (°C)
125
100
75
50
25
0
-25
BC
Ice
D
Water vapor.
Liquid water and vapor
(vaporization)
Liquid water
Ice and liquid water (melting)
F
E
A
Heat added (each division corresponds to 4 kJ)

Transcribed Image Text:Sample Exercise 10.3 Calculating AH for Temperature and Phase Changes
Calculate the total enthalpy change upon converting 1.00 mol of ice at -25 °C to water
vapor (steam) at 125 °C under a constant pressure of 1 atm. The specific heats of ice,
water, and steam are 2.03 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H₂O, AHfus
= 6.01 kJ/mol and Ahvap
40.67 kJ/mol.
Format for AB, CD, or EF:
=
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- 2 attempts left Check my work Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.611 mol of gaseous ethanol at 300.0°C and atm to liquid ethanol at 25.0°C and 1 atm: b.p. at 1 atm: 78.5°C AH" : 40.5 kJ/mol vap Cgas 1.43 J/g °C Cliquid: 2.45 J/g °Carrow_forward14. Calculate how many Joules of energy would be required to change 32.9 g of water at 35°C to steam at 120°C. You will need to break this problem into four steps. a) Find the Joules needed to heat the water to the boiling point. (8938.9 J) b) Find the Joules needed to vaporize the water. (74,354 J) c) Find the Joules needed to heat the vapor (steam) from the boiling point to 120°C. (1329 J) d) Add your answers to steps a, b, and c. (84,622 J)arrow_forwardLearning Two 20.0 g ice cubes at -18.0 °C are placed into 255 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H, O(s) 37.7 J/ (mol-K) heat capacity of H, O(1) 75.3 J/ (mol-K) Tf = °C enthalpy of fusion of H, O 6.01 kJ/molarrow_forward
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