Review Quiz IIIName: is ultinLab Section:1. (4.0 points) Rank the following in order of increasing boiling points by considering themost important intermolecular forces and give your reason:NH3, H₂O, Ne, and CO2. (4.0 points) A beaker contains 350.0 g of warm water at 98.0 °C. A piece of metal at 5.90°C is placed in the beaker. The final temperature of the system reaches 67.0 °C.Determine the mass of the metal if its specific heat is 0.298 J/g °C. The specific heat ofwater is 4.184 J/g °C.m. 0.29465192.61. E-350g - 4.184 513-31°Cm. 18,20785= 45396.4 I142078718.20785m=2493, 24,Ch3. (4.0 points) Without any detailed calculation consider the following equations andpredict the sign of AS.a. N2(g) + 3H2 (g) → 2NH3 (g)b. 2H2(g) + O2 (g) → 2H2O (1)c. CH4 (g) +202 (g) → CO2 (g) + 2H2O (1)d. 2N2 (g) +502 (g) → 2N20s (g)

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Answered: Review Quiz III Name: is ultin Lab…

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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How much heat would be required to convert 5.31 mol of a pure substance from a liquid at 40.0°C to a gas at 113.0°C?
Use the following values to answer each part. The specifi c heat of water is 1.00 cal/(g · °C); the heat of fusion of water is 79.7 cal/g; and the heat of vaporization of water is 540 cal/g. a. How much energy (in calories) is needed to melt 45 g of ice at 0.0 °C and warm it to 55 °C? b. How much energy (in calories) is released when 45 g of water at 55 °C is cooled to 0.0 °C, and frozen to solid ice at 0.0 °C? c. How much energy (in kilocalories) is released when 35 g of steam at 100. °C is condensed to water, the water is cooled to 0.0 °C, and the water is frozen to solid ice at 0.0 °C?
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How much energy (in kJ) is released when 275 g of water (H2O) is formed according to the following chemical equation? C3H8 + 5O2 → 3CO2 + 4H2O ΔH = -2200 kJ **Energy is released so record your answer as a negative number.
A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a graph of the results: 110. 90. 70. temperature (°C) 50. 30. 10. 0. 10. 20. 30. 40. 50. 60. heat added (kJ/mol) Use this graph to answer the following questions: What is the boiling point of X ? (check all that apply) O solid What phase (physical state) of X would you expect to find in the flask after 13 kJ/mol of heat has been added? O liquid O gas ?
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7. Which diagram below best represents the heating curve for ethanol? Physical Data for Ethanol A) C) E) B) Temperature (°C) Temperature (°C) 150 100 Temperature (°C) 50 0 150 100 0 50 0 -50 -100 -150 -50 -100 -150 150 100 50 0 -50 -100 -150 Tmp = -114.14 °C = 78.24 °C Tbp AHfus = 4.9 kJ/mol AHvap = 38.56 kJ/mol Heat added- -Heat added- -Heat added- Cliquid ethanol Csolid ethanol Cgaseous ethanol on D) Temperature (°C) = 111.5 J/mol C = 112.4 J/mol C = 78.28 J/mol C 150 100 50 Temperature (°C) 0 -50 -100 -150 150 100 50 0 -50 -100 -150 -Heat added-> -Heat added-> 8. 1026 kJ of heat is added to a sample of water at 1 atm pressure and the temperature rises from 40 °C to 80 °C. If 1026 kJ more heat is added, what will the final temperature of the water be? A) 120 °C because the water will continue to heat up at the same rate. B) More than 100 °C but less than 120 °C because some of the heat will be used to boil the water.

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