||| = OSTATES OF MATTER Identifying phase transitions on a heating curve 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 graph of the results: 150. temperature (°C) 110. 130. Explanation 81°F Partly sunny 90. 70. What is the boiling point of X ? 0. Use this graph to answer the following questions: Check 10. 20. 30. heat added (kJ/mol) °C 40. (check all that annly) - -- Q Search 50 0/5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce 四 LDLOO

||| = OSTATES OF MATTER Identifying phase transitions on a heating curve 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 graph of the results: 150. temperature (°C) 110. 130. Explanation 81°F Partly sunny 90. 70. What is the boiling point of X ? 0. Use this graph to answer the following questions: Check 10. 20. 30. heat added (kJ/mol) °C 40. (check all that annly) - -- Q Search 50 0/5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce 四 LDLOO

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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Use the phase diagram of Substance X below to find the melting point of X when the pressure above the solid is 7.0 atm. بالا pressure (atm) solid []c 200 liquid 400 X gas temperature (K) Note: your answer must be within 25 °C of the exact answer to be graded correct. 600
[References) Use the References to access important values if needed for this question. Refer to the following phase diagram (not to scale!) for xenon: 57.6 1.00 atm 0.37 152.0 161.3 165.0 289.7 T Kelvin A sample of xenon at a pressure of 0.370 atm and a temperature of 140 K is compressed at constant temperature to a pressure of 66.5 atm. Which of the following are true? Choose all that apply | The sample is initially a gas. O No phase change will occur. O The solid initially present will vaporize. O The final state of the substance is a solid. Previous O The sample is initially a solid. En rch
The vapor pressure of Substance X is measured at several temperatures: temperature vapor pressure -98. °C 0.0231 atm -85. °C 0.0964 atm -72. °C 0.334atm Use this information to calculate the enthalpy of vaporization of X. Round your answer to 2 significant digits. Be sure your answer contains a correct unit symbol. x10
Try Again Your answer is incorrect. The enthalpy of vaporization of Substance X is 23.0 Round your answer to 2 significant digits. 0.32 atm x10 X kJ and its normal boiling point is 10. °C. Calculate the vapor pressure of Xat - 18. °C. mol S
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Refer to the following phase diagram (not to scale!) for sulfur dioxide: P atm 78 1.00 0.0017 197.6 200.4 Choose all that apply T Kelvin A sample of sulfur dioxide at a pressure of 1.70×10-3 atm and a temperature of 266 K is compressed at constant temperature to a pressure of 83.7 atm. Which of the following are true? 263.1 430.7 The sample is initially a gas. The liquid initially present will vaporize. The final state of the substance is a liquid. The sample is initially a solid. One or more phase changes will occur.
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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5. Refer to the phase diagram of water below: Pressure, atm 1.0 В 0.006 A 0.61 Temperature, °C
- Suppose a small sample of pure X is held at -182. °C and 0.8 atm. What will be the state of the sample (solid, liquid, or gas)? - Suppose the temperature is held constant at -182. °C but the pressure is increased by 0.3 atm. What will happen to the sample (nothing, it will melt, it will freeze, it will boil, it will condense, it will sublime, or it will deposit)? - Suppose, on the other hand, the pressure is held constant at 0.8 atm but the temperature is increased by 178.°C. What will happen to the sample (nothing, it will melt, it will freeze, it will boil, it will condense, it will sublime, or it will deposit)? This all part of one question
Calculate the change in the boiling point of NH3, at the normal boiling point (239.82 K at 1 bar), per pascal change in the atmospheric pressure. The molar heat of vaporization of ammonia at the normal boiling point is 23.33 kj/mol. The molar volume of liquid ammonia is 0.02495 L/mol and the molar volume of ammonia gas at the boiling point is 19.8 L/mol
Why does the temperature of a substance stay constant during a phase change such as vaporization? Sketch the heating curve for water to help illustrate your answer.