OSTATES OF MATTERIdentifying phase transitions on a heating curveA 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 agraph of the results:120.temperature (°C) 30.100.Explanation77°FSunny60.40.0.Use this graph to answer the following questions:What is the melting point of X ?Check10.heat added (kJ/mol)20.0°C(check all that annly)Q Search30.1/5kLDCGMia▸oloArⒸ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | AccessibilityE92/13 heat added (kJ/mol)Use this graph to answer the following questions:What is the melting point of X ?What phase (physical state) of X wouldyou expect to find in the flask after20 kJ/mol of heat has been added?Пос(check all that apply)solidliquidgasX3

Answered: Image /qna-images/answer/07656a77-b9f1-46b0-8f17-0a43cdf8b60d.jpg

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: 120. 100.- temperature (°C) 30.- 60. 40 - heat added (kJ/mol) Use this graph to answer the following questions: What is the melting point of X? 0°C (check all that annly) 4 00 Ar B

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: 120. 100.- temperature (°C) 30.- 60. 40 - heat added (kJ/mol) Use this graph to answer the following questions: What is the melting point of X? 0°C (check all that annly) 4 00 Ar B

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter6: The States Of Matter

Section: Chapter Questions

Problem 6.71E

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Similar questions

Open the PhET States of Matter Simulation (http://openstaxcollege.org/l/16phetvisual) to answer the following questions: (a) Select the Solid, Liquid, Gas tab. Explore by selecting different substances, heating and cooling the systems, and changing the state. What similarities do you notice between the four substances for each phase (solid, liquid, gas)? What differences do you notice? (b) For each substance, select each of the states and record the given temperatures. How do the given temperatures for each state correlate with the strengths of their intermolecular attractions? Explain. (c) Select the Interaction Potential tab, and use the default neon atoms. Move the Ne atom on the right and observe how the potential energy changes. Select the Total Force button, and move the Ne atom as before. When is the total force on each atom attractive and large enough to matter’? Then select the Component Forces button, and move the Ne atom. When do the attractive (van der Waals) and repulsive (electron overlap) forces balance? How does this relate to the potential energy versus the distance between atoms graph? Explain.
The amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.
The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.
Heat is added to boiling water. Explain why the temperature of the boiling water does not change. What does change?
Assume you have 1 cup of ice (237 g) at 0.0 C. Calculate how much heating is required to melt the ice, warm the resulting water to 100.0 C, and then boil the water to vapor at 100.0 C. (Hint: Do three separate calculations and then add the results.)
Using the explanation of unbalanced forces as the source of surface tension, justify why it requires energy to increase the surface area of a liquid. Is there any circumstance in which energy is given off when increasing a liquids surface area?
Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.
Some water is placed in a sealed glass container connected to a vacuum pump (a device used to pump gases from a container), and the pump is turned on. The water appears to boil and then freezes. Explain these changes using the phase diagram for water. What would happen to the ice if the vacuum pump was left on indefinitely?
Sublimation is the phase change from solid to gas without going through a liquid phase. Solid CO2, called dry ice, is an example of one substance that sublimed. Use Hesss law to show that the enthalpy of sublimation, subH, is equal to fusH vapH.
What is U when 1.00 mol of liquid water vaporizes at 100C? The heat of vaporization, Hvap, of water at 100C is 40.66 kJ/mol.
Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.
Elemental carbon has one gas phase, one liquid phase, and two different solid phases, as shown in the phase diagram: (a) On the phase diagram, label the gas and liquid regions. (b) Graphite is the most stable phase of carbon at normal conditions. On the phase diagram, label the graphite phase. (c) If graphite at normal conditions is heated to 2500 K while the pressure is increased to 1010 Pa, it is converted into diamond. Label the diamond phase. (d) Circle each triple point on the phase diagram. (e) In what phase does carbon exist at 5000 K and 108 Pa? (f) If the temperature of a sample of carbon increases from 3000 K to 5000 K at a constant pressure of 106 Pa, which phase transition occurs, if any?