The measured melting point for each of twosamples was 89-91 °C, yet a 1:1 mixture ofthe two had a melting point of 77-83 °C.What is the explanation for these results?

Given that Two separate samples with melting points in range 89-91 °C. 1:1 mixture of these samples…

Answered: The measured melting point for each of…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 107E

See similar textbooks

Similar questions

Dry ice, CO2(s) , does not melt at atmospheric pressure. It sublimes at a temperature of 78 °C. What is the lowest pressure at which CO2(s) will melt to give CO2(l) ? At approximately what temperature will this occur? (See Figure 10.34 for the phase diagram.)
As minerals were formed from the molten magma, different ions occupied the same cites in the crystals. Lithium often occurs along with magnesium in minerals despite the difference in the charge on their ions. Suggest an explanation.
Examine the nanoscale diagrams and the phase diagram for Question 112. Match each particulate diagram (1 through 7) to its corresponding point (A through H) on the phase diagram.
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?
Associate each of the solids BN, P4S3, Pb, and CaCl2 with one of the following sets of properties. a A bluish white, lustrous solid melting at 327C; the solid is soft and malleable. b A white solid melting at 772C; the solid is an electrical nonconductor but dissolves in water to give a conducting solution. c A yellowish green solid melting at 172C. d A very hard, colorless substance melting at about 3000C.
Phase diagrams for materials that have allotropes can be more complicated than those shown in the chapter. Use the phase diagram for carbon given here to answer the following questions. (a) How many triple points are present and what phases are in equilibrium for each? (b) Is there a single point where all four phases are in equilibrium? (c) Which is more stable at high pressures, diamond or graphite? (d) Which is the stable phase of carbon at room temperature and 1 atmosphere pressure?
A 250-g sample of hard water contains 0.20gofCa(CO3). What is the hardness of the water in parts per million (ppm)? How would the water be classified?
At very low temperatures oxygen, O2, freezes and forms a crystalline solid. Which best describes these crystals? (a) ionic (b) covalent network (c) metallic (d) amorphous (e) molecular crystals
1.In what phase is the substance at 50 °C and 1 atm pressure?2.At what pressure and temperature conditions will all three phases of the substance be present?3.What is the normal melting point of the substance?4.What phase(s) will exist at 1 atm and 70 °C?
3. What is the normal melting point of the substance?4. What phase(2) will exist at 1 atm and 70 degree Celcius?
Two different pure solids are melted, and one exhibits a melting point of 138 oC, while the other exhibits a melting range of 135-147 oC. Explain the difference between the two.

Recommended textbooks for you

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

EBK A SMALL SCALE APPROACH TO ORGANIC L

Chemistry

ISBN:

9781305446021

Author:

Lampman

Publisher:

CENGAGE LEARNING - CONSIGNMENT

SEE MORE TEXTBOOKS

The measured melting point for each of two samples was 89-91 °C, yet a 1:1 mixture of the two had a melting point of 77-83 °C. What is the explanation for these results?