Laboratory Techniques in Organic Chemistry
4th Edition
ISBN: 9781464134227
Author: Jerry R. Mohrig, David Alberg, Gretchen Hofmeister, Paul F. Schatz, Christina Noring Hammond
Publisher: W. H. Freeman
expand_more
expand_more
format_list_bulleted
Question
Chapter 6, Problem 3Q
Interpretation Introduction
Interpretation:
The reason to never add boiling stones to the hot liquid should be determined. Also, the process that is followed when you forget to add boiling stones should be determined.
Concept introduction:
Boiling stones is a chemically inert compound of carbon and silicon. It isunevenly shaped piece of substances that consist of sharp edges and air pockets. They help in the formation of bubbles and prevent the violent eruption of a heated liquid as it starts to boil.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
What is formed when gas is enclosed in a chamber then liquified under very high pressure? *
What latent heat value signifies the lost of heat during a phase change?
What is the unique temperature and pressure at which the three phases of a substance are in equilibrium with each other? *
Which liquid crystal is of pharmaceutical significance? *
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?
What should you do if you begin to heat a liquid and see that you have forgotten to add a boiling stone?
Chapter 6 Solutions
Laboratory Techniques in Organic Chemistry
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?arrow_forwardYou are camping and contemplating placing some hot objects into your sleeping bag to warm it. You warm a rock and a canteen of water, of roughly equal mass, around the fire. Which would be more effective in warming your sleeping bag? Why?arrow_forwardEnthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?arrow_forward
- How much heat is evolved when 1255 g of water condensesto a liquid at 100°C?arrow_forwardAre changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forwardIf 100. J of heat energy is applied to a 25-g sample of mercury, by how many degrees will the temperature of the sample of mercury increase? (See Table 10.1.)arrow_forward
- Define the joule in terms of SI base units.arrow_forward3. Is solid > liquid → gas an endothermic or exothermic process? Describe how this energy change affects the energy of the molecules and their intermolecular forces.arrow_forward1. Why do solids and liquids behave differently? 2. How do heat and work affect a system?arrow_forward
- What is true about the specific heat of ice and water? * the same since they are essentially made up of same molecules. water has twice the specific heat of ice. ice has higher specific heat because it is colder. It depends on the initial temperature of ice. none of the above.arrow_forwardIn the above image, you have a solid at less than 0 oC. As you add heat (Q), the temperature of the solid increases until it hits a point when it would start melting. In the case of water, this is at 0 oC. Notice that at this point the temperature stops rising and we have a mixture of solid/liquid. We are still adding heat but the temperature is not changing. Once all of our solid becomes liquid, the temperature starts to rise again until it hits another plateau, at 100 oC. This is the point where the water boils and starts becoming a gas. Again, we add heat but the liquid/gas mixtures temperature does not change. Once all the liquid has become gas, the temperature will start to rise again. Is it possible to have 0 oC water and 0 oC ice? Yes or No?arrow_forwardThirty grams of silicon at 80.0°C is added to 70.0mL of water at 20.0°C. Calculate the final temperature after the two substances are mixed together. The specific heat of water is 4.184J/g°C and the specific heat of silicon is 0.7121 J/g°C.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- World of ChemistryChemistryISBN:9780618562763Author:Steven S. ZumdahlPublisher:Houghton Mifflin College DivChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher: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
World of Chemistry
Chemistry
ISBN:9780618562763
Author:Steven S. Zumdahl
Publisher:Houghton Mifflin College Div
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY