Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Mercury, with a freezing point of -38.8°C, is the only metal that is liquid at room temperature. How much heat energy (in joules) must be released by mercury if 1.60 mL of the metal is cooled from room temperature (23.0°C) to -38.8°C and then frozen to a solid? (The density of mercury is 13.6 g/cm. Its specific heat is 0.140 J/g*K and its heat of fusion is 11.4 3/g.)

Mercury, with a freezing point of -38.8°C, is the only metal that is liquid at room temperature. How much heat energy (in joules) must be released by mercury if 1.60 mL of the metal is cooled from room temperature (23.0°C) to -38.8°C and then frozen to a solid? (The density of mercury is 13.6 g/cm. Its specific heat is 0.140 J/g*K and its heat of fusion is 11.4 3/g.)

Chemistry
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...
See similar textbooks
icon
Related questions
Question

I need help with these 3 heating and cooling curve  word problems. Will you please send work? You might have to enlarge the picture.

Mercury, with a freezing point of -38.8°C, is the only metal that is liquid at room temperature. How much heat energy (in joules) must be released by mercury if1.60 mL of the metal is cooled from roorm temperature (23.0°C) to -38.8°C and then frozen to a solid? (The density of mercury is 13.6 g/cm. Its specific heat is 0.140 J/g•K and its heat of fusion is 11.4 1/g.) Chloromethane, CH CI, is used as a topical anesthetic. The temperature at which CH3CI liquid turns into a vapor (the boiling point) is -24.09°C. What quantity of heat must be absorbed by the liquid to convert 170. g of liquid to a vapor at -24.09°C? The heat of vaporization of CH Cl is 21.40 kJ/mol. kJ MEK Ethanol, CH5OH, boils at 78.29°C. How much heat energy (in kilojoules) is required to heat 1.40 kg of this liquid from 23.0°C to the boiling polnt and then change the liquid completely to a vapor at that temperature? (The specific heat of liquid ethanol is 2.44 J/g-K and its enthalpy of vaporization is 38.56 kJ/mol.) kJ Submit Answer
Transcribed Image Text:Mercury, with a freezing point of -38.8°C, is the only metal that is liquid at room temperature. How much heat energy (in joules) must be released by mercury if1.60 mL of the metal is cooled from roorm temperature (23.0°C) to -38.8°C and then frozen to a solid? (The density of mercury is 13.6 g/cm. Its specific heat is 0.140 J/g•K and its heat of fusion is 11.4 1/g.) Chloromethane, CH CI, is used as a topical anesthetic. The temperature at which CH3CI liquid turns into a vapor (the boiling point) is -24.09°C. What quantity of heat must be absorbed by the liquid to convert 170. g of liquid to a vapor at -24.09°C? The heat of vaporization of CH Cl is 21.40 kJ/mol. kJ MEK Ethanol, CH5OH, boils at 78.29°C. How much heat energy (in kilojoules) is required to heat 1.40 kg of this liquid from 23.0°C to the boiling polnt and then change the liquid completely to a vapor at that temperature? (The specific heat of liquid ethanol is 2.44 J/g-K and its enthalpy of vaporization is 38.56 kJ/mol.) kJ Submit Answer
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Quality Assurance and Calibration Methods
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
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS