Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Calculate the amount of energy necessary to raise the temperature of
1 L of ethanol (d=0.7849 g/mL) from 25 to 78.3 degrees Celsius.
Specific heat=2.44 j/K and heat of vaporization is 38.56 j/g.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 3 steps with 3 images
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
- Benzene is used primarily as a solvent in the chemical and pharmaceutical industries. The molecular formula of benzene is C6H6. The melting point and boiling point of benzene are 278.61 K and 353.2 K, respectively. The enthalpy of vaporization of benzene is 30.8 kJ/mol and the enthalpy of fusion of benzene is 10.59 kJ/mol. When 47.56 gram of benzene changes from solid to liquid at 278.61 K, how many kJ of heat is needed? __________ kJarrow_forwardThe heat of vaporization for CH4 is 152 cal/g. How much heat is needed (in calories) to vaporize 0.4 moles of CH4?arrow_forwardIf the heat of fusion for water is 80. cal/g, how many calories are needed to melt 4.65 g of ice at 0 °C? Treat the heat of fusion as an exact value.arrow_forward
- When 4.61 grams of ice at - 20°C have absorbed 2500 calories of heat, what is the temperature of the resulting water? specific heat of ice = 0.50 cal/g°c specific heat of water = 1.0 cal/g °C latent heat of fusion = 80 cal /garrow_forwardWater has a vaporization enthalpy of 2256 J/g, making it the largest of any molecular substance. For example, methane, CH4, has nearly the same molar mass, but its vaporization enthalpy is only 185 J/g. What explanation can be offered for this?arrow_forwardhow many joules of heat are required to heat 25.0 g of ethyl alcohol from the prevailing room temperature, 22.5 oC , to its boiling point, 78.5oC?arrow_forward
- The following information is given for silver at 1atm: boiling point = 2212 °C melting point = 961 °C specific heat solid= 0.238 J/g °C specific heat liquid 0.285 J/g °C = KJ AHvap(2212 °C) = 254 kJ/mol AHfus (961 °C) = 12.0 kJ/mol What is AH in kJ for the process of freezing a 32.4 g sample of liquid silver at its normal melting point of 961 °C. |arrow_forwardUsing the heat of vaporization of benzene, 395 J/g, calculate the grams of benzene that will condense at its boiling point if 9.28 kJ is removed.arrow_forward5. The heat of vaporization of an organic solvent is 39.8 kJ/mol. Find the temperature in degrees Celsius at which the solvent boils on a day in a ski resort when the barometric pressure is 0.749 atm. The normal boiling point of the liquid is 73.2°C (R = 8.314 J/K mol).)arrow_forward
- If it requires 70.4 kJ of heat to boil 1.60 moles of water, what is its enthalpy of vaporization?arrow_forwardWhat amount of heat (in kJ) is required to convert 26.6 g of an unknown solid (MM = 92.14 g/mol) at -115.0 °C to a liquid at 32.3 °C? (specific heat capacity of solid = 1.06 J/g °C; specific heat capacity of liquid = 1.71 J/g. °C; AHfus = 6.61 kJ/mol; normal freezing point, Tf = -95.0 °C)arrow_forwardWhat amount of heat (in kJ) is required to convert 11.9 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g °C; specific heat capacity of gas = 0.932 J/g °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3°C) %3D %3Darrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY