Question 24Shown below is the heating curve (q vs. T) for some substance.(3)D20-heat added (kl/ml)melting pointenthalpy of fusion-35. "C5.00 kJ/mol2.90 g/cm³ (solid)boiling pointenthalpy ofvaporizationdensity25. "C30.00 kJ/mol28. J-K mel (sold)2.20 g/ml. (quid)heat capacity56. JK mel30. JK mel (liquid)(vapor)Which value was used to determine line segment AB?O 5.00 kJ/mol30.00 kJ/mol28 J K¹ mol¹30 J K¹¹ mol-156 J K¹ mol¹

For line segment AB, since it is before the melting point of the substance, which is 35∘ C, the only…

Answered: Question 24 Shown below is the heating…

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

Similar questions

Carbon disulfide, CS 2, has a heat of vaporization of 29,200 J/mol. The normal boiling point* of CS 2 is 317K What is the vapor pressure at 268K? (* BP at 760 mm Hg)
4. Calculate the amount of energy absorbed when 5g ice @ 0°C melts to water at 0°C. Did a phase change occur? If so, which one? Is this endothermic or exothermic?
The enthalpy change for converting 10.0 g of ice at -50.0 °C to water at 50.0 °C is ________ kJ. The specific heats of ice, water, and steam are 2.09 J-g/K, 4.18 J-g/K, and 1.84 J-g/K respectively. For H 2O, ΔH fus = 6.01 kJ/mol, and ΔH_vap= 40.67 KJ/mol.
Calculate the amount of heat needed to change 45.0 grams of ice at -25.0 °C to steam at 250.0 °C. (For water, ΔHfus = 333 J/g; ΔHvap = 2260 J/g; Specific Heat (ice) = 2.10 J g-1 K-1; Specific Heat (steam) = 2.00 J g-1 K-1) a. 14.7 kJ b. 33.7 kJ c.116 kJ d.152 kJ e. 175 kJ
How much heat is released at constant pressure if a 15.0-L tank containing 47.0 atm of hydrogen sulfide gas condenses at its boiling point of -60.0°C? The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0°C. (R= 0.0821 L• atm/(K • mol)) O 7.54 x 10° J O 2.68 x 10° J O 1.87x 10* J O 4.64x 10² J O 1.31 x 10² J
13) Ethanol melts at -114 C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of evaporation is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 and 2.3 J/gK, respectively. How much heat is required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C?
What quantity of heat (in KJ) would be required to convert 11.1 g of ice to water 0.00 C ? (Hfus=6.01 KJ/ mol for water)
Determine the amount of heat, in kJ, required to heat 19 g of solid Ca at 125 C to 851C (still solid). Melting Point = 851C Boiling Point = 1487C Molar Heat Capacities: Csolid = 26.2 J/mol C C liquid = 31.0 J/molC AH_fusion = 9.33 kJ/mol AH_vaporization = 162 kJ/mol
Calculate the heat required to convert 25.0 g solid ethanol at -135.0 C to liquid at 72.0 C. Specific heat of solid ethanol 0.97 J/g C. Specific heat liquid ethanol 2.3JL %3D AH of ethanol 4.9 kJ/mol %3D AH of ethanol = 38.56 kJ/mol %3D Heating Curve of Ethanol 1.843 78 72C 3856) mol 2.3 414 493 Temperature (*C)
What amount of heat (in kJ) is required to convert 10.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･ °C; specific heat capacity of liquid = 1.58 J/g･ °C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3 °C)
What amount of heat (in kJ) is required to convert 17.2 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)
The latent heat of fusion and vaporization of water is 333.6 J/g and 2256.7 J/g respectively at the normal melting and boiling point. Cp=4.19 Jg-1K-1 for liquid water, density=0.917 g/cm3 for ice at 1 atm and 0 oC, density=1.000 g/cm3 and 0.958g/cm3 for water at 1 atm and 100 0C respectively. For liquid water, Cp varies slightly with T. The value given is an average over the range 0 oC and 100 oC respectively. Calculate work for the melting for 1 mol of ice at 0 oC and 1 atm.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

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

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

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

SEE MORE TEXTBOOKS