Ethanol (C₂H5OH) melts at -114 °C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g-K), respectively. Part A How much heat is required to convert 47.5 g of ethanol at 23 °C to the vapor phase at 78 °C? Express your answer in kilojoules to three significant figures. ■V ΑΣΦ ↑ ? kJ Q= Submit Previous Answers Request Answer X Incorrect; Try Again; 8 attempts remaining The entered value corresponds to the heat required to convert liquid ethanol into the vapor pl °C. The amount of heat needed to raise the temperature of a substance is the product of the Part B How much heat is required to convert 47.5 g of ethanol at -160 °C to the vapor phase at 78 °C? Express your answer in kilojoules to two significant figures. IΫΠ| ΑΣΦ + Ò ? Request Answer Q= Submit kJ
Ethanol (C₂H5OH) melts at -114 °C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g-K), respectively. Part A How much heat is required to convert 47.5 g of ethanol at 23 °C to the vapor phase at 78 °C? Express your answer in kilojoules to three significant figures. ■V ΑΣΦ ↑ ? kJ Q= Submit Previous Answers Request Answer X Incorrect; Try Again; 8 attempts remaining The entered value corresponds to the heat required to convert liquid ethanol into the vapor pl °C. The amount of heat needed to raise the temperature of a substance is the product of the Part B How much heat is required to convert 47.5 g of ethanol at -160 °C to the vapor phase at 78 °C? Express your answer in kilojoules to two significant figures. IΫΠ| ΑΣΦ + Ò ? Request Answer Q= Submit kJ
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...
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The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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Transcribed Image Text:Ethanol (C₂H5OH) melts at -114 °C and boils at 78 °C. The enthalpy of fusion of ethanol is
5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and
liquid ethanol are 0.97 and 2.3 J/(g-K), respectively.
Part A
How much heat is required to convert 47.5 g of ethanol at 23 °C to the vapor phase at 78 °C?
Express your answer in kilojoules to three significant figures.
■V ΑΣΦ ↑
?
kJ
Q=
Submit
Previous Answers Request Answer
X Incorrect; Try Again; 8 attempts remaining
The entered value corresponds to the heat required to convert liquid ethanol into the vapor pl
°C. The amount of heat needed to raise the temperature of a substance is the product of the
Part B
How much heat is required to convert 47.5 g of ethanol at -160 °C to the vapor phase at 78 °C?
Express your answer in kilojoules to two significant figures.
IΫΠ| ΑΣΦ
+
Ò
?
Request Answer
Q=
Submit
kJ
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