Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change q=m. Cs AT where Cs is specific heat and m is mass. Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase change q= n·ΔΗ where, n is the number of moles and AH is the enthalpy of fusion, vaporization, or sublimation. The following table provides the specific heat and enthalpy changes for water and ice. Substance Specific heat (Jg-¹ °C-¹) Part A water ice ΔΗ = 35.1 kJ Submit Calculate the enthalpy change, AH, for the process in which 14.2 g of water is converted from liquid at 17.4 °C to vapour at 25.0 °C. For water, Avap H = 44.0 kJ mol-¹ at 25.0 °C and Cs = 4.18 Jg-¹ °C-¹ for H₂O(1). -1 Express your answer to three significant figures and include the appropriate units. View Available Hint(s) Part B 4.18 2.01 Previous Answers ✓ Correct The enthalpy change is positive because heat is being transferred from the surroundings into the system. ΔΗ (kJ mol-¹) 44.0 6.01 How many grams of ice at -22.6 °C can be completely converted to liquid at 20.6 °C if the available heat for this process is 4.54x103 kJ ? For ice, use a specific heat of 2.01 Jg-1°C-1 and Afus H=6.01kJ mol-¹. Express your answer to three significant figures and include the appropriate units
Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change q=m. Cs AT where Cs is specific heat and m is mass. Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase change q= n·ΔΗ where, n is the number of moles and AH is the enthalpy of fusion, vaporization, or sublimation. The following table provides the specific heat and enthalpy changes for water and ice. Substance Specific heat (Jg-¹ °C-¹) Part A water ice ΔΗ = 35.1 kJ Submit Calculate the enthalpy change, AH, for the process in which 14.2 g of water is converted from liquid at 17.4 °C to vapour at 25.0 °C. For water, Avap H = 44.0 kJ mol-¹ at 25.0 °C and Cs = 4.18 Jg-¹ °C-¹ for H₂O(1). -1 Express your answer to three significant figures and include the appropriate units. View Available Hint(s) Part B 4.18 2.01 Previous Answers ✓ Correct The enthalpy change is positive because heat is being transferred from the surroundings into the system. ΔΗ (kJ mol-¹) 44.0 6.01 How many grams of ice at -22.6 °C can be completely converted to liquid at 20.6 °C if the available heat for this process is 4.54x103 kJ ? For ice, use a specific heat of 2.01 Jg-1°C-1 and Afus H=6.01kJ mol-¹. Express your answer to three significant figures and include the appropriate units
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Question
Transcribed Image Text:Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change
q=m.C, AT
where C's is specific heat and m is mass.
Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase change
q = n·ΔΗ
where, n is the number of moles and AH is the enthalpy of fusion, vaporization, or sublimation.
The following table provides the specific heat and enthalpy changes for water and ice.
Specific heat
Substance
-1 o
(J g−¹ °℃−¹)
Part A
ΔΗ = 35.1 kJ
Submit
water
ice
Part B
Calculate the enthalpy change, AH, for the process in which 14.2 g of water is converted from liquid at 17.4 °C to vapour at 25.0 °C.
For water, AvapH = 44.0 kJ mol-¹ at 25.0 °C and Cs = 4.18 J -1
g °C-¹ for H₂O(1).
Express your answer to three significant figures and include the appropriate units.
► View Available Hint(s)
0
Previous Answers
Correct
The enthalpy change is positive because heat is being transferred from the surroundings into the system.
Submit
μÅ
5.22 104
How many grams of ice at -22.6 °C can be completely converted to liquid at 20.6 °C if the available heat for this process is 4.54×10³ kJ ?
For ice, use a specific heat of 2.01 J g-1 °C-1 and Afus H = 6.01kJ mol-¹.
Express your answer to three significant figures and include the appropriate units.
►View Available Hint(s)
g
.
4.18
2.01
Previous Answers
?
X Incorrect; Try Again; 3 attempts remaining
ΔΗ
(kJ mol-¹)
44.0
6.01
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