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13 Dec 2019

What are the relationships between change in internal energy, ΔU, heat, work and change in enthalpy, ΔH? You may wish to use a graph to illustrate your explanation.

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Tod Thiel
Tod ThielLv2
17 Dec 2019

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Related questions

Consider 1.50 mol of a monoatomic ideal gas (Cv,m = 3/2R) thatis initially at 390.K (taken as 3 significant figures) and 2.20 atmpressure. For this system, calculate the change in entropy (ΔS),the change in internal energy (ΔU), and the change in enthalpy (ΔH)for a reversible adiabatic expansion of this gas to a finalpressure of 1.10 atm. Also calculate the final temperature (T) andvolume (V).

What is the change in internal energy of the system (ΔU) if 50 kJ of heat energy is released What is the change in internal energy of the system   (ΔU)  if   50 kJ   of heat energy is released

by the system and 40 kJ of work is done by the system for a certain process?by the system and   40 kJ   of work is done by the system for a certain process?

Select one:

a.
−90 kJ−90 kJ

b.
+90 kJ+90 kJ

c.
10 kJ10 kJ

d.
+10 kJ

Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change

q=m⋠Cs⋠ΔT

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⋠ΔH

where, n is the number of moles and ΔH 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
[J/(g⋠∘C)]		 ΔH
(kJ/mol)
water 4.18 44.0
ice 2.01 6.01

Part A

Calculate the enthalpy change, ΔH, for the process in which 45.7 g of water is converted from liquid at 10.1 ∘C to vapor at 25.0 ∘C .

For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and Cs = 4.18 J/(g⋠∘C) for H2O(l).

Part B

How many grams of ice at -12.5 ∘C can be completely converted to liquid at 8.1 ∘C if the available heat for this process is 5.27×103 kJ ?

For ice, use a specific heat of 2.01 J/(g⋠∘C) and ΔHfus=6.01kJ/mol.

Express your answer to three significant figures and include the appropriate units.

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