Heat is added to 1.0 mol of an ideal gas at a constant pressure of 1.0 atm, and the volume increases from 2.0 L to 4.0 L. What is the temperature change for this process? +48.8 K +24.4 K +12.2 K What is the work w for this process? –202 J –405 J –304 J What is ΔE for this process? \ ΔE = 3/2 nRΔT = 3/2 Δ(PV) +51 J +304 J +101 J What is the heat, ΔH, for this process? +304 J +507 J +405 J
Heat is added to 1.0 mol of an ideal gas at a constant pressure of 1.0 atm, and the volume increases from 2.0 L to 4.0 L. What is the temperature change for this process? +48.8 K +24.4 K +12.2 K What is the work w for this process? –202 J –405 J –304 J What is ΔE for this process? \ ΔE = 3/2 nRΔT = 3/2 Δ(PV) +51 J +304 J +101 J What is the heat, ΔH, for this process? +304 J +507 J +405 J
Chapter3: The First Law Of Thermodynamics
Section: Chapter Questions
Problem 79AP: Consider the process shown below. During steps AB and BC, 3600 J and 2400 J of heat, respectively,...
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Question
Heat is added to 1.0 mol of an ideal gas at a constant pressure of 1.0 atm, and the volume increases from 2.0 L to 4.0 L.
What is the temperature change for this process?
|
+48.8 K |
|
+24.4 K |
|
+12.2 K |
What is the work w for this process?
|
–202 J |
|
–405 J |
|
–304 J |
What is ΔE for this process? \
ΔE = 3/2 nRΔT = 3/2 Δ(PV)
|
+51 J |
|
+304 J |
|
+101 J |
What is the heat, ΔH, for this process?
|
+304 J |
|
+507 J |
|
+405 J |
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