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

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

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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