A 0.617 mol sample of Xe(g) initially at 298 K and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 14.9 K. Assuming ideal gas behavior, calculate the amount of heat (?)in joules required to affect this temperature change and the total change in internal energy, Δ?. Note that some books use Δ? as the symbol for internal energy instead of Δ?. Type of gas Molar heat capacity at constant volume (??,?) atoms (3/2)? linear molecules (5/2)? nonlinear molecules 3? where ? is the ideal gas constant
A 0.617 mol sample of Xe(g) initially at 298 K and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 14.9 K. Assuming ideal gas behavior, calculate the amount of heat (?)in joules required to affect this temperature change and the total change in internal energy, Δ?. Note that some books use Δ? as the symbol for internal energy instead of Δ?. Type of gas Molar heat capacity at constant volume (??,?) atoms (3/2)? linear molecules (5/2)? nonlinear molecules 3? where ? is the ideal gas constant
Physics for Scientists and Engineers: Foundations and Connections
1st Edition
ISBN:9781133939146
Author:Katz, Debora M.
Publisher:Katz, Debora M.
Chapter21: Heat And The First Law Of Thermodynamics
Section: Chapter Questions
Problem 50PQ
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A 0.617 mol sample of Xe(g) initially at 298 K and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 14.9 K.
Assuming ideal gas behavior, calculate the amount of heat (?)in joules required to affect this temperature change and the total change in internal energy, Δ?. Note that some books use Δ? as the symbol for internal energy instead of Δ?.
Type of gas | Molar heat capacity at constant volume (??,?) |
---|---|
atoms | (3/2)? |
linear molecules | (5/2)? |
nonlinear molecules | 3? |
where ? is the ideal gas constant |
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