If a container of fuel is thought to release a total of 11,000 kJ of energy into a room with a volume of 30,000 L, and all of that energy was contained as heat in the air molecules only (i.e. no heat losses anywhere), what would be the average temperature increase in °C of the air molecules. Assume that air has a constant heat capacity of 1 kJ/kg.K and an average molar mass of 28.9 g/mol. R = 0.082 L.atm/K.mol. To help the calculations, assume that the room starts at 25°C (298K) and any heating of the air does not affect the number of moles or pressure in the room (i.e., n and P are also constant).
If a container of fuel is thought to release a total of 11,000 kJ of energy into a room with a volume of 30,000 L, and all of that energy was contained as heat in the air molecules only (i.e. no heat losses anywhere), what would be the average temperature increase in °C of the air molecules. Assume that air has a constant heat capacity of 1 kJ/kg.K and an average molar mass of 28.9 g/mol. R = 0.082 L.atm/K.mol. To help the calculations, assume that the room starts at 25°C (298K) and any heating of the air does not affect the number of moles or pressure in the room (i.e., n and P are also constant).
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 87QRT
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If a container of fuel is thought to release a total of 11,000 kJ of energy into a room with a volume of 30,000 L, and all of that energy was contained as heat in the air molecules only (i.e. no heat losses anywhere), what would be the average temperature increase in °C of the air molecules.
Assume that air has a constant heat capacity of 1 kJ/kg.K and an average molar mass of 28.9 g/mol. R = 0.082 L.atm/K.mol. To help the calculations, assume that the room starts at 25°C (298K) and any heating of the air does not affect the number of moles or pressure in the room (i.e., n and P are also constant).
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