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). Do not include commas, scientific notation, spaces, or the units of °C in the answer.
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).
Do not include commas, scientific notation, spaces, or the units of °C in the answer.
AI-generated content may present inaccurate or offensive content that does not represent bartleby’s views.
Unlock instant AI solutions
Tap the button
to generate a solution
