Final answer:
The amount of heat absorbed/released during the process is 351,237.6 J. This is equivalent to 83,873.3 calories. The system is an open system, and the reaction is exothermic. If the pan material is changed to tin, the heat absorbed/released would decrease.
Step-by-step explanation:
To calculate the amount of heat absorbed/released during the process, we can use the equation Q = mcΔT. In this case, the mass of the aluminum pan (m) is 3040 grams, the specific heat of aluminum (c) is 0.897 J/g°C, and the change in temperature (ΔT) is 150°C - 20°C = 130°C. Plugging these values into the equation, we get Q = (3040 g)(0.897 J/g°C)(130°C) = 351,237.6 J.
To convert the heat in joules to calories, we can use the conversion factor 1 calorie = 4.184 J. Therefore, Q in calories is 351,237.6 J / 4.184 J/cal = 83,873.3 calories.
The type of system in this case is an open system because matter (gas) is entering and leaving the system during the burning process.
This is an exothermic reaction because heat is being released from the burning gas and transferred to the aluminum pan.
If the pan material is changed to tin, the specific heat for tin (c) is 0.214 J/g°C. Using the same mass (3040 g) and change in temperature (130°C), we can calculate the heat absorbed/released by the tin pan using the equation Q = mcΔT: Q = (3040 g)(0.214 J/g°C)(130°C) = 102,972.8 J. Therefore, changing the pan material to tin would decrease the amount of heat absorbed/released during the process.