Problem: When 1 mol of a fuel is burned at constant pressure, it produces 3453 kJ of heat and does 12 kJ of work. What is the value of ΔH for the combustion of the fuel?

FREE Expert Solution

$\overline{){\mathbf{∆}}{\mathbf{E}}{\mathbf{=}}{\mathbf{q}}{\mathbf{+}}{\mathbf{w}}}$

ΔE = internal energy, J
q = heat, J
w = work, J

For heat, q:

+ q → if the system gains, takes in, or absorbs heat or energy
– q → if the system loses, evolves, gives off, or releases heat or energy

For work, w:

+ w → work is done on the system by the surroundings (volume: compresses)
– w → work is done by the system on the surroundings (volume: expands)

Problem Details

When 1 mol of a fuel is burned at constant pressure, it produces 3453 kJ of heat and does 12 kJ of work. What is the value of ΔH for the combustion of the fuel?