# 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)

83% (438 ratings) ###### 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?

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