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

E=q+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)

View Complete Written Solution
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?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Internal Energy concept. You can view video lessons to learn Internal Energy. Or if you need more Internal Energy practice, you can also practice Internal Energy practice problems.