When 1 mol of a fuel is burned at constant pressure it produces 3453 kj of heat and does 12 kj of work?

Answer 1

I'm guessing you need (answer wise) ΔH and ΔE

To solve for ΔE, you need to add -(3453+12)/ 1mol = -3465kJ (it's negative due to the fact that you're producing heat)

To solve for ΔH, you need to multiply -3454 by the pressure (in this case, it's assumed we're at standard pressure) so: -3453*1= -3453kJ

Hope that helps :)

Answer 2

its 1 mol of fuel, and 3450 kj and 11kj of work. Please answer!!

Answer 3

-3465