Question

Lighters are usually fueled by butane (C4H10). When 1 mole of butane burns at constant pressure, it produces 2658 kJ of heat and does 3 kJ of work.​
Part A
What are the values of ΔH and ΔE for the combustion of one mole of butane?
Part B
Express your answer using four significant figures.

Answer 1

Answer:

see explanation below

Explanation:

This is actually something that you can solve using the following expression:

ΔH = q + PΔV

ΔE = q + W

As the exercise states that the butane is burned at constant pressure, we can assume that P = 0, therefore:

ΔH = q

According to this, ΔH = q = 2658 kJ. However, as it's produced in the reaction, this value is negative, so ΔH = -2658 kJ

To get ΔE:

ΔE = 2658 + 3 = 2661 kJ

But as before, this is produced in the reaction, so this value is also negative

ΔE = -2661 kJ