A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in the following figure. When the gas undergoes a particular chemical reaction, it absorbs 829J of heat from its surroundings and has 0.69kJ of P-V work done on it by its surroundings. What is the value of ΔH for this process?

Question

Celia Ramos

Physics

20 April, 22:06

A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in the following figure. When the gas undergoes a particular chemical reaction, it absorbs 829J of heat from its surroundings and has 0.69kJ of P-V work done on it by its surroundings. What is the value of ΔH for this process?

+4

Answers (1)

Know the Answer?

Jason · Answer 1

From the first law of thermodynamics, we use the equation expressed as:

ΔH = Q + W

where Q is the heat absorbed of the system and W is the work done.

We calculate as follows:

ΔH = Q + W

ΔH = 829 J + 690 J = 1519 J

Hope this answers the question. Have a nice day.