Question

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?

Answer 1

Answer:The value of ΔH for this process is 2209 Joules.

Explanation:

Work done on the system by its surroundings,W =$P\Delta V$= 0.69 kJ = 690 J

Heat added or absorbed by the system,Q = 829 J

According to first law of thermodynamics:

$\Delta U=Q+W=829 J+690 J=1519 J$

The $\Delta H$ of the process is given by:

$\Delta H=\Delta U+P\Delta V=1519 J+690 J=2209 J$

The value of ΔH for this process is 2209 Joules.

Answer 2

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.