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 824J of heat from its surroundings and has 0.62kJ of P−V work done on it by its surroundings. What is the value of ΔH for this process? What is the value of ΔE for this process?

qp = delta H

Work done by the surroundings on the system is +
dE = q+w.

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 827 J of heat from its surroundings and has 0.62 kJ of P−V work done on it by its surroundings.

To find the values of ΔH and ΔE for this process, we need to understand their definitions and how they relate to heat and work.

1. ΔH (change in enthalpy):
ΔH represents the change in enthalpy, which is a measure of the heat absorbed or released in a reaction at constant pressure. It is given by the equation:
ΔH = q + PΔV
where q is the heat absorbed or released and PΔV is the work done on or by the system.

2. ΔE (change in internal energy):
ΔE represents the change in internal energy, which is the sum of the kinetic and potential energies of the particles in the system. It is given by the equation:
ΔE = q + w
where q is the heat absorbed or released and w is the work done on or by the system.

In this case, the gas undergoes a chemical reaction and absorbs 824J of heat from its surroundings. Also, 0.62kJ of P−V work is done on the gas.

To find the value of ΔH, we can substitute the given values into the equation:
ΔH = q + PΔV
= 824J + 0.62kJ (remember to convert kJ to J, 1 kJ = 1000 J)
= 824J + 620J
= 1444J

Therefore, the value of ΔH for this process is 1444J.

To find the value of ΔE, we can substitute the given values into the equation:
ΔE = q + w
= 824J + 0.62kJ
= 824J + 620J
= 1444J

Therefore, the value of ΔE for this process is 1444J.

Hence, both ΔH and ΔE in this process have the same value, which is 1444J.