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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?

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Lanuel

The value of enthalpy change (ΔH) for this process is 139 Joules

Given the following data:

  • Energy absorbed, Q = 829 Joules.
  • P-V work = 0.69kJ  to J = [tex]0.69 \times 1000[/tex] = 690 Joules.

To determine the value of enthalpy change (ΔH) for this process, we would apply the First Law of Thermodynamics:

What is the First Law of Thermodynamics?

Mathematically, the the First Law of Thermodynamics is given by this formula:

[tex]\Delta H = Q - W[/tex]

Where;

  • [tex]\Delta H[/tex] is the enthalpy change or change in internal energy.
  • Q is the quantity of heat absorbed.
  • W is the work done.

Substituting the parameters into the formula, we have;

[tex]\Delta H = 829 - 690\\\\\Delta H = 139[/tex]

Enthalpy change (ΔH) = 139 Joules.

Read more on enthalpy change here: https://brainly.com/question/11628413

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