The relationship between enthalpy and internal energy change is

Δ U = Δ H + P Δ V

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Δ H = Δ U + P Δ V

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Δ H = Δ U - P Δ V

No worries! We‘ve got your back. Try BYJU‘S free classes today!

P Δ V = Δ U + Δ H

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B $Δ H = Δ U + P Δ V$
Chemical reactions are generally carried out at constant pressure (atmospheric pressure) so it has been found useful to define a new state function Enthalpy (H) as :
$H = U + P V$ ( By definition )
$Δ H = Δ U + Δ (P V)$
$Δ H = Δ U + P Δ V$ (at constant pressure) combining with first law.
$Δ H = q_{p}$

Suggest Corrections

Similar questions

At constant pressure (∆P=0)

Than, Enthalpy

∆H=∆U+∆(PV)

∆H=∆U+P∆V+V∆P; But as (∆P=0)

∆H=∆U+P∆V

But if the Volume is constant (∆V=0)

Than the equation becomes

∆H=∆U+V∆P

What does this Equation implies and what is it's application?

Δ H

Δ H = Δ U + P Δ V

Δ H > Δ U

Δ H =

Δ U =

Join BYJU'S Learning Program