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Difference between Internal Energy and Enthalpy

Question

For the gaseous reaction : $N_{2} O_{4} ⟶ 2 N O_{2}$
$Δ H > Δ U$
$Δ H < Δ U$
$Δ H = Δ U$
$Δ H = 0$

A

Δ H > Δ U

B

Δ H = 0

C

Δ H < Δ U

D

Δ H = Δ U

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Solution

Verified by Toppr

$Δ H = Δ U + Δ n R T$
$Δ n = n_{P} - n_{R} = 2 - 1 = 1$
$∴ Δ H = Δ U + (1) R T$
$∴ Δ H > Δ U$

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Similar Questions

Q1

N_{2} O_{4} ⟶ 2 N O_{2}

For this reaction relate

Δ H

and

Δ U

.

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Q2

For which reaction,

Δ H > Δ U

? (

Δ H =

change in enthalpy,

Δ U =

change in internal energy )

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Q3

For gaseous reactions, if

Δ H

is the change in enthalpy and

Δ U

that in internal energy, then

Δ H

is always greater than

Δ U

.
If true 1 else 0.

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Q4

For the reaction, N₂ + 3H₂ ⇌ 2NH₃, ∆H= …………….

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Q5

Assertion :In the following reaction:

C (s) + O_{2} (g) ⟶ C O_{2} (g); Δ H = Δ U - R T

Reason:

Δ H

is related to

Δ U

by the equation,

Δ H = Δ U - n_{g} R T

View Solution