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Standard XII

Chemistry

First Law of Thermodynamics

A vessel cont...

Question

A vessel contains 100 litres of a liquid $x$ . Heat is supplied to the liquid in such a fashion that, Heat given = change in enthalpy. The volume of the liquid increases by 2 litres. If the external pressure is one atm, and 202.6 Joules of heat were supplied then, [ U - total internal energy ]

∆U = 0, ∆H = 0

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∆U = + 202.6 J, ∆H = + 202.6 J

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∆U = - 202.6 J, ∆H = - 202.6 J

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∆U = 0, ∆H = + 202.6 J

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Solution

The correct option is D
∆U = 0, ∆H = + 202.6 J

$Δ H$ = heat gives so process is isobaric.

$w = - P_{n e x t} (Δ V) = - 1 \times 2 l i t r e . a t m = - 202.6 J$ -as one litre.atm=101.33 joules

Hence $q = 202.6 J = Δ H$ and $Δ E = q + w = 0$

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Similar questions

Q. A vessel contains

100

litres of a liquid X. Heat is supplied to the liquid at a constant pressure of

1

atm in such a fashion that heat given is equal to the change in enthalpy of the system. The volume of the liquid increases by

2

litres. If

202.6

joules of heat were supplied, then the values of

△ U

and

△ H

would have been:

[△ U = change in internal energy, △ H change in enthalpy]

Q. A vessel contains

100

litres of a liquid X. Heat is supplied to the liquid at a constant pressure of

1

atm in such a fashion that heat given= change in enthalpy. The volume of the liquid increases by

2

litres. If

202.6

joules of heat were supplied, then

[Δ U, Δ H = change in internal energy and enthalpy

is:

Q. A vessel contains 100 litres of a liquid x. Heat is supplied to the liquid in such a fashion that, Heat given = change in enthalpy. The volume of the liquid increases by 2 litres. If the external pressure is one atm, and 202.6 Joules of heat were supplied then, [

U \to

total internal energy]:-

Q. For which reaction,

Δ H > Δ U

? (

Δ H =

change in enthalpy,

Δ U =

change in internal energy )

Q. For gaseous reactions, if

Δ H

is the change in enthalpy and

Δ U

that in internal energy, then

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If true 1 else 0.

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A vessel contains 100 litres of a liquid x. Heat is supplied to the liquid in such a fashion that, Heat given = change in enthalpy. The volume of the liquid increases by 2 litres. If the external pressure is one atm, and 202.6 Joules of heat were supplied then, [ U - total internal energy ]

The correct option is D ∆U = 0, ∆H = + 202.6 J ΔH = heat gives so process is isobaric. w = −Pnext (ΔV) = −1 × 2 litre.atm = −202.6 J -as one litre.atm=101.33 joules Hence q = 202.6 J = ΔH and ΔE = q + w = 0

A vessel contains 100 litres of a liquid $x$ . Heat is supplied to the liquid in such a fashion that, Heat given = change in enthalpy. The volume of the liquid increases by 2 litres. If the external pressure is one atm, and 202.6 Joules of heat were supplied then, [ U - total internal energy ]

The correct option is D
∆U = 0, ∆H = + 202.6 J

$Δ H$ = heat gives so process is isobaric.

$w = - P_{n e x t} (Δ V) = - 1 \times 2 l i t r e . a t m = - 202.6 J$ -as one litre.atm=101.33 joules

Hence $q = 202.6 J = Δ H$ and $Δ E = q + w = 0$