The latent heat of vaporisation of water is 2240 J. If the work done in the process of vaporization of 1 g is 168 J, then increase in internal energy will be

Question

The latent heat of vaporisation of water is 2240 J. If the work done in the process of vaporization of 1 g is 168 J, then increase in internal energy will be (A) 1904 J (B) 2072 J (C) 2240 J (D) 2408 J

Tardigrade Admin · Accepted Answer

From first law of thermodynamics, we have

Δ U = Q - W

Which states that if an amount of heat

Q

is given to a system, a part of it will be used in increasing the internal energy

(Δ U)

of the system and the rest in doing work

(W)

∴

We have

Q = M L = 1 \times 2240 J

and

W = 168 J

∴ Δ U = 2240 - 168 = 2072 J

Q. The latent heat of vaporisation of water is $2240 J$ . If the work done in the process of vaporization of $1 g$ is $168 J$ , then increase in internal energy will be

$1904 J$

$2072 J$

$2240 J$

$2408 J$

Q. The latent heat of vaporisation of water is 2240J. If the work done in the process of vaporization of 1g is 168J, then increase in internal energy will be

1904J

2072J

2240J

2408J

From first law of thermodynamics, we have ΔU=Q−W Which states that if an amount of heat Q is given to a system, a part of it will be used in increasing the internal energy (ΔU) of the system and the rest in doing work (W) ∴ We have Q=ML=1×2240J and W=168J ∴ΔU=2240−168=2072J

Q. The latent heat of vaporisation of water is $2240 J$ . If the work done in the process of vaporization of $1 g$ is $168 J$ , then increase in internal energy will be

$1904 J$

$2072 J$

$2240 J$

$2408 J$