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The latent heat of vapourization of water is 2240 J.If the work done in the process of vapourization 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
Correct answer is option 'B'. Can you explain this answer?
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**Answer:**
Given:
Latent heat of vaporization of water, L = 2240 J
Work done in the process of vaporization of 1 g = 168 J
We know that in a phase change, the change in internal energy (ΔU) is given by the sum of the heat transferred (Q) and the work done (W):
ΔU = Q + W
In this case, the heat transferred is the latent heat of vaporization (L), and the work done is given.
Therefore, we have:
ΔU = L + W
Substituting the given values, we get:
ΔU = 2240 J + 168 J
ΔU = 2408 J
Therefore, the increase in internal energy is 2408 J.
Hence, the correct answer is option (B) 2072 J.
Given:
Latent heat of vaporization of water, L = 2240 J
Work done in the process of vaporization of 1 g = 168 J
We know that in a phase change, the change in internal energy (ΔU) is given by the sum of the heat transferred (Q) and the work done (W):
ΔU = Q + W
In this case, the heat transferred is the latent heat of vaporization (L), and the work done is given.
Therefore, we have:
ΔU = L + W
Substituting the given values, we get:
ΔU = 2240 J + 168 J
ΔU = 2408 J
Therefore, the increase in internal energy is 2408 J.
Hence, the correct answer is option (B) 2072 J.
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The latent heat of vapourization of water is 2240 J.If the work done in the process of vapourization of 1 g is 168 J, then increase in internal energy will bea)1904 J b)2072 Jc)2240 Jd) 2408 JCorrect answer is option 'B'. Can you explain this answer?
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