Answer :
Explanation:
For the reaction.......
H
2
O
(
l
)
+
Δ
→
H
2
O
(
g
)
WHERE BOTH PRODUCT AND REACTANT ARE AT
100
∘
C
,
..........
Δ
H
∘
vaporization
=
40.66
⋅
k
J
⋅
m
o
l
−
1
And thus we need to assess the molar quantity of the water vaporized......
Δ
H
rxn
=
5.00
⋅
g
18.01
⋅
g
⋅
m
o
l
−
1
×
40.66
⋅
k
J
⋅
m
o
l
−
1
=11.3 kJ
For the reaction.......
H
2
O
(
l
)
+
Δ
→
H
2
O
(
g
)
WHERE BOTH PRODUCT AND REACTANT ARE AT
100
∘
C
,
..........
Δ
H
∘
vaporization
=
40.66
⋅
k
J
⋅
m
o
l
−
1
And thus we need to assess the molar quantity of the water vaporized......
Δ
H
rxn
=
5.00
⋅
g
18.01
⋅
g
⋅
m
o
l
−
1
×
40.66
⋅
k
J
⋅
m
o
l
−
1
=11.3 kJ
The energy is needed to evaporate 5 grams of water is 1670 kJ.
What is energy?
The energy is the ability to do work.
Energy required to change the phase of an object is mass times the latent heat of vaporization.
Q = mL
where, latent heat of vaporization L =334J/g
Given is the mass of water m =5g, then the energy needed will be
Q =5 x 334
Q =1670 kJ
Thus, the energy needed to evaporate water is 1670kJ.
Learn more about energy.
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