The assumption is Originally at 20°C
Now
We need ∆T
- Q=mc∆T
- 1=1(0.108)∆T
- 0.108∆T=1
- ∆T=1/0.108=9.26°C
Now
- ∆T=T_f-20
- 9.26=T_f-20
- T_f=29.26°C
Option A
a
We should change it to mol and then ×Number of Avogadro
The heat released from the calculation is 33.56 kJ.
<h3>Heat of vaporization</h3>
The heat of vaporization is the heat absorbed when a substance changes from liquid to vapor. It is equal to the heat released when the vapor is condensed.
The total heat released = Heat of condensation + Heat lost to the skin
= (13.3 g × 2260 J/g) + (13.3 g × 4.18 J/g/°C × ( 100 - 37)°C)
= 30058 + 3502
= 33.56 kJ
The heat released from the calculation is 33.56 kJ.
Learn more about heat of vaporization: brainly.com/question/2427061
