Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Can you help me number 4? Is this correct answer with show my work including the Significant Figures number?
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The heat of fusion of ice is 79.7 cal/g.
The heat of vaporization of water is 540 cal/g.
Report the answer using the correct number of significant figures!
1. How much energy is required to melt 100.0 grams of ice?
100.0 g 79.7 cal
·cal = 7970 cal
9
2. How much energy is required to vaporize 234.5 g of water?
1.2663 х 105
234.5g 540 cal
g
1.3X105cal
Answer: 1.3 x 105 cal
3. If 30.6 calories are required to vaporize 25 g of a substance, what is the heat of vaporization of
that substance?
30.6 cal
259
1.224
1.2 cal/g
Answer: 1.2 cal/g
4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 °C?
500.09
1 cal) (-1.10°C) = [550 cal
500.g
-2,3012×103
4.184J (-1.10) = √2.30×10³5
Answer: -550. cal (or -2.30 x 10³ J)
I cal
5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 °C to
M=1000.09 Q=S•m. (OT)
s=lcal/g °C
T1=23.00%
26.00 °C?
1000,03 (1Cal) (3°C) = 5+00X10³ cal
go c
1,2552x10
-1.26x1045
3,00x10³ cal 4.1845).
1461845-1-20
10.0924 cal
9°C
Answer: 7970 cal
1) (100.0°C) = 12,4 cal
6. The specific heat of copper is (0.0924 cal/g°C), how much energy is required to raise the
temperature of 10.0 g of copper by 100.0 °C?
10.09
T2= 26.00°C
Answer: 3.00 x 10³ cal (or 1.26 x 10¹J)
25,65=786g xs x (35°C -20°c)
5=25.65
2.171331637X10
(7869 x 15°C) (2.17X/10-3³5/9°C
Tfinal-Tinitial
26.00-23.00=3c
-3
Answer: 92.4 cal
7. If 25.6 J of energy raised 786 g of a substance from 20.0°C to 35.0°C, what is the specific heat of
the substance (S)?
Tfinal-Tinitial
35.0°C-20.0°= 15.00
Answer: 2.17 x 10-³J/g °C"
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Given: mass = 500 g
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