16.9. -1.10-2.30X 10³ J 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.AT S=1 cal/goc Trinal-Tinitid 26.00-23.00=35 26.00 °C? 000»04 ! T₁ = 23.00% 4, 1845/1.25521104 14618451 1.25 52×10²4 12=26.00°C Answer: 3.00 x 10³ cal (or 1.26 x 10¹J) I cal 1.36 × 1047 3% 1 Cal (3x) = 3.00×10 cal gºe 3.00x 10³ cal
16.9. -1.10-2.30X 10³ J 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.AT S=1 cal/goc Trinal-Tinitid 26.00-23.00=35 26.00 °C? 000»04 ! T₁ = 23.00% 4, 1845/1.25521104 14618451 1.25 52×10²4 12=26.00°C Answer: 3.00 x 10³ cal (or 1.26 x 10¹J) I cal 1.36 × 1047 3% 1 Cal (3x) = 3.00×10 cal gºe 3.00x 10³ cal
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.
Question
Can you help me with the number 5 questions? Also can you please show the step-by-step including the formula?
Transcribed Image Text:Calculations for Temperature and Phase Change Worksheet
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? Mass of ice = 100.0g
Heat of fusion of ice: 79.
100.0g|79.7.cal-1970 cal
2. How much energy is required to vaporize 234.5 g of water?
234.5g 540 cal-
-
1.224
1.2 cal/g
12 6630 1.2663X105
1.3x105
Answer: 1.3 x 105 cal
cal
3. If 30.6 calories are required to vaporize 25 g of a substance, what is the heat of vaporization of
that substance?
mass of substance: 25g
energy require vaporization: 30.6 Cal
may
30.6 cal
259
26.00 °C?
100c,05 (6બ (22)=xtel
3.00x 10³cal
4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 °C?
mass m) = 500.09
AT=-1.10°C
500.0g (ca.1000) = [
500.g (4.1845 -1.10 23.01.2-2,3012×10³.
-550 cal
5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 °C to
0.0924 cal
3-21) (100.024)
до с
m= 1000.09 Q=SOMIAT
S=1 cal/goc Teinal-Tinitid
T₁ = 23.00%
T2=26.00°C
3.00 x 10³ cal (or 1.26 x 10¹J)
is required to raise the
mass of copper: 100g
Specific heat copper: 0.0924cal/g °C
AT=100.0°C
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)?
= mxsx Delta + mass(m) = 786 gram
T₁ = 20.0%
T₂=35:0°C
-0.002171332 TFinal-Tinitial
0.00217
4184511.2552x10
Içal
6. The specific heat of copper is (0.0924 cal/g°C), how much energy
temperature of 10.0 g of copper by 100.0 °C?
10.09
Mass of water 234.59
Heat of vaporization: 540 cal/g
Heat of vaporization substance: 1.2 cal/g
Answer: 1.2 cal/g
25.65=786 gx sx35°C-20°c)
---5=25.6J
7869x
:79.7 cal/g
Answer: 7970 cal
15°C
Q==ssocal
Answer: -550. cal (or -2.30 x 10³ J)
92.4call
(2617X10³J/g °C
26.00-23.00=3%
Answer: 2.17 x 10-³J/g °C
35.0%-2010°C = 15.0°C
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