I can provide the video and the lab manual. 

Raw Data

Element Mass (g) Element

Tinitial (°C) Tfinal (°C
)

Water

Tinitial (°C) Tfinal (°C
)

Iron 10.93 g
99.7 C

25.9 C 24.1 C 25.9 C

Cadmium 31.34 g 98.9 C

27.2 C

24.2 C

27.2 C

Tin 8.29 g 99.8 C

25.8 C

24.1 C

25.8 C

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Lab Report 7

General Chemistry I (California State University Los Angeles)

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Lab Report 7
General Chemistry I (California State University Los Angeles)

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Experiment 5: Heat and Temperature. The Law of Dulong and Petit

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Purpose:

The purpose of this experiment is to calculate the specific heat of a substance by using a mercury

in glass thermometer to measure the temperature changes when a known amount of a pure

substance is placed in water.

Theory/ Principles:

We are told that heat is a form of energy and specific heat is an amount of energy required to

raise the temperature of a substance. While the heat capacity allows us to calculate how much

energy is required to increase or decrease temperature for a sample by a temperature change. For

our experiment in order to calculate the specific heat of my substances (Al, Fe, Zn) we will first

need to calibrate our thermometer in order to gain the accuracy of our measurements and to

move on to our procedures. To gain accuracy for our work the readings must be compared to two

convenient standards of temperature which are the freezing and steam points of water on the

Centigrade scale. Before determining the specific heat of a substance we would need to calculate

our true steam and the true temperature by using the formula Ttrue=(Ttrue steam-0/Tsteam-

Tice)Texp+Tice. Then to find our specific heat of our substances we would need the equation of

S=mw(4.184 J/g * K )(Tf – Ti)/mel (Th-Tf). We would also need to find the atomic heat by

C=AW(S), the average error, the percent error, and the average atomic heat.

Experimental Procedures:

Goldwhite, H.; Tikkanen, W. Experiment 5. Heat and Temperature. The Law of Dulong and

Petit, Experiments in General Chemistry, 4th ed.;The McGraw Hill Companies. (35-39)

Data Tables/ Summary:

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– Table 1: Raw signed data of my measurements for calibrating the thermometer during

ice and steam point until their endpoints / measurements for initial and final temperatures

for my substances of Al, Fe, and Zn/ pressure of mercury

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– Table 2: Formatted table from my measurements above of Ice and Steam points

– Table 3: Formatted raw date for my measurements of initial/ final temperatures for Al,

Fe, and Zn, including the pressure of mercury

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– Table 4: Mass of Elements used for experiment

Mass of Zinc (g) Mass of Iron (g) Mass of Aluminum (g)

10.71 g 10.75 g 2.25 g

Results and Discussion:

Sample Calculations:

– True steam= 100°C + (754 mmHg) x 0.37°C/ 10 mmHg= 128. °C

– True= (128. °C – 0°C/ 99.3 °C- (-0.2°C))0.1°C + (-0.2°C)= -12.82 °C

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– Al (specific heat) 1st run: S=50g(4.184 j/g*k)(21.8°C-23°C)/2.25 g(21.1°C-21.8°C)=

159.3 J/g*k

2nd Round: S= 116.3 J/g*k

Average specific heat: 137.75 J/g*k

Average error: 2 J/g*k

% error: 0.900 J/g*k- 137.75 J/g*k/137.75 J/g*k x 100= -99%

Atomic Heat (1st Run): C=26.9 g(159.3 J/g*k)= 4285.17 J/k  2.58 x 10^30 J/mol*k

2nd Run: C= 1.88 x 10^30 J/mol*k

Average atomic heat: 2.23×10^30 J/mol*k

– Zn (specific heat) 1st run: S=50g(4.184 j/g*k)(22.4°C-23°C)/10.71 g(21.1°C-22.4°C)=

9.01 J/g*k

2nd run: 2.79 J/g*k

Average specific heat: 5.9 J/g*k

Average error: 9.48 J/g*k

% error: 0.39 J/g*k- 5.9 J/g*k/5.9J/g*k x 100= -93 %

Atomic Heat (1st Run): C= 65.38 g(9.01 J/g*k)=589.07 J/k 3.54 x 10^29 J/mol*k

2nd run: C= 1.098 x 10^29 J/mol*k

Average atomic heat: 2.31×10^29 J/mol*k

– Fe (specific heat) 1st run: S=50g(4.184 j/g*k)(22.2°C-23°C)/10.75 g(21.2°C-22.2°C)=

15.56 J/g*k

2nd run: 4.49 J/g*k

Average specific heat: 10.02 J/g*k

Average error: 2.0 J/g*k

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% error: 0.450 J/g*k- 10.02J/g*k/10.02 J/g*k x 100= -55%

Atomic Heat (1st Run): C= 55.8 g (15.56 J/g*k)= 868 J/k  5.22 x 10^29 J/mol * k

2nd run: C= 1.589 x 10^29 J/mol* k

Average atomic heat: 3.40 x 10^29 J/mol* k

Logical Explanation:

The law of Dulong and Petit state that the product of a specific heat from a solid element and its

mass per mole is always constant. In this experiment in order to determine our specific heat per

element (Al, Fe, Zn) we had to calibrate our thermometer by ice and steam point till its endpoint

temperature is constant. Calibrating our thermometer assisted in gaining accurate measurements

when it came to finding the specific heat of our substances. Besides gaining initial and final

temperature for each element twice we are to gain their masses. We are told before calculating

the specific heat for each element that the initial temperature of our element Th and the final

temperature of the element is the same as the water Tf. Taking this in consideration I was able to

determine the specific heat for each element for each run and calculate the overall average of

specific heat. The two specific heats I found for Al were 159.3 J/g*k and 116.2 J/g*k and its

overall average is 137.75 J/g*k. For Zn its specific heats were 9.01 J/g*k and 2.79 J/g*k and

overall average is 5.9 J/g*k. Finally, for Fe its specific heats were 15.56 J/g*k and 4.49 J/g*k ad

overall average is 10.02 J/g*k.

Discussion Ques:

1. Melting point of Glauber’s salt in our thermometer would be: 884 °C

2. Atomic heat= atomic weight x specific heat

Metal Specific Heat Atomic Mass Atomic Heat (kJ)

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Ba 0.2044 137.3 28.06

Be 1.824 9.01 16.43

Cu 0.3845 63.5 24.41

C 0.71 12 8.52

I 0.214 126.9 27.15

S 0.71 32 22.72

3. a) C=0.38 J/gC Cu(s) +xCl2(g)  CuClx

m=0.5007 g

m=1.0586 g

MW (Cl)= 35.5 g/mol

MW of metal= ?

1.0586g-0.5007g= 0.5579 g Cl

Mol of Cl2= 0.5579g/35.5 g/mol= 0.015715 mol

MW (Cu)= 63.5 g/mol

Mol of Cu= 0.5007g/63.5 g/mol= 0.00787 mol

b) Color of the chloride would be green and bluish color.

4. Uncertainty would be given by the formula (0.5 ml/50 ml + 0.05 + 2°C/ S H20°C +

0.10°C/Sele + 0.005g/ mele g + 0.5 mmHg/754 mmHg) x 100 %

Al= 3.75 %

Fe=4.49 %

Zn= 5.19 %

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Conclusions:

By calibrating our thermometer by the two given standards of ice and steam point we were able

to gain our measurements with accuracy. From here we are able to move on to the next

procedure in finding our initial and final temperature for each of our elements used in this

experiment to later on using this information to assist in determining each of their specific heats.

References:

Goldwhite, H.; Tikkanen, W. Experiment 5. Heat and Temperature. The Law of Dulong and
Petit, Experiments in General Chemistry, 4th ed.;The McGraw Hill Companies. (35-39)
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