CHEM110L UCSB General Engineering Chemistry Experiments Lab Report please read the attachments before writing the report.
Read the instructions that we followed for lab experiment to know the tools we used and the chemicals.
Also read the attached slides which is also about the three simple experiment we did, it will help.
Report sheets for the three experiments are attached which include all the data that we collected for this lab report.
Report Style: ( the lap reprt should include 1. Heat of solution of salt 2. Heat capacity of calorimeter 3. Heat capacity of a metal.) (report should include the three experiment)
1-Cover Page (50 points)
2-Introduction (50 points) (should include what is the lab about, how the report will cover the experiment. General information about the three simple experiment)
3- Typed data and observations (400 points) (should include all the data attached as report sheets with further information like what you think of the reactions and how we got these numbers. Also, pictures while doing the experiments will be attached)
4- What’s Up (200 points) (how can we involve these three experiments in our daily life in engineering) ( a real life example for each one)
5-Conclusion (100 points) (explanation of the three experiments and what you learn from these experiments and what you think) (explosions of how you thing the data are, and explain what error occurred in the experiments if)
(More pictures will be attached for during the experiment)
(Example of the complete work will be attached)
(There will be a plagiarism check)
More information will be attached to write the rep 15
Date
Exp. No.
Name
Lab Partner
Locker/
Desk No.
Course &
Section No.
5.00 g
Sioo
45 mlig
50
25 C
18 °C
ExperimenvSubject The ealme: vist at everyy
6
• O.S
DA
Heat of solution na salt
Call ,
NH4 Cl
a. Grams of sales
-g
g
Ba Milliliter (grams) afuator in Cup 95 mLeg
C. Grams of solution (20+2b)
50
32 18
-g
d. Find the tampretmen Saution
e. Initial Temperture of water
°C 25°C
Fo Temperature Change
Z-
C
С
go Totul Calories of haut
Chergy
cal
cal
elelveted evolved or ceh,somhed
(show the calculation)
h. Was the preess exothermic or
exothermic endothrinic
endotherimic?
1. Heat at solution per gram
of
salt (2g/2a); indicate
(+)
whether chsorbed (4) arte erdved –*–caly)
cally
.-Z-
(-)
1.
GA
3100
Witness/TA
Date
Date
Signature
Note: Insert Divider Under Copy Sheet Before Writing
THE HAYDEN-MCNEIL STUDENT LAB NOTEBOOK
16
Date
Lab Partner
Locker/
Desk No.
Course &
Section No.
Experiment Subject Het capacity of calorimeter
Katana
OA
(Heat coperty of calorimeter)
50.0 ml of water at 65° is added to a calorimeter
Cantanig 500mL of water at After wating for the
system to equilibrate, The Firel Temp reach is 35 C
Calculation the heat capacity of calorimeter
ra that
ra
35C – 65 C = -30C
= 4.18 4 Jlgxi
Sp-heat of water
& At cold
35c-1°C
24 cl
* 9 cold
That masp- heat & At
(50g) X(4-184J1gxC) x&#ZE)(-300) = -6276J
(50g (4.184 J/gxC)( 24 ) = 50 20.83
By rearranging the g equation, qhot = -(qcold-qcal),
* acal
we solve for a cal
*
q hat – q cold
5020-8262767 –
6276J – 5020.8 +1255.2J
Heat capacity of the calorimeter Ccal
Renewper the calorimeter Includes the Im.Og of water
So we must include the heat cepaty of the much water.
Coal = 532
1255-23 +4.184 fly
xCx100g
24°C
2
Date
Witness/TA
Date
Signature
Note: Insert Divider Under Copy Sheet Before Writing
THE HAYDEN-MCNEIL STUDENT LAB NOTEBOOK
EXPERIMENT #7: CALORIMETRY IN A COFFEE CUP
Purpose:
The purpose of this experiment is to measure, using a “coffee cup” calorimeter, the enthalpy of reaction for two acid-base reactions and show that Hess’s Law of Heat Summation holds true, measure the enthalpy of
dissolution for calcium chloride, and measure the heat capacity for a metal.
Special Apparatus:
2 Styrofoam cups
Plastic lid
Thermometer
Discussion:
Chemical reactions and processes may produce or absorb heat when they occur. For example when methane (a major component of natural gas) burns, heat is produced. As you may guess, it is of major importance to the
chemist whether heat is absorbed or produced by a particular reaction and how much heat is produced or absorbed for a given amount of material. The study of heat transfer during chemical reactions is called
thermochemistry.
Heat is defined as the energy that flows into or out of a system. Typically we are examining reactions occurring open to the atmosphere (and therefore at a constant pressure); we refer to the heat exchanged at constant
pressure as the change in enthalpy, delta H. Thermodynamically, the system is defined as the substance or substances that we are studying in which a change occurs. For chemical reactions, the system is generally the
chemicals involved in the reaction. The system is in contrast with the surroundings which is everything else in the neighborhood of the system; this includes water of solution.
The standard SI unit for energy (and therefore heat) is the joule (J) and is defined as one Newton of force acting over the distance of one meter or:
1 Joule =(kg-m-/s2)
Another commonly used unit of heat energy is the calorie (cal) which was originally defined
as the amount of heat needed to raise the temperature of 1 gram of water by 1 degree Celsius. The calorie is now defined in terms of the joule:
1 calorie = 4.184joules (exact)
Exp. No.
Experiment/Subject
Name
Lab Partner
Locker/
Desk No.
Course &
Section No.
TE (from graph)
Iso sea
((Heat capacity of Ajmetal)
offen metal) (Time)
Mass of metal g(9.8) 80 – 9
30 sec
turtial T of metalqoc) 80
60 sec
Maess of water (53.99, -180 ។
90 sec
Initial T of water 60 80
120 sec
20
– T
change for water 8011
180 sec
– Heat capacity of water (572) TO F-32 (a)=2
Heat
gated by water (J)
4T =80-21.1=58.9
gained
– Tchange for metall C) 80-90 = -10°C
spesific heat of metal (J1g.)
4.184
3
GO
Socha
Date
Witness/TA
Date
Signature
Note: Insert Divider Under Copy Sheet Before Writing
THE HAYDEN-MCNEIL STUDENT LAB NOTEBOOK
When using calories be careful to distinguish between Calories with a capital C and calories with a small c. One food Calorie is equal to 1000 calories.
When we examine the amount of heat produced or absorbed during a reaction we refer to the heat of reaction (enthalpy of reaction if the change in the system occurs at constant pressure). The heat of reaction is the
amount of heat needed to return a system to a given temperature after the reaction is complete. A reaction that produces heat has a negative heat of reaction and is called exothermic and a reaction that absorbs heat has a
positive heat of reaction and is called endothermic.
In writing a thermochemical equation the enthalpy of reaction is written kJ per mole of equation and the physical states of the substances and amounts involved must be clearly stated. Enthalpies of reaction must be
determined by experimental measurement or determined by using other known experimental values.
To determine experimentally the amount of heat absorbed or produced during a chemical reaction, we use a device called a calorimeter (meter = “to measure” and calori = “calories”). For this experiment we will use a
“coffee cup” calorimeter which consists of two nested polystyrene coffee cups and a thermometer. See diagram. We determine the amount of heat exchanged in a process by measuring changes in temperature for the
immediate surroundings which are insulated from the rest of the universe. In our experiment the polystyrene coffee cups act as an insulated container to keep all heat energy in the solution in the cups. Because the cups are
open to the atmosphere, any reaction carried out in the cups is done at constant pressure and the amount of heat exchanged will be the enthalpy change, delta H.
In order to determine how much heat is exchanged based on a temperature Anange, we must also know the heat capacity of the material for which we are measuring the change in temperature. The amount of heat exchanged
is equal to the heat capacity of the material times the change in temperature:
where q is the heat exchanged, C is the heat capacity, and delta T is the temperature change.
Specific heat capacity values C, (heat capacity per gram) or molar heat capacity values Cm (heat capacity per mole) for a variety of substances can be found in standard handbooks, for example the CRC Handbook of
Chemistry and Physics. Remember, when using specific heat or molar heat capacities you have to take into account how much of the material you have.
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