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2025-2026 (CHEM 103) LAB REPORT 4 | PORTAGE LEARNING| GRADED A+, Exams of Chemistry

University of Illinois - Urbana-ChampaignChemistry

2025-2026 (CHEM 103) LAB REPORT 4 | PORTAGE LEARNING| GRADED A+

Typology: Exams

2024/2025

Available from 05/08/2025

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2025-2026 (CHEM 103) LAB REPORT 4 | PORTAGE
LEARNING| GRADED A+
Chemistry Lab
Report
May 10, 2025
Experiment # 4
Title: Thermochemistry
Purpose:
Through the acid-base experiment, we can determine the heat of the reaction, or ΔH. We can
also measure how much heat it takes to raise 500 grams of water by 15 degrees Celsius through
the heat of combustion of a hydrocarbon fuel.
Procedure:
Acid Base Experiment:
NaOH + HCl → NaCl + H₂O
H=? Salt water is being formed
Determine the weight (Calorimeterer)
1. Grab a vessel to measure, a calorimeter (refered to as coffee cup calorimeter) or use a
styrofoam cup with good insulation and a cardboard lid that doesn't need to be super
insulated at the top .
2. Mix solution of sodium hydroxide and NaCl and kmeasure temperature change ,
Acid base reaction will result in heat (exothermic)
3. First we need to determine the heat capacity of the calorimeter. We need to figure out
how much heat the calorimeter will absorb(FYI no calorimeter is perfect inc the
container used).
4. 1st sample-Pour 50 mL of tap room temp water into the calorimeter,Place
thermometer with stopper so it can stay in place.
5. 2nd sample Take another 50 mL of water cup and put in a water bath and set at 40
degrees. Let sit for 5 minutes. Pull out the warm water and put the temperature gauge
in to warm up the water.
6. Set 22 .8 degrees of tap water in the calorimeter and the warm water set in
water bath temperature is now 38 degrees.
7. Now pour 50 mL of warm water (what was in the water bath) to 50 mL of tap water(
what was in the carlorimeter). Every 15 seconds take a temperature reading and do
the calculations. (See chart)
Completing Reaction Acid Base Experiment-Determine the the change in energy:
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Download 2025-2026 (CHEM 103) LAB REPORT 4 | PORTAGE LEARNING| GRADED A+ and more Exams Chemistry in PDF only on Docsity!

2025 - 2026 (CHEM 103) LAB REPORT 4 | PORTAGE

LEARNING| GRADED A+

Chemistry Lab Report May 10, 2025 Experiment # 4 Title: Thermochemistry Purpose: Through the acid-base experiment, we can determine the heat of the reaction, or ΔH. We can also measure how much heat it takes to raise 500 grams of water by 15 degrees Celsius through the heat of combustion of a hydrocarbon fuel. Procedure: Acid Base Experiment: NaOH + HCl → NaCl + H₂O ⃤ H=? Salt water is being formed Determine the weight (Calorimeterer)

  1. Grab a vessel to measure, a calorimeter (refered to as coffee cup calorimeter) or use a styrofoam cup with good insulation and a cardboard lid that doesn't need to be super insulated at the top.
  2. Mix solution of sodium hydroxide and NaCl and kmeasure temperature change , Acid base reaction will result in heat (exothermic)
  3. First we need to determine the heat capacity of the calorimeter. We need to figure out how much heat the calorimeter will absorb(FYI no calorimeter is perfect inc the container used).
  4. 1st sample-Pour 50 mL of tap room temp water into the calorimeter,Place thermometer with stopper so it can stay in place.
  5. 2nd sample Take another 50 mL of water cup and put in a water bath and set at 40 degrees. Let sit for 5 minutes. Pull out the warm water and put the temperature gauge in to warm up the water.
  6. Set 22 .8 degrees of tap water in the calorimeter and the warm water set in water bath temperature is now 38 degrees.
  7. Now pour 50 mL of warm water (what was in the water bath) to 50 mL of tap water( what was in the carlorimeter). Every 15 seconds take a temperature reading and do the calculations. (See chart) Completing Reaction Acid Base Experiment-Determine the the change in energy:

NaOH + HCl yields NaCl + H2O, Mix in calorimeterer and check temperature. Calorimeter is cleaned out and dried.

  1. Pour 50 mL of HCL into the calorimeter and monitor temperature for 1 minute
  2. Insert themoemter into cylinder with NaOH and measure for 1 minute
  3. Initial temperature of calorimeter is almost 22.8 ° C
  4. Initial temperature of NaOh is alsomost 22.4 ° C
  5. These need to be within .5 degrees, wait for 3 minutes and once they are at the same temperature mic them and record the temperature every 15 seconds.
  6. Temperature rises from 22.8° C to 28.0° C Continue to record, (See Chart) Heat of Combustion of Hyrdrocarbon Fuel: C4H10O3(Diethylene glycol) + 5O2 - > 4 CO2 (carbondioxide) + 5H2O(water vapor) HO - CH2 - CH2- O - CH2-Ch2-OH Fuel Value= 6020cal/g (This calorie is not the same as food, food calorie is kilocalorie or with Cal)
  7. Use a fuel source on the bottom of the ring stand with a copper pan above ( Copper conducts heat very well) , put water in and add a thermometer to measure temperature.
  8. Measure the mass of the fuel before burning (the total initial mass = 203.2382 grams)
  9. Measure out 500 mL of water and pour that water into the copper bowl, cover it and then sit the thermometer in.
  10. Water should have been at room temperature at thatpoint but then check to make sure the temperature is stabilized , the initial temperature is 21.4 degrees celsius.
  11. Cover and stopper is put on, light the fuel positions far enough away that it isn’t smothered, causing black smokes but close enough to heat up the water.
  12. Stir occasionally. When the temperature has reached 36 degrees celsius we put out the flame and cover the heat source. Stir the water and make sure it is well mixd to get out the final temperature.
  13. The final temperaure should be 37.2 degrees celsius and then measure the mass of the heat source which the final mass hsould be 2002244 grams. Do the calculations. Data/Results/Calculations: Part 1:Heat capacity of calorimeter

calorimeter. Part 2: Acid Base Reaction ● Initial temperature of HCl + calorimeter: 22.8 C ● Highest temperature : 28.6° C and then slowly receded and stayed at 28.4 ° C ● △ T =5.8° C(or K) is the overall change in difference ● Heat gained by solution : 5.8 K x 100 g x 4.18 J/K-G = 2424.4 J (amount gained by solution)

  • 4.18 J/K-G is the value for water
  • 100 g( this number if from the 50mL from both sources) ● Heat gained by calorimeter: 5.8 K x 13.9 J/K=80.6 J (Calorimeter absorbs a little heat) ● 2424.4 + 80.6 = 2505 Jules (total heat given by reaction of NaOH and HCI) Now figure out Kilojoules per Mole: 0.050 L HCI x 1.0 mol HCI/1 L x 1 mol H₂O/1 mol HCL= 0.050 mol H₂O ● Convert above to a product in order to get heat per mole of a product ● Reaction will always want to be in terms of a production of a product ● This reaction has a 1 - 1 relationship 2505 J÷ 0.050 mol= 50, 100 J/ mol or 50.10 kilojules/mol This is the emphylIP of the reaction and it is exothermic with negative value ● This compares to the accepted valye of 56.2 Joules per mole (which is a 12% error) and using the emphylP of reaction for this acid base reaction.

Part 3 Heat Combustion Fuel Initial 203.2383 grams Final mass 200.2244 grams How much was used? 3.0138 grams Water Initial: 21.4 ° C Final Temperature: 37.2° C △ T =15.8 ° C temp change Copper pan is 218.87 grams 500 mL x 1g/1mL (density of water is one gram /per mililiter) 500mL x 1g/1mL @ 24C= 500g which is the mass of the water that we are using. Because density of water is 1 - 1 it makes it easy to know the conversions and this will be used in the change of heat formula. The heat is transferred from the fuel into water and copper pan; measuring the differenc ein the mass of the fuel but the heat that we measure we will assume that it is all being transferred int o the water in the copper pan. Change in heat △q=M(mass) C (Heat capacity) △T (change in temp) △ q=(500 g x 1.00 cal/g - C) + (copper pan 218.87 grams x acc. Val 0.092 Cal/g C) x 15.8°C (change in temp)

Example reaction (exothermic): Methane reacts with oxygen combustion reactions to produce CO₂ and water. CH₄(g) + 2O₂(g) → CO₂ (g) + 2H₂O (i) ⃤ H = - 212.8Kcal Exothermic Reaction (heat given off for every mole, negative sign shows heat given off) In thermochemical reactions, the heat change is added onto the reaction that is represented by Delta H (enthalPY) and it is added to the end of the reaction and gives us a heat value. For every 1 mole of Ch4 that burns we get a (The change in enthalPY) - 212.8 Kcal (Extensive) Is we double this and go 2mol CH4= we would double - 425.6 Kcal Extensive Property of chemical reactions meaning it depends on the amount ● Not all properties are extensive, some are intensive ● An example of this is density-density of water is the same if you have a few drops or a lot of it, the density is the same (intensive property) Reactions give off heat in one direction and can pick up heat in another direction Example Reaction (Endothermic): Calcium carbonate is heated and broken downas calcium oxide as well as CO₂ given off CaCO₃ → CaO + CO₂ ⃤H=+42. Kcal Delta H is +42.4 Kilo Calories

  • Positive Value of Delta H means that it is an endothermic reaction because energy needs to be put in to make this react
  • Positive means energy needs to go in to make the calcium carbonate break into calcium oxide and CO₂ so they are different If in reverse, CaO + CO₂ → CaCO₃ ⃤= - 42.4 Kcal if taken in the same direction but writein opposite direction to produce calcium carbonate, then the same energy change will happn but with opposite sign because it is going in opposite direction.
    • The opposite would be exothermic because the heat is given off
      • sign means energy needs to be added to the direction (feels cold) (endothermic)
    • sign means energy is given off (feels hot) which is exothermic Chemical ice packs break the components and it will cause a reaction of endothermic and it will feel cold