In this experiment, you measured the thermal energy associated with an acid-base reaction or a reduction-oxidation reaction. To process your data, you would calculate the heat using q=mCs∆T to further find out the heat of the reaction performed. From that, using the # of moles and qrxn, you would find out the ∆Hrxn for the corresponding balanced chemical reactions performed.
In this assignment, you will need to submit (individually) a typed Word document answering the following post-lab summary questions. Use equation editor to input any calculations (instruction video below). Make sure to include an appropriate title, your name and section number at the top of the page.
-Choose one of the reactions performed by your group in this project. With the data you collected in the lab using the commercial calorimeter (one trial) and the coffee-cup calorimeter (one trial), fill in the following tables and answer the questions below. Make sure to include all the corresponding calculations and balanced chemical equation of the reaction you chose.
Table 1: Experimental Data for Reaction X using Commercial Calorimeter (3 points for data)
Table 2: Experimental Data for Reaction X using Coffee-cup Calorimeter (3 points for data)
1.Calculations for each trial using each type of calorimeter (5 points each, 10 points total)
2. How close is your experimental
Hrxn value to the theoretical value of the reaction chosen? (4 points)
3. Was your reaction an exothermic or endothermic reaction? Why? Does your data support your answer? (4 points)
4. Work the following problem. Show your calculations (6 points):
When 25.0 mL of 1.5 M H2SO4 (aq) and 50.0 mL of 2.0 M NaOH(aq), both at 25.0 °C are added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of 28.9 °C. What is the approximate amount of heat produced by this reaction? (𝐶𝑠 𝑜𝑓 𝑤𝑎𝑡𝑒𝑟 = 4.184 J/g
C) Assume the density of all solutions to be 1.0 g/mL.
H2SO4 + 2 NaOH → Na2SO4 + 2 H2O